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Title: Acids, Alkalis and Salts
Author: Adlam, George Henry Joseph
Language: English
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                COMMON COMMODITIES AND INDUSTRIES SERIES

 Each book in crown 8vo, cloth, with many illustrations, charts, etc.,
                                2/6 net


  TEA. By A. Ibbetson
  COFFEE. By B. B. Keable
  SUGAR. By Geo. Martineau, C.B.
  OILS. By C. Ainsworth Mitchell, B.A., F.I.C.
  WHEAT. By Andrew Millar
  RUBBER. By C. Beadle and H. P. Stevens, M.A., Ph.D., F.I.C.
  IRON AND STEEL. By C. Hood
  COPPER. By H. K. Picard
  COAL. By Francis H. Wilson, M.Inst., M.E.
  TIMBER. By W. Bullock
  COTTON. By R. J. Peake
  SILK. By Luther Hooper
  WOOL. By J. A. Hunter
  LINEN. By Alfred S. Moore
  TOBACCO. By A. E. Tanner
  LEATHER. By K. J. Adcock
  KNITTED FABRICS. By J. Chamberlain and J. H. Quilter
  CLAYS. By Alfred B. Searle
  PAPER. By Harry A. Maddox
  SOAP. By William A. Simmons, B.Sc. (Lond.), F.C.S.
  THE MOTOR INDUSTRY. By Horace Wyatt, B.A.
  GLASS AND GLASS MAKING. By Percival Marson
  GUMS AND RESINS. By E. J. Parry, B.Sc., F.I.C., F.C.S.
  THE BOOT AND SHOE INDUSTRY. By J. S. Harding
  GAS AND GAS MAKING. By W. H. Y. Webber
  FURNITURE. By H. E. Binstead
  COAL TAR. By A. R. Warnes
  PETROLEUM. By A. Lidgett
  SALT. By A. F. Calvert
  ZINC. By T. E. Lones, M.A., LL.D., B.Sc.
  PHOTOGRAPHY. By Wm. Gamble
  ASBESTOS. By A. Leonard Summers
  SILVER. By Benjamin White
  CARPETS. By Reginald S. Brinton
  PAINTS AND VARNISHES. By A. S. Jennings
  CORDAGE AND CORDAGE HEMP AND FIBRES. By T. Woodhouse and P. Kilgour
  ACIDS AND ALKALIS. By G. H. J. Adlam


                        _OTHERS IN PREPARATION_

    [Illustration: _Copyright by Messrs Flatters & Garnett, Manchester_
    BACTERIA NODULES ON THE ROOT OF LUPIN]

               PITMAN’S COMMON COMMODITIES AND INDUSTRIES



                        ACIDS, ALKALIS AND SALTS


                                   BY
                            G. H. J. ADLAM,
                          M.A., B.Sc., F.C.S.
                 Editor of “The School Science Review”

                                 London
          Sir Isaac Pitman & Sons, Ltd., 1 Amen Corner, E.C.4
                      Bath, Melbourne and New York

 Printed by Sir Isaac Pitman & Sons, Ltd., London, Bath, Melbourne and
                                New York



                                PREFACE


It has often been said, and still more often implied, that
considerations of utility in education are incompatible with its main
object, which is the training of the mind. Extremely divergent views
have been expressed on this point. Schoolmen have looked askance at some
branches of knowledge because they were supposed to be tainted with the
possibility of usefulness in after life. On the other hand, business men
and others have complained bitterly of the present state of education
because very little that is considered “useful” has up to the present
been taught in schools.

It is possible to err in both directions. A university professor,
lecturing on higher Mathematics, is reported to have told his audience
that it was a source of great satisfaction to him that the theorem which
he was demonstrating could never be applied to anything “useful.” On the
other hand, we have the well-authenticated story of the man who took his
son to the Royal School of Mines to “learn copper,” and not to waste his
time over other parts of Chemistry, because “they would be of no use to
him.”

For narrowness of outlook, there is nothing to choose between the pedant
and the “practical” man. National education would deteriorate if its
control should ever pass into the hands of extremists of either type,
for nothing worthy of the name of education could ever be given or
received in such an irrational spirit.

In dealing with the subject of “Acids, Alkalis, and Salts,” I have
endeavoured to give prominence to the commercial and domestic importance
of the substances dealt with. I thereby hope to gain the interest of the
reader, since interest stands in the same relation to education that
petrol does to the motor-car. It is not education itself, but it is the
source of its motive power. I have also included some considerations of
a theoretical nature which may well be taken as a first step towards the
continuation of the study of Chemistry.

My sincere thanks are offered to my colleagues, F. W. G. Foat, M.A.,
D.Litt., and Mr. I. S. Scarf, F.I.C., for much valuable help and advice;
to Sir Edward Thorpe, C.B., F.R.S., and Messrs. William Collins & Sons
for permission to reproduce Figures 3, 11, and 14; to Messrs. Longmans &
Co. for Figures 4, 5, 9, 12, 13, 16; Messrs. Macmillan & Co., for
Figures 8, 10 and 15. I have also availed myself of the assistance of
several standard works on Chemistry. My acknowledgments in this
direction take the practical form of the short bibliography which
follows—


  Lunge, Dr. G.
    _The Manufacture of Sulphuric Acid and Alkali._ Vols. I, II, and
          III.
  Roscoe & Schorlemmer
    _Treatise on Chemistry._
      Vol. I. The Non-metallic Elements (1911).
      Vol. II. The Metals (1913).
  Brannt, W. T.
    _The Manufacture of Vinegar and Acetates._
  Thorp, F. H.
    _Outlines of Industrial Chemistry_ (1913).
  Thorpe, T. E.
    _A Manual of Inorganic Chemistry._
  Newth, G. S.
    _A Text-book of Inorganic Chemistry._
  Mellor, J. W.
    _Modern Inorganic Chemistry._
  Cohen, J. B.
    _Theoretical Organic Chemistry._


                                                             G. H. J. A.


    City of London School, E.C.



                                CONTENTS


  CHAP.                                                              PAGE
   PREFACE                                                              v
  I. INTRODUCTION                                                       1
  II. SULPHURIC ACID AND SULPHATES                                     10
  III. NITRIC ACID AND NITRATES                                        28
  IV. THE HALOGEN ACIDS                                                43
  V. CARBONIC ACID AND CARBONATES                                      49
  VI. PHOSPHORIC, BORIC, AND SILICIC ACIDS                             56
  VII. ORGANIC ACIDS                                                   67
  VIII. MILD ALKALI                                                    80
  IX. CAUSTIC ALKALIS                                                  95
  X. ELECTROLYTIC METHODS                                             101
   INDEX                                                              109



                             ILLUSTRATIONS


  FIG.                                                               PAGE
  BACTERIA NODULES ON THE ROOT OF LUPIN                    _Frontispiece_
  1. DIAGRAM                                                            7
  2. PLAN OF SULPHURIC ACID WORKS                                      13
  3. GENERAL VIEW OF SULPHURIC ACID WORKS                              15
  4. SULPHUR TRIOXIDE—THE CONTACT PROCESS                              19
  5. PREPARATION OF NITRIC ACID                                        30
  6. NITROGEN CYCLE (DIAGRAM)                                          38
  7. NITRIC ACID FROM AIR (DIAGRAM)                                    41
  8. PREPARATION OF HYDROCHLORIC ACID                                  45
  9. BORIC ACID                                                        59
  10. QUICK VINEGAR PROCESS                                            71
  11. DUTCH PROCESS FOR WHITE LEAD                                     74
  12. SALT CAKE FURNACE                                                83
  13. BLACK ASH FURNACE                                                85
  14. THE SOLVAY PROCESS                                               89
  15. THE ELECTROLYSIS OF SALT SOLUTION                               102
  16. THE CASTNER PROCESS                                             105



                        ACIDS, ALKALIS, AND SALTS



                               CHAPTER I
                              INTRODUCTION


Acids. A vague hint from Nature gave mankind the first indication of the
existence of acids. The juice pressed from ripe grapes is a sweetish
liquid. If it is kept for some time, the sweetness goes, and the liquid
acquires a burning taste. If kept still longer, the burning taste is
lost, and in its place a sharp acid flavour, not entirely displeasing to
the palate, is developed. The liquid obtained in this way is now called
wine vinegar; the particular substance which gives it its characteristic
taste is acetic acid.

The strongest vinegar does not contain more than 10 per cent. of acetic
acid, which is itself a comparatively weak acid. It is, therefore, not a
very active solvent. Nevertheless, for metals and for limestone rock,
and other substances of a calcareous nature, its solvent power is
greater than that of any other liquid known at the time of its
discovery. It was this property which seems to have appealed most
strongly to the imagination of the early chemists; and, as is very often
the case, the description of its powers was very much exaggerated. Livy
and Plutarch, who have given us an account of Hannibal’s invasion of
Italy by way of the Alps, both gravely declare that the Carthaginian
leader cleared a passage for his elephants through solid rocks by
pouring vinegar over them!

In the Middle Ages, the study of Chemistry was fostered mainly as a
possible means whereby long life and untold riches might be obtained.
The “Philosopher’s Stone,” by the agency of which the base metals were
to be changed to gold, and the “Elixir of Life,” which was to banish
disease and death, were eagerly sought for. Though these were vain
imaginings according to modern ideas, nevertheless they were powerful
incentives towards experimental work. Many new substances were
discovered in this period, and among these were nitric acid (aqua
fortis), hydrochloric acid (spirit of salt), and sulphuric acid (oil of
vitriol).

Acids were then valued above all other substances. The mediaeval chemist
(or alchemist, as he was called) clearly saw that unless a body could be
dissolved up there was no hope of changing it. Nitric acid, therefore,
which, in conjunction with hydrochloric acid, dissolved even gold
itself, was very highly esteemed. Oil of vitriol also was scarcely less
important, for it was required for the production of other acids.

So far, taste and solvent power were considered to be the characteristic
feature of acids. In the time of Robert Boyle (1627-1691), they were
further distinguished from other substances by the change which they
produced in the colour of certain vegetable extracts. Tincture of red
cabbage was first used, but, as this liquid rapidly deteriorates on
keeping, it was soon replaced by a solution of litmus, a colouring
matter obtained from _Roccella tinctoria_ and other lichens. It imparts
to water a purple colour, which is changed to red by the addition of
acids.

Alkalis. Wood ashes were valued in very early times because they were
found to be good for removing dirt from the skin. Mixed with vegetable
oil or animal fat, they formed a very primitive kind of soap, which was
afterwards much improved by using the aqueous extract instead of the
ashes themselves, and also by the addition of a little caustic lime.

When plant ashes are treated with water, about 10 per cent. dissolves.
If the insoluble matter is then allowed to settle down and the clear
liquid evaporated to dryness, a whitish residue is obtained. The soluble
matter thus extracted from the ashes of plants which grow in or near the
sea is mainly soda; that from land plants, mainly potash. Formerly no
distinction was made, and the general term “alkali” was applied to both.

In order to bring the properties of alkalis into contrast with those of
acids, we cannot do better than make a few simple experiments with a
weak solution of washing soda. Its taste is very different from that of
an acid; it is generally described as caustic. If a little is rubbed
between the fingers, it feels smooth, almost like very thin oil. It does
not dissolve metals or limestone. Its action on vegetable colouring
matter is just as striking as that of acids. Tincture of red cabbage
becomes green; the purple of litmus is changed to a light blue. This
colour change is characteristic of alkalis.

Neutralization. When the colour of litmus solution has been changed to
red by the addition of an acid, the original colour can be restored by
adding an alkali. The change can be repeated as often as desired by
adding acid and alkali alternately. From this we get a distinct
impression of antithesis between the two. In popular language, an alkali
“kills” an acid; in Chemistry, the same idea is expressed by the term
“neutralization.”

Salts. Both “neutralization” and “killing the acid” are modes of
expression which describe the phenomenon fairly well. When an acid is
neutralized, its characteristic taste, its solvent power, and its action
on litmus, are all changed; in fact, the acid as an acid ceases to
exist, and so does the alkali. When the neutral solution is evaporated
to dryness, a residue is found which on examination proves to be neither
the acid nor the alkali, but a compound formed from the two. This
substance is called a salt.

To most people, salt is the name for that particular substance which is
taken as a condiment with food. Its use in this connection dates from
time immemorial. It is distinctly unfortunate that another and very much
wider usage of the term has been introduced into Chemistry. When the
early chemists recognized that other substances, which they vaguely
designated as “saline bodies,” were similar to common salt in
composition, they took the name of the individual and applied it to the
whole class.


                    OTHER METHODS OF SALT FORMATION

Solution of Metals in Acids. Alkalis are not the only substances which
neutralize acids. Speaking in a broad and general sense, we may say that
an acid is neutralized when a metal is dissolved in it, because, when
the point is reached at which no more metal will dissolve, all the
characteristic properties of the acid are destroyed. A salt is formed in
this case also.

An example will now be given to illustrate this method of salt
formation. Before two pieces of metal can be united by soldering, it is
necessary to clean the surfaces of the metal and the soldering iron. The
liquid used for this purpose is made by adding scraps of zinc to
muriatic acid (hydrochloric acid). The zinc dissolves with
effervescence, which is caused by the escape of hydrogen gas. When
effervescence ceases and no more zinc will dissolve, the liquid is ready
for use. The acid has been “killed” or neutralized by the metal. A salt
called zinc chloride has been formed. This salt can be recovered from
the liquid by evaporation.

Solution of Oxides in Acids. The substances most used in commerce with
the express purpose of destroying acidity are quicklime, washing soda,
and powdered chalk.

Since quicklime is a compound of the metal calcium and the gas oxygen,
its systematic name is calcium oxide; when it neutralizes an acid, it
forms the corresponding calcium salt; for example, if it neutralizes
acetic acid, calcium acetate is formed.

An instance of the neutralization of an acid by an oxide of a metal is
furnished by one method of preparing blue vitriol (copper sulphate).
Copper does not dissolve very quickly in dilute sulphuric acid; hence,
to make blue vitriol from scrap copper, the metal is first heated very
strongly while freely exposed to air. Copper and oxygen of the air
combine to form the brownish black powder, copper oxide, and this
dissolves very readily in sulphuric acid, making the salt, copper
sulphate.

Solution of Carbonates in Acids. Washing soda and chalk belong to a
different class of chemical substances. They are carbonates, that is,
they are salts of carbonic acid. At first it may seem a little
perplexing to the reader to learn that a salt can neutralize an acid to
form a salt. It must be remembered, however, that acids differ from one
another in strength, that is, in chemical activity, and that carbonic
acid is a weak acid. When a salt of carbonic acid—sodium carbonate or
washing soda, for example—is added to a stronger acid such as sulphuric
acid, sodium sulphate is formed and carbon dioxide liberated.

As an example of the neutralization of acids by carbonates, we may
mention here a practical sugar saving device. Unripe fruit is very sour
because it contains certain vegetable acids dissolved in the juice.
These acids are not affected by boiling; and, therefore, to make a dish
of stewed fruit palatable, it is necessary to add sugar in quantity
sufficient to mask the sour taste. If a pinch of bicarbonate of soda is
added to neutralize the acid, far less sugar will be necessary for
sweetening.

Insoluble Salts. The methods given above apply only to those salts which
are soluble in water. Insoluble salts are obtained by mixing two
solutions, the one containing a soluble salt of the metal, and the
other, a soluble salt of the acid or the acid itself.

The formation of an insoluble salt by the interaction of two soluble
substances is well illustrated in the preparation of Burgundy mixture,
the most effectual remedy yet proposed for checking the spread of potato
disease. This mixture contains copper carbonate, that is, the copper
salt of carbonic acid. For its preparation we require copper sulphate
and sodium carbonate (washing soda), a soluble carbonate. When these two
substances, dissolved in separate portions of water, are mixed, copper
carbonate is formed as a pale blue solid which is in such a state of
fine subdivision that it remains suspended in the solution of sodium
sulphate, the other product of the reaction.

The change is represented diagrammatically below. Each circle represents
the atom or a group of atoms named therein. At the moment of mixing,
these groups undergo re-arrangement.

Bordeaux mixture, which some gardeners prefer, is a similar preparation
containing copper hydroxide instead of copper carbonate. It is made by
mixing clear lime water (a soluble hydroxide) with copper sulphate.

    [Illustration: Fig. 1]

Elements and Compounds. It is scarcely possible to discuss chemical
processes without having from time to time to use terms which are not in
everyday use. A few preliminary definitions and explanations of terms
which will be frequently used may serve to simplify descriptions, and
render it unnecessary to encumber them with purely explanatory matter.

Among the many different kinds of materials known, which in the
aggregate amount to several hundreds of thousands, there are about
ninety substances which up to the present time have not been broken up
into simpler kinds. These primary materials are called “elements,” the
remainder being known as “compounds.”

The following is a list of the commonest of these elements, together
with the symbols by which they are represented in Chemistry.

  METALS
  Aluminium                       Al.
  Antimony (_Stibium_)            Sb.
  Barium                          Ba.
  Bismuth                         Bi.
  Cadmium                         Cd.
  Calcium                         Ca.
  Chromium                        Cr.
  Copper (_Cuprum_)               Cu.
  Gold (_Aurum_)                  Au.
  Iron (_Ferrum_)                 Fe.
  Lead (_Plumbum_)                Pb.
  Lithium                         Li.
  Magnesium                       Mg.
  Manganese                       Mn.
  Mercury (_Hydrargyrum_)         Hg.
  Nickel                          Ni.
  Platinum                        Pt.
  Potassium (_Kalium_)            K.
  Silver (_Argentum_)             Ag.
  Sodium (_Natrium_)              Na.
  Strontium                       Sr.
  Tin (_Stannum_)                 Sn.
  Zinc                            Zn.

  NON-METALS
  Boron                           B.
  Bromine                         Br.
  Carbon                          C.
  Chlorine                        Cl.
  Fluorine                        F.
  Hydrogen                        H.
  Iodine                          I.
  Nitrogen                        N.
  Oxygen                          O.
  Phosphorus                      P.
  Silicon                         Si.
  Sulphur                         S.

The first step in the building-up process consists of the union of a
metallic with a non-metallic element. Such compounds are binary
compounds, and are distinguished by the termination -ide added to the
name of the non-metallic element; for example, copper and oxygen unite
to form copper oxide, sodium and chlorine form sodium chloride, iron and
sulphur form iron sulphide or sulphide of iron.

A compound containing more than two elements is distinguished by the
termination -ate. Most salts fall within this category; thus we speak of
acetate of lead and chlorate of potash, also of sodium sulphate and
copper sulphate, the latter form being the more correct.

A difficulty arises when two bodies are composed of the same elements
combined in different proportions. Then we have to resort to other
distinguishing prefixes or suffixes. For this reason we meet with
sulphur_ous_ acid and sulphur_ic_ acid, the corresponding salts being
sulph_ites_ and sulph_ates_.

Crystals and Water of Crystallization. When a soluble salt is to be
recovered from its solution, the latter is reduced in bulk by
evaporation until, either by experience or by trial, it becomes evident
that the solid will be formed as the liquid cools. In some cases, when
time is not an important factor, evaporation is left to take place
naturally. Under either set of conditions, the substance generally
separates out in particles which have a definite geometrical form. These
are spoken of as crystals.

Crystals often contain a definite percentage of water, called “water of
crystallization.” In washing soda, this combined water forms nearly 63
per cent. of the total weight; in blue vitriol, it is approximately 36
per cent. On being heated to a moderate temperature, the water is
expelled from the solid; the substance which is left behind is called
the anhydrous (that is, the waterless) salt.



                               CHAPTER II
                      SULPHURIC ACID AND SULPHATES


Key Industries. The importance of the chemical industries depends mainly
on the fact that they constitute the first step in a series of
operations by which natural products are adapted to our needs. The
materials which are found in earth, air, and water are both varied in
kind and abundant in quantity, but in their natural state they are not
generally available for immediate use. Moreover, very many substances
now deemed indispensable are not found ready formed in Nature.

The end product of the chemical manufacturer is often one of the primary
materials of some other industry. Soda ash and Glauber’s salt are
essential for making glass; soap could not be produced without caustic
alkali; the textile trade would be seriously handicapped if bleaching
materials, mordants, and dye-stuffs were not forthcoming. Considered in
this light, the preparation of chemicals is spoken of as a “key
industry.”

Furthermore, very few of these indispensable substances can be made
without using sulphuric acid. This acid is, on that account, just as
important to chemical industries as the products of these are to other
branches of trade. It may, therefore, be looked upon as a master key of
industrial life.

Primary Materials. The composition of sulphuric acid is not difficult to
understand. Air is mainly a mixture of oxygen and nitrogen; and when a
combustible body burns, it is because chemical action between the
material and oxygen is taking place. In this way, sulphur burns to
sulphur dioxide. This gas, dissolved in water, forms sulphur_ous_ acid,
which changes slowly to sulphur_ic_ acid by combination with more
oxygen. Hence, sulphur, oxygen, and water are the primary materials
required for making sulphuric acid.

Sulphur is the familiar yellow solid commonly known as brimstone. It is
found native in the earth, and is fairly abundant in certain localities,
notably in the neighbourhood of active and extinct volcanoes. Italy,
Sicily, Japan, Iceland, and parts of the United States are the principal
sulphur-producing countries. Though very plentiful and consequently
cheap, only a relatively small quantity of sulphuric acid is made
directly from native sulphur, because at the time when this industry was
started in England, restrictions were placed on the export of sulphur
from Sicily and, consequently, the plant which was then established was
adapted to the use of iron pyrites.

Iron pyrites contains about 53 per cent. of sulphur combined with 47 per
cent. of iron, and when this is burnt in a good draught, nearly the
whole of the sulphur burns to sulphur dioxide, leaving a residue of
oxide of iron which can be used for making cast iron of a low grade.

Iron pyrites is often supplemented by the “spent oxide” from the gas
works. Crude coal gas contains sulphur compounds which, if not removed,
would burn with the gas and form sulphur dioxide. The production of
these pungent and suffocating fumes would be a source of great
annoyance, and therefore it is necessary to remove the sulphur
compounds. To do this, the gas is passed through two purifiers, the
first containing slaked lime and the second ferric oxide, both in a
slightly moist condition. After being some time in use, the purifying
material loses its efficacy; the residue from the lime purifier is sold
as “gas lime,” but that from the ferric oxide purifier is exposed to the
air and so “revived.” At length, however, it becomes so charged with
sulphur that it is of no further use for its original work. It is then
passed on to the sulphuric acid maker.

Evolution of the Manufacturing Process. In dealing with the main
processes for the manufacture of acids and alkalis, reference will
frequently be made to the methods of bygone times. Although as an exact
science Chemistry is comparatively modern, as a branch of human
knowledge its history goes back to the dawn of intelligence in man. It
is agreed that the higher types of living things are more easily
understood when those of a simpler and more primitive character have
been studied. In like manner, the highly specialized industries of
modern times become more intelligible in the light of the efforts of
past generations to achieve the same object.

Basil Valentine, who lived in the fifteenth century, states that the
liquid which we now call sulphuric acid was in his day obtained by
heating a mixture of green vitriol and pebbles. Until quite recent
times, sulphuric acid of a special grade was made by precisely the same
method, except that the pebbles were dispensed with. In passing, we may
remark that the common name “vitriol,” or “oil of vitriol,” is accounted
for by this connection with green vitriol. The second method, quoted by
Basil Valentine, consisted of the ignition of a mixture of saltpetre and
sulphur in the presence of water. This is actually the modern lead
chamber process in embryo.

    [Illustration: Fig. 2. PLAN OF SULPHURIC ACID WORKS]

About the middle of the eighteenth century, “Dr.” Ward took out a patent
for the manufacture of sulphuric acid, to be carried on at Richmond in
Surrey. He used large glass bell jars of about 40-50 galls. capacity, in
which he placed a little water and a flat stone to support a red-hot
iron ladle. A mixture of saltpetre and sulphur was thrown into the ladle
and the mouth of the vessel quickly closed. After the vigorous chemical
action was over, the ladle was re-heated and the process repeated until
at last fairly concentrated sulphuric acid was produced.

The large glass vessels used by Ward were costly and easily broken. They
were soon replaced by chambers about 6 ft. square, made of sheet lead,
but otherwise the process was just the same. The next advance consisted
in making the process continuous instead of intermittent. An enormously
increased output was thereby rendered possible, and the main features of
the modern process gradually developed.

The Lead Chamber Process. We can now consider the actual working of the
lead chamber process, aided by the diagrammatic plan of the works shown
in Fig. 2. Sulphur dioxide is produced in a row of kilns (A-A) by
burning iron pyrites in a carefully regulated current of air. The
mixture of gases which leaves the pyrites burners contains sulphur
dioxide, excess of oxygen, and a very large quantity of nitrogen. To
this is added the vapour of nitric acid, generated from sodium nitrate
and concentrated sulphuric acid contained in the “nitre pots,” which are
placed at B. The mixture of gases then passes up the Glover tower (C)
and through the three chambers in succession, into the first two of
which steam is also introduced. Sulphuric acid is actually produced in
the chambers, and collects on the floors, from which it is drawn off
from time to time. The residual gas from the last chamber is passed up
the Gay Lussac tower (D), and after that is discharged into the air by
way of the tall chimney (J).

    [Illustration: Fig. 3. GENERAL VIEW OF SULPHURIC ACID WORKS]

The Oxygen Carrier. We have seen that sulphur dioxide, oxygen, and water
are the only substances required to produce sulphuric acid. Why, then,
is the nitric acid vapour added to the mixture? As described in a former
paragraph, the combining of these gases was represented as being a very
simple operation. So indeed it is, for it even takes place
spontaneously. Yet, as a commercial process, it would be quite
impracticable without the nitric acid vapour, for although the gases
combine spontaneously, they do so very slowly, and it is the nitric acid
vapour which accelerates the rate of combination.

It is not known with any degree of certainty how the nitric acid acts in
bringing about this remarkable change. It has been suggested that
reduction to nitrogen peroxide first takes place, and that sulphur
dioxide takes oxygen from this body, reducing it still further to nitric
oxide, which at once combines with the free oxygen present to form
nitrogen peroxide again. So the cycle of changes goes on, the nitrogen
peroxide playing the part of oxygen carrier to the sulphur dioxide; and
since it is continually regenerated, it remains at the end mixed with
the residual gases.

Recovery of the Nitrogen Peroxide. If the gases from the last chamber
passed directly into the chimney shaft, there would be a total loss of
the oxides of nitrogen, and the consequence of this would be that more
than 2 cwt. of nitre would have to be used for the production of 1 ton
of sulphuric acid. This would be a serious item in the cost of
production, and it is therefore essential that this loss should be
prevented.

The recovery of the oxides of nitrogen is effected in the Gay Lussac
tower, a structure about 50 ft. in height, built of sheet lead and lined
with acid-resisting brick. It is filled with flints, over which a slow
stream of cold concentrated sulphuric acid is delivered from a tank at
the top. As the gas from the last chamber passes up this tower, it meets
the stream of acid coming down. This dissolves and retains the nitrogen
peroxide. The acid which collects at the bottom of the tower is known as
nitrated vitriol.

The next step is to bring the recovered nitrogen peroxide again into
circulation. The nitrated vitriol is raised by compressed air to the top
of the Glover tower, and as it trickles down over the flints in this
tower it is diluted with water, while at the same time it meets the hot
gases coming from the pyrites burners. Under these conditions, the
nitrogen peroxide is liberated and carried along by the current of gas
into the first lead chamber. The stream of cold acid coming down the
Glover tower also serves to cool the hot gases before they enter the
first chamber.

In order to complete the description of the works, it is necessary to
add a note on the lead chambers themselves. The sheet lead used in their
construction is of a very substantial character; it weighs about 7 lb.
per square foot. The separate strips are joined together by autogenous
soldering, that is, by fusing the edges together. In this way the
presence of another metal is avoided; otherwise this would form a
voltaic couple with the lead, and rapid corrosion would take place.

The size of the chambers has varied a great deal. In the early years of
the nineteenth century, the capacity of a single chamber was probably
not more than 1,000 cu. ft.; at the present time, 38,000 cu. ft. is an
average size, and there may be three or five of these chambers. The
necessity for this large amount of cubic space is easily accounted for.
The reaction materials are all gases, and a gas occupies more than one
thousand times as much space as an equal weight of a solid or liquid.
Moreover, oxygen constitutes only about one-fifth of the total volume of
air used in burning the pyrites; the other four-fifths is mainly
nitrogen, which, though it does not enter into the reaction at all, has
to pass through the chambers.

Modern Improvements. Among the modern innovations in the lead chamber
process, the following are worthy of note. “Atomized water,” that is,
water under high pressure delivered from a fine jet against a metal
plate, has certain advantages over steam. In order to bring about a more
rapid mixing of the gases in the chamber, it is proposed to make these
circular instead of rectangular, and to deliver the gases tangentially
to the sides. Another suggestion is to replace the lead chambers by
towers containing perforated stoneware plates set horizontally. By this
arrangement, since the holes are not placed opposite one another, the
gases passing up the tower must take a zig-zag course. This makes for
more efficient mixing.


                          THE CONTACT PROCESS

Sulphur Trioxide. When elements are combined in different proportions by
weight, they produce different compounds. Thus, in the case of sulphur
and oxygen, there are two well-known compounds, namely, sulphur dioxide
and sulphur trioxide. In the former, a given weight of oxygen is
combined with an _equal_ weight of sulphur; in the latter, this same
weight of sulphur is combined with 50 per cent. more oxygen. On this
account, sulphur trioxide is spoken of as the higher oxide.

We can now state in general terms another method by which sulphuric acid
can be built up from its elements. Sulphur, as we have seen, burns in
oxygen, forming sulphur dioxide. This substance can then be made to
unite with more oxygen to give sulphur trioxide, which, with water,
yields sulphuric acid. There are three steps in this synthesis. The
first, namely, sulphur to sulphur dioxide, has already been considered;
the last, sulphur trioxide to sulphuric acid, only requires that sulphur
trioxide and water shall be brought together: we can, therefore, confine
our attention to the intermediate step, namely, the conversion of
sulphur dioxide into trioxide.

This operation, when carried out in a chemical laboratory, is a very
simple one. Fig. 4 shows the necessary apparatus. Sulphur dioxide from a
siphon of the liquefied gas and air from a gasholder are passed into the
Woulff’s bottle A, containing concentrated sulphuric acid; this removes
moisture from the gases. The drying process is completed in the tower B,
which contains pumice stone soaked in sulphuric acid. The mixed gases
then pass through the tube C, containing platinized asbestos heated to
about 400° C.: the sulphur trioxide collects in the cooled receiver D.

    [Illustration: Fig. 4. SULPHUR TRIOXIDE—THE CONTACT PROCESS]

Platinized asbestos is made by soaking long-fibred asbestos in a
solution of platinum chloride. The material is then dried and subjected
to a gentle heat. In this way, metallic platinum in an exceedingly fine
state of subdivision is deposited on the asbestos fibre, which merely
serves as a convenient support.

Catalytic or Contact Action. The influence of the finely divided
platinum is a very important factor in the reaction. It cannot, however,
be said to _cause_ the union of sulphur dioxide with oxygen, for the
gases combine to a very slight extent when it is not present. What the
platinum actually does is to influence the rate of formation to such a
degree that, under favourable conditions, practically the whole of the
sulphur dioxide is changed to sulphur trioxide instead of an exceedingly
small fraction of it.

The most interesting, and at the same time the most perplexing, feature
of the reaction is that the platinum itself does not appear to undergo
any change. It is not diminished in quantity, for only a very small
amount is necessary for the conversion of a very large amount of the
mixed gases. Its activity lasts for a very long time, and even when it
does become inactive, it can be shown that this is due to some external
cause, such as the presence of dust and certain impurities in the gases.

Many other similar cases are known in which the presence of a small
quantity of a third substance greatly influences the course of a
chemical reaction without appearing in any other way to be necessary to
the reaction. These substances, which are often metals in a very fine
state of subdivision, are called catalytic or contact agents.

The Contact Process for making sulphuric acid is nothing more nor less
than the simple laboratory operation which we have described above,
carried out on a larger scale.

The sulphur dioxide is produced as in the lead chamber process by
roasting iron pyrites in a current of air. This gas, together with the
excess of air, is passed into the contact furnace, which consists of
four tubes, each containing platinized asbestos, supported on perforated
plates. The union of the two gases is said to be almost complete: an
efficiency of 98 per cent. of the theoretical value is claimed for this
process. The sulphur trioxide, or “sulphuric anhydride”[1] is either
condensed in tin-lined drums or absorbed in ordinary concentrated
sulphuric acid.

The proposal to manufacture sulphuric acid by this method was first made
in 1831 by Peregrine Phillips, of Bristol. The early attempts were not
successful, and it was not until about forty-four years later that the
difficulties arising in the working of the contact process were overcome
sufficiently to enable the sulphuric acid produced in this way to be
sold at the same price as that made by the lead chamber process. Since
1890, the total quantity of acid made by the contact method has
increased very rapidly, so that it now furnishes about one-half of the
world’s supply, and seems likely in time to displace the lead chamber
process altogether.

The history of the rise of the contact process is interesting because it
illustrates in a striking manner the very great difference that there is
between a successful laboratory process and a successful manufacturing
process, though seemingly identical.

The first and possibly the most serious difficulty encountered in the
working of the contact process was the frequent interruption caused by
the loss of activity of the contact substance. Iron pyrites always
contains arsenic which volatilizes on heating, and this quickly caused
the platinum to lose its activity, or, as it was sometimes rather
fancifully expressed, “poisoned the catalyst.” Dust also is inevitable,
and this, carried forward mechanically with the stream of gas, settled
on the contact substance and caused the action to cease.

To get over this difficulty it is necessary to purify the gases. They
are first passed slowly through channels in which the coarser particles
of dust settle down. Steam is injected into the mixture to wash out the
finer particles of solid, and also to get rid of arsenic, and then the
gases are passed through scrubbers. Before being admitted to the contact
furnace, the moist gas is submitted to an optical test. It is passed
through a tube, the ends of which are transparent; a bright light is
placed at one end and viewed from the other through a column of gas of
considerable length. If the purification process is working
satisfactorily, there is a complete absence of fog. The gases are then
dried by passing through concentrated sulphuric acid and admitted to the
contact tubes.

In all operations carried out on a large scale, the regulation of
temperature is a matter of some difficulty. In the case which we are
considering, the most suitable temperature range is a rather narrow one,
and the difficulty of keeping within the limits is very much increased
by the large amount of heat given out when the sulphur dioxide and
oxygen combine. The result of the failure to maintain the temperature at
a fairly constant level was that the process worked in a very irregular
manner, for as soon as it was working really well and sulphur trioxide
was being formed rapidly, the heat given out by the reaction itself was
also great, and consequently, the higher temperature limit was exceeded.

The method of controlling the temperature in the contact process is
worth noting, because it is really ingenious. The tubes containing the
platinized asbestos are surrounded by wider concentric tubes. The gases
which are about to enter the contact furnace pass through the annular
space between the two tubes, and are thereby heated to the required
temperature, while at the same time they serve to cool the inner tubes.
The most satisfactory temperature is about 400° C. The tubes are first
warmed to 300° C. to start the reaction, and thereafter the heat evolved
by the reaction itself is sufficient to keep it going.

The absorption of the sulphur trioxide also caused some difficulty at
first. This substance reacts most violently with water, dissolving with
a hissing sound like that produced when a red-hot poker is plunged into
water. At the same time great heat is developed, and consequently, much
of the sulphur trioxide is vaporized, and in that way lost. This
difficulty was got over by using 98 per cent. sulphuric acid for the
absorption, the acid being kept at this strength by the simultaneous
addition of water.

The contact process has some very distinct advantages over the older
lead chamber process. The plant covers a much smaller area than the
bulky lead chambers. Although the preliminary purification of the gases
is somewhat tedious and costly, this is in great measure compensated by
the purity of the acid produced. No separate plant is required for
concentration and purification, as in the older process. Finally,
sulphuric acid of any concentration can be produced at will, including
the fuming acid, which is required as a solvent for indigo, and in the
manufacture of artificial indigo and other organic chemicals.

The lead chamber process produces what is called chamber sulphuric acid
very cheaply. Although this is only a 60-70 per cent. solution and very
impure, nevertheless, it is quite good enough for the heavy chemical
trade, particularly for the first stage of the Leblanc soda process, and
for making superphosphate. These two industries alone consume many
thousands of tons of this sulphuric acid every year. Probably for some
years to come the two processes will continue to exist side by side, but
it may be doubted whether new works will now be installed to make
sulphuric acid by the lead chamber process.

Properties of Sulphuric Acid. The pure non-fuming acid is a colourless
oily liquid whose density is 1·84. It mixes with water in all
proportions, yielding dilute sulphuric acid, and it also dissolves
sulphur trioxide, yielding the fuming acid.

The mixing of sulphuric acid and water is accompanied by an evolution of
heat and by contraction in volume. It is an operation which must be
carried out with great care, the acid being always poured into the
water, otherwise the water floats on the heavier acid, and so much heat
is developed at the surface of separation that some of the water will be
suddenly converted into steam, and this, escaping from the liquid with
explosive violence, may cause the contents of the vessel to be scattered
about.

Strong sulphuric acid chars most organic substances. From substances
such as wood, sugar, paper, starch, it withdraws the elements of water,
liberating carbon. Since it acts in the same way upon human flesh, it is
clear that the concentrated acid must be handled with very great care,
for it causes most painful burns. For this reason, vitriol throwing has
always been regarded as a most serious and dastardly offence. A simple
first-aid remedy for burns produced by sulphuric acid is the liberal
application of an emulsion of linseed oil and lime water. The lime,
being an alkali, neutralizes the acid, and the oil excludes air from the
wound.

The readiness with which sulphuric acid combines with water is often
made use of both in the laboratory and in industrial Chemistry for the
purpose of drying gases. One illustration of this use has already been
given in describing the contact process. Another instance which may be
fairly familiar occurs in the case of liquefying air, where the gas must
be thoroughly dried before being passed into the refrigerating
apparatus, otherwise this would soon become blocked with ice.

The position which sulphuric acid occupies in Chemistry is due mainly to
three outstanding features. In the first place, it is a strong mineral
acid and displaces all other acids from their salts. Secondly, it has a
high boiling point (338° C.), and consequently, the displaced acid with
the lower boiling point can be distilled from the mixture. Lastly,
sulphuric acid can be made very cheaply from materials which are very
abundant in Nature, and, therefore, it meets all the requirements of an
acid which is to be used for general purposes.


                               SULPHATES

All the common metals, except gold and platinum, dissolve either in
concentrated or in dilute sulphuric acid, forming sulphates. These salts
are highly important and interesting substances. They are all soluble in
water, with the exception of the sulphates of calcium, strontium,
barium, and lead.

Ferrous Sulphate, also called green vitriol and copperas, is obtained by
dissolving iron in dilute sulphuric acid. The solution is green, and
when it is evaporated, the crystals which separate out look like bits of
green glass. It was because of this that the substance was first called
green vitriol (_vitrum_ = glass). It is used very largely in dyeing as a
mordant. Writing ink and Prussian blue are also made from it.

The Alums are double sulphates. They are made by crystallizing solutions
of potassium, sodium, or ammonium sulphate together with solutions of
iron (ferric), chromium, or aluminium sulphates. In this way, we may
have potassium aluminium alum, or iron ammonium alum, and so on, but
whichever combination of elements is present, the salt which is formed
always crystallizes in octahedra. The chief use of the alums, as also of
aluminium sulphate, is as mordants in dyeing.

Since a great many metallic salts, particularly acetates and sulphates,
are used in the dye industry as mordants, it may be well to explain here
very briefly what a mordant is.

It must be remembered that almost all the dyes are solids which dissolve
in water, yielding intensely coloured solutions. Hence, in most cases,
if a fabric is merely dipped in the dye and then dried, the colouring is
not permanent, but can be washed out with water. In order to fix the
colouring matter, the material is first dipped in the mordant, usually a
bath of some metallic salt, and then, generally after exposure to air or
after steaming, into the dye bath, with the result that the colour
becomes fixed. The first part of the process is called “mordanting” the
material. The mordant either adheres to or combines with the fibres, and
the dye forms with the mordant a coloured compound called a “lake,”
which resists the action of water. The colour is then said to be “fast,”
that is, firmly fixed.

For printing on calico, the mordant is thickened with gum arabic or
other glutinous substance. The design is then stamped on the material
with the thickened mordant liquor. The subsequent treatment consists of
dipping the material in the dye and afterwards in water, when the colour
comes away from those parts which have not received the impress of the
mordant.

Sodium Sulphate, or Glauber’s salt, is made from common salt by the
action of concentrated sulphuric acid. It is one of the raw materials
used in making glass.

Ammonium Sulphate. (_See_ p. 99.)

Calcium Sulphate, or gypsum, occurs in large quantities in Nature. The
salt contains 20·9 per cent. of combined water, and when carefully
heated to 120° C, it loses about two-thirds of this water, yielding a
white powder known as plaster of Paris. This substance, when made into a
paste with water, gradually sets to a hard mass, because the partially
dehydrated gypsum re-combines with the water.

Lead Sulphate, the chief impurity of commercial oil of vitriol, is a
white powder which is very often used for making white paint in place of
lead carbonate (white lead). The sulphate has the advantage over the
carbonate in not being so readily discoloured; its disadvantage is that
it lacks “body.”

Copper Sulphate, or blue vitriol, is frequently found in the drainage of
copper mines, where it is formed by the oxidation of copper pyrites. It
is made on a large scale by roasting sulphide ores of copper in a
current of air. Oxygen combines with copper sulphide, forming copper
sulphate, which is extracted with water and crystallized. It forms large
blue crystals containing 36 per cent. of water. This salt is put to many
different uses. Very large quantities are used for dyeing and calico
printing; some of the green pigments, such as Schweinfurt green, are
made from it.



                              CHAPTER III
                        NITRIC ACID AND NITRATES


Nitric acid, the _aqua fortis_ of the alchemists, must be placed next to
sulphuric acid in the scale of relative importance, because of the
variety of its uses. It is indispensable for making explosives, and is
used for the preparation of drugs and fine chemicals, including the
coal-tar dyes. The acid also dissolves many metals, forming nitrates,
which are put to several uses. Silver nitrate is the basis of marking
ink, and it is also the substance from which the light-sensitive silver
compounds required for the photographic industry are made. The important
pigments, chrome yellow and chrome red, are prepared from lead nitrate.
The solvent action of nitric acid on copper is made use of in etching
designs on copper plates. Over and above all this, it must be mentioned
that an adequate supply of “nitrate” is required for artificial manure.
Thus it can be said that with the uses of this acid and its salts are
associated our supply of daily bread, our freedom from foreign
oppression, and many of the refinements and conveniences of life.

We shall begin the study of nitric acid by taking stock, as it were, of
the natural sources of supply. The free acid is not found in Nature
except for very small traces in the air after thunderstorms. We have,
therefore, to rely entirely on that which can be obtained artificially.
Until quite recently, it could be said that there was only one method of
making the acid, namely, by the distillation of a mixture of potassium
or sodium nitrates and concentrated sulphuric acid. Now, however, nitric
acid is being made from the air, though as yet only in small quantity,
notwithstanding the great development of this method owing to war
requirements; hence, we are still mainly dependent on the naturally
occurring nitrates just mentioned.

Potassium Nitrate (nitre, saltpetre, sal prunella) is found in the soil
of hot countries, especially in the neighbourhood of towns and villages
where the sanitary arrangements are primitive. In very favourable
circumstances, it may even appear as a whitish, mealy efflorescence on
the surface of the ground. To obtain the salt, it is only necessary to
agitate the surface soil with water and, after the insoluble matter has
settled down, to evaporate the clear solution.

Potassium nitrate is required for making gunpowder, which, until quite
recent times, was the only explosive used in warfare. Continental
countries that could not afford to rely entirely on sea-borne nitre had
to make their own. The refuse of the farmyard, mixed with lime and
ashes, was made up into a heap of loose texture, which was periodically
moistened with the drainage from the stables. In the course of years,
saltpetre and calcium nitrate were formed in the surface layers, from
which they were extracted from time to time. The farmer was then allowed
to pay part of his taxes in nitrates.

Sodium Nitrate, also called caliche, Chili-saltpetre, or Chili-nitrate,
comes mainly from South America. The beds extend for a distance of about
220 miles in Chili, Peru, and Bolivia, between the Andes mountains and
the sea. The deposit is about 5 ft. thick, and its average breadth 5
miles. The crude material is treated with water in steam-heated wooden
vats. The clear solution is evaporated, and the residue obtained is
washed with the mother liquor and dried. This product may contain as
much as 98 per cent. of the nitrate.

    [Illustration: Fig. 5. PREPARATION OF NITRIC ACID]

Nitric Acid. Chili-nitrate is always used for making nitric acid. It is
the more abundant of the two naturally occurring nitrates, and therefore
cheaper; moreover, weight for weight, it yields more nitric acid than
the corresponding potassium compound. A mixture of sodium nitrate and
sulphuric acid is heated in a large cast-iron retort (C, Fig. 5). The
retort is entirely surrounded by flame and hot gases to prevent the
condensation of the acid on the upper parts. If this precaution were not
taken, the acid would dissolve the iron and the life of the retort would
not be long; moreover, the product would contain ferric nitrate as an
impurity. The vapour of the acid is led away by the tube D into a series
of two-necked earthenware receivers called _bonbonnes_ (E), and there
condenses to a liquid. The lower figure shows how the leading tube of
the retort is protected from corrosion by the clay tube _a_, _b_; and
how it is connected to the first receiver by the glass tube _e_, which
is luted on at _f_. The percentage strength of the acid which distils
over depends upon that of the sulphuric acid used and on the purity of
the sodium nitrate.

Pure nitric acid is a colourless liquid 1·559 times as heavy as water,
volume for volume. It fumes strongly in air, and is a very corrosive
liquid. The pure acid of commerce is obtained by distillation of a less
concentrated acid. It is 68 per cent. pure. It is rendered free from
dissolved oxides of nitrogen by blowing air through it. When kept
exposed to light, the colour changes at first to yellow and then to
brown, because light causes a certain amount of decomposition.

Red fuming nitric acid owes its colour to the great quantity of oxides
of nitrogen dissolved in it. It is made by distilling sodium nitrate
that has been thoroughly dried with the strongest sulphuric acid; the
distillation is carried out at a high temperature, with the express
purpose of decomposing some of the nitric acid to furnish the oxides of
nitrogen. Sometimes a little powdered starch is also added to facilitate
the formation of these oxides. This variety of nitric acid is
particularly active and is used in many operations, especially in making
dyes, explosives, and other organic chemicals.

Nitric acid has all the general properties of an acid, that is, it has a
sour taste even in very dilute solution, it changes the colour of litmus
to red, and dissolves carbonates and many metals.

When the vapour of nitric acid is passed through a red-hot tube, and
also when a nitrate is strongly heated, oxygen gas is given off.
Analysis shows that the oxygen combined in pure nitric acid amounts to
76 per cent. of its weight, while that in sodium and potassium nitrates
is 56 and 50 per cent. respectively. Nitric acid and the nitrates are,
therefore, highly oxygenated compounds; moreover, under favourable
circumstances, they are rather easily broken up.

Pure nitric acid will set fire to warm, dry sawdust, and a piece of
charcoal or sulphur thrown on the surface of molten nitre takes fire
spontaneously and is quickly consumed, giving out a very vivid light.
The explanation of this is that the supply of oxygen is abundant; it is
also readily available and concentrated in a small space. We can vary
the experiment. When a mixture of 75 parts by weight of finely-powdered
saltpetre, with 15 of charcoal dust and 10 of ground sulphur, is
ignited, it burns very vigorously, and is soon consumed. This mixture
is, indeed, home-made gunpowder.

Explosives. Gunpowder was discovered in very early times by the Chinese,
but for many years the secret of its composition did not get outside the
Great Wall. In the fifth century A.D., it was apparently re-discovered
at Constantinople, and that city was for a long time defended by the use
of what is known in history as Greek Fire, an incendiary mixture very
similar to, if not actually the same as, gunpowder. But again the secret
of its composition was jealously guarded, and it was not until the
thirteenth century that it was discovered, apparently for the third
time, and introduced to Western Europe by Roger Bacon. It was used in
siege cannon early in the fourteenth century and in field guns at Crécy;
but it was apparently not employed for blasting until about 1627,
although in 1605, Guy Fawkes and his fellow-conspirators were able to
obtain it in large quantity.

From the battle of Crécy in 1346 to the beginning of the South African
campaign in 1889, gunpowder was the only explosive used in warfare.
“Villainous saltpetre” has therefore played a very important part in
shaping the course of events in the world’s history. At the present day,
gunpowder has become “old-fashioned.” In warfare, it has been superseded
by “smokeless” powders of much greater power; while for mining
operations, explosives with a much greater shattering effect have long
since taken its place.

The composition of gunpowder may vary, but on the average it contains 75
parts by weight of saltpetre to 15 of charcoal and 10 of sulphur. It is,
therefore, a mixture of two combustible substances, with a large
quantity of a third very rich in oxygen. The separate constituents are
very finely ground and afterwards thoroughly incorporated. When the
mixture is ignited, charcoal and sulphur burn very fiercely in the
oxygen supplied by the saltpetre.

The secret of the action of gunpowder lies in the extraordinary rapidity
with which combustion, started at one point, is propagated through the
whole mass. Moreover, the products of combustion are mainly gases, and
these occupy several thousand times the volume of the solid from which
they are produced. In a confined space, a gas may exert enormous
pressure when its normal tendency to expand is resisted.

Propellants. Although combustion is propagated through a quantity of
gunpowder with very great rapidity, it is not done instantaneously. The
time required is about one-hundredth of a second under ordinary
conditions, and this interval, short though it is, is very important.
When the object is to throw a projectile, the inertia of the latter has
to be overcome, that is, a certain amount of force has to be applied
before the heavy body begins to move. In order that the strain on the
breech of the gun may be as small as possible, the pressure must be
gradually developed and must reach its maximum just as the projectile
begins to move.

The time factor in the explosion constitutes the difference between what
we now call “propellants” and “high explosive.” Propellants are
explosives which develop pressure gradually, and are therefore used to
launch the projectile; high explosive develops pressure instantaneously,
and is therefore used as the bursting charge inside the shell, bomb, or
torpedo, and also in blasting operations.

Cordite, or smokeless powder, is the propellant now most used. It is
made by macerating guncotton and nitroglycerine with their common
solvent acetone. A pulp is thus made to which 5 per cent. of vaseline is
added. The mixture is then forced through a die, and in this way it is
formed into threads or rods, which harden as the acetone evaporates.
Cordite produces no smoke, because all the products of its combustion
are invisible gases.

High Explosive. _Nitroglycerine_ and _Guncotton_ are both explosives of
the instantaneous kind. The former is made by forcing glycerine, under
pressure in a very fine stream, into a mixture of fuming nitric and
concentrated sulphuric acids; the latter by soaking cotton-wool in a
similar mixture. Both products are washed with water until quite free
from acid, and subsequently dried.

Nitroglycerine is a colourless oil with a burning taste. The oil itself
is very dangerous to handle, for it is liable to explode spontaneously
even when the utmost care has been taken in its preparation. A mere spot
on a filter paper explodes with a deafening report when gently hammered
on an anvil; and one drop, when heated on a stout iron plate, blows a
hole through the plate. No use could be made of this substance for many
years after its discovery because it was so liable to explode during
transportation; now, however, it is made safer by mixing with absorbent
infusorial earth or _kieselguhr_. This mixture is known as dynamite.
Blasting gelatine, like cordite, is a mixture of nitroglycerine and
guncotton.

_Trinitrotoluene_ (T.N.T.) is made from toluene and nitric acid, and is
a type of the modern high explosive. It is a yellow crystalline
substance which melts at 79°-81·5° C., and is poured into the shell in a
molten condition. It is a remarkably stable substance, which burns
quickly when heated to 180° C.; it cannot be exploded even by hammering.
Explosion is only brought about by that of a subsidiary substance called
the detonator. The percentage composition of T.N.T. is as follows—

  Carbon                      33·5
  Hydrogen                     2·3
  Nitrogen                    19·5
  Oxygen                      44·7
                             100·0

The oxygen present is only just sufficient to burn the whole of the
carbon to carbon monoxide; but since carbon dioxide is also formed,
which requires twice as much oxygen for the same weight of carbon, and
since the hydrogen and nitrogen may also be oxidized, the combustion of
the carbon is not complete; and therefore the explosion of T.N.T. is
accompanied by a dense black smoke, consisting of finely divided
particles of carbon.

The explosive known as ammonal is a mixture of T.N.T., aluminium powder,
and ammonium nitrate; the function of the latter substance is to supply
more oxygen to render the combustion of the carbon of T.N.T. complete.

Nitrates and the Food Supply. Chemical analysis shows that compounds of
nitrogen enter largely into the composition of the living tissues of all
plants and animals; hence, either nitrogen itself or some of its
compounds must be assimilated by all living organisms to provide for
growth and development, and to repair wastage. Air, since it contains
approximately four-fifths of its volume of free nitrogen, is the most
obvious source of supply. At every breath, a mixture of oxygen and
nitrogen is inhaled by animals, but only part of the oxygen is used.
Practically the whole of the nitrogen is returned to the atmosphere
unchanged; it serves only to dilute the oxygen. From this it is clear
that animals do not build up their nitrogenous constituents from
elementary nitrogen.

With plants it is very much the same, for, although they obtain their
principal food, namely, carbon, from the carbon dioxide which is present
in air, it is only in a few exceptional cases that free nitrogen is
assimilated. The exceptions will be considered first, because it was
through these that we first began to learn something definite about the
great importance of nitrogen in agriculture.

Virgil, who was born in 70 B.C., wrote a poem in praise of agriculture.
Almost in the opening lines he deals with the treatment of corn land. He
advises that, in alternate years, this should either be left fallow or
sown with pulse, vetch, or lupin; but not with flax or oats, because
they exhaust the land. From this we learn that rotation of crops was one
of the established principles of good husbandry even at the beginning of
the Christian era.

It was not until the later years of the nineteenth century that any
explanation as to why rotation of crops is beneficial was put forward.
Let us first state the facts more precisely. Peas, beans, vetches,
clover, and other members of the natural order called _Leguminosae_,
which includes about 7,000 species, produce fruits rich in complex
nitrogen compounds without being dependent in any way upon nitrogen
compounds in the soil. Moreover, they do not exhaust the land as far as
these compounds are concerned; hence wheat and other grain can be grown
on the same land the following year.

It is now known that leguminous plants assimilate atmospheric nitrogen
with the help of certain bacteria. If anyone will dig up a lupin root,
he will observe[2] conspicuous wrinkled swellings or nodules at various
points on the roots. These, when examined with a high-power microscope,
are found to contain colonies of bacteria. It is these minute vegetable
organisms which assimilate nitrogen and pass on nitrogen compounds to
the larger plant. Other plants cannot assimilate what we might call raw
nitrogen; they require soluble nitrates. These they build up into
complex organic nitrogen compounds suitable for the feeding of animals
which can assimilate neither free nitrogen nor nitrates.

The Nitrogen Cycle. The supply of nitrates in the soil needs continually
to be renewed by the addition of decaying vegetable matter, stable or
farmyard manure, or Chili saltpetre. The natural manures contain organic
nitrogen compounds which were built up during the life of some animal or
plant. They are not immediately available as food for other plants,
because they are, as it were, the end products of life, and are not
soluble in water. But Nature provides for this. The manures decay,
forming humus, and ultimately ammonia, one of the simplest of inorganic
nitrogen compounds. Ammonia is then transformed to nitrites by certain
bacteria present in the soil, while other bacteria change nitrites into
nitrates. Both of these organisms are quite distinct from the root
nodule bacteria of the _Leguminosae_.

The nitrates pass into the plant in solution, and then begins again that
wonderful cycle of changes which we have described. This is perhaps made
clearer by the following diagram.

    [Illustration: Fig. 6.  THE NITROGEN CYCLE]

It now remains to show why artificial manures also are necessary. Let us
consider what happens to a piece of ground which is left uncultivated.
Although nothing is taken from it in the way of a crop, yet it very
quickly deteriorates, and the soil becomes infertile through the loss of
nitrogen compounds. This is explained by the fact that nitrates are
soluble in water, and so they get washed away from the top soil. In
addition to this, the nitrogen which is returned to the land forms quite
an insignificant fraction of that which is taken from it, for we waste a
great deal of organic nitrogen. The difference on both these accounts
has, therefore, to be made up by the addition of artificial manures
containing soluble nitrates.

The natural supply of nitrate is very limited. According to a report of
the Chilian Government published in 1909, the nitre beds of that country
were expected to last for less than a century at the current rate of
consumption. Wheat, above all things, will not grow to perfection on
soil which is deficient in nitrate. In 1908, Sir William Crookes called
attention to the difficulty which might be experienced in the near
future in supplying the people of the world with bread. Statistics
showed that wheat was grown on 159,000,000 acres out of a possible
260,000,000. The average yield is 12·7 bushels per acre. By 1931, it is
calculated that the population of the world will be 1,746,000,000; and
to supply these with bread, wheat would have to be grown on 264,000,000
acres, that is, 4,000,000 acres beyond the total available wheat land.

The remedy which Sir William Crookes suggested in order to avoid famine
was to raise the average yield from 12·7 to 20 bushels per acre by the
application of an additional 12,000,000 tons of Chili saltpetre per
annum. In view of the possible exhaustion of the supply of this
substance, this would only mean a postponement of the evil day. The
position, however, is now modified to a great extent because undeveloped
deposits of sodium nitrate are known to exist in Upper Egypt, and the
making of nitric acid from the air, which in 1908 was put forward as a
suggestion, is now an accomplished fact.

Nitric Acid from Air. The supply of nitrogen in the air is truly
inexhaustible; it amounts to about 7 tons for every square yard of the
earth’s surface, which is about 200,000,000 square miles. It is quite
evident that anything man may do in the way of taking nitrogen from the
air will make no perceptible difference to its composition.

Every time a flash of lightning passes between a cloud and the earth,
oxygen and nitrogen combine in the path of the spark, producing oxides
of nitrogen. These dissolve in water, and are washed into the earth as a
very dilute solution of nitric acid. As long ago as 1785, H. Cavendish
imitated this natural phenomenon. A reference to the diagram (Fig. 7)
will show how nitric acid can be made from the air on a small scale. The
globe contains air under slightly increased pressure. The platinum wires
or carbon rods are connected with the terminals of an induction coil,
which in its turn is connected to accumulators supplying the current
required.

When the coil is put into action, a spark passes across the gap between
the ends of the carbon rods. With a larger coil and a more powerful
battery, there is an arching flame which can be blown out and
re-lighted. This is actually nitrogen burning in oxygen. The result in
either case is the same; the air in the globe sooner or later acquires a
reddish-brown colour due to oxides of nitrogen, which, when shaken with
water, form a very dilute solution of nitric acid.

The same process is now carried out on a large scale. Air is driven by
fans through a very powerful electric arc, whereby 1·5 to 2 per cent. is
converted into nitric oxide. This combines spontaneously with more
oxygen to form nitrogen peroxide, which, when dissolved in water, gives
a very dilute solution of nitrous and nitric acids.

    [Illustration: Fig. 7. NITRIC ACID FROM AIR]

The absorption of the oxides of nitrogen is carried out systematically.
The mixed gases, after passing through the arc, are passed through a
series of towers filled with acid-resisting material over which a stream
of water is flowing. The solution of nitric acid so obtained is very
dilute, but by using the liquid over and over again, a moderately strong
solution is ultimately produced. This is collected in granite tanks and
neutralized with lime, forming calcium nitrate or Norwegian saltpetre,
as it is now called.

This is a new industry and a rapidly-growing one; in the course of five
years (1905-1909) the annual output of Norwegian or “air” saltpetre
increased from 115 to 9,422 tons. Mountainous countries like Norway and
Switzerland are perhaps in a specially favoured position with respect to
this industry. Rapid streams and waterfalls, in conjunction with
turbines, are used for driving the dynamos, and in this way electricity
is produced at very low cost. It is interesting, however, to note that a
plant for the manufacture of nitric acid from air has now been
established in Manchester.



                               CHAPTER IV
                           THE HALOGEN ACIDS


A group of acids, namely, hydrochloric, hydrofluoric, hydrobromic,
hydriodic, must now be considered together with their corresponding
salts. In appearance and in other physical properties they resemble one
another very closely; they are, therefore, called by the general name
“halogen acids.” This name is derived from the Greek word meaning
“sea-salt,” which is a mixture of the salts of these acids, and from
which the acids themselves can be obtained by treatment with oil of
vitriol.

Hydrochloric Acid. When concentrated sulphuric acid is added to common
salt, a gas is liberated which has a very pungent acid smell and taste.
This is a compound of the elements hydrogen and chlorine, and therefore
called hydrogen chloride. It is extremely soluble in water; a given
volume of water dissolves as much as 500 times its own volume of the
gas. The solution produced in this way is now called hydrochloric acid,
but formerly it was known as spirits of salt, or muriatic acid.

Hydrochloric acid has all the general properties of acids. It dissolves
many metals, such as zinc, iron, aluminium, and magnesium; hydrogen gas
is given off, and the chloride of the metal is formed. It also dissolves
limestone, marble, and all forms of calcium carbonate; carbon dioxide
gas is liberated, and a solution of calcium chloride remains.

The hydrochloric acid of commerce is obtained as a by-product in the
manufacture of washing soda from common salt by the method proposed by
Nicholas Leblanc towards the end of the eighteenth century. In the first
stage of this process, salt is mixed with sulphuric acid; this causes
the liberation of hydrogen chloride gas, which, when dissolved in water,
produces hydrochloric acid.

The past history of this branch of chemical industry is interesting.
Until about 1870, there was no very great demand for hydrochloric acid,
and in the early days of the working of the Leblanc process the soda
manufacturer took no pains to recover more than he could actually sell.
Consequently, a large quantity of hydrogen chloride gas was allowed to
escape into the air, with results which can well be imagined. For miles
around, great damage was frequently sustained by the growing crops; when
it rained in the neighbourhood of the works, the gas was washed out of
the air and, speaking quite literally, it rained dilute hydrochloric
acid, which rapidly corroded all stone and metal work. It is not,
therefore, surprising to learn that alkali makers were frequently
involved in litigation, and chemical works were regarded as a great
nuisance.

By the Alkali Act of 1863, chemical manufacturers were compelled to
prevent the escape of more than 5 per cent. of hydrochloric acid gas;
and by a subsequent Act, this limit was lowered to 0·2 grain per cubic
foot. The provisions of the Acts were not difficult to carry out,
because hydrogen chloride is extremely soluble in water.

The gases coming from the pans in which the salt was decomposed were led
into towers (see Fig. 8) built of bricks or Yorkshire flags soaked in
tar. These towers were filled up with coke or other acid-resisting
material, which was kept moist by water flowing from the tank F. In this
way, hydrogen chloride gas was removed and hydrochloric acid collected
in tanks (not shown in the figure) at the bottom of the towers. Even
then, there was no market for the greater part of the recovered acid,
consequently much of it found its way into drains and streams, and so
carried on its work of destruction in a less obtrusive way.

    [Illustration: Fig. 8. PREPARATION OF HYDROCHLORIC ACID]

By another piece of legislation, which at first sight seems to be wholly
unconnected with Chemistry, hydrochloric acid acquired a greatly
enhanced value. In 1861, the tax on paper was removed, and in the next
twenty years the demand for that commodity increased so much that raw
material both cheaper and more abundant than rag had to be found.
Esparto grass and eventually wood pulp proved successful substitutes.
There is really very little difference in composition between cotton and
linen rag on the one hand and wood fibre on the other, for both are
mainly composed of cellulose, which is a definite chemical compound.
Wood fibre is the less pure, and it is also coloured, and therefore has
to be bleached before it can be used for making white paper. It was this
circumstance which led to the greatly increased demand for hydrochloric
acid.

At the beginning of this chapter, it was mentioned, in passing, that
hydrogen chloride gas is a compound of hydrogen and chlorine. The latter
element is a very active bleaching agent, and is most easily obtained by
treating hydrogen chloride or its solution in water with pyrolusite
(black oxide of manganese), whereby the hydrogen is oxidized, forming
water, and chlorine gas is set free. Being a gas, chlorine is not
convenient to handle in large quantities; it is, therefore, converted
into bleaching powder, commonly but wrongly called chloride of lime.

Bleaching Powder. The manufacture of bleaching powder is carried out in
the following way. Slaked lime to the depth of 3 or 4 in. is spread over
the floor of a special chamber which can be made gas-tight. The lime is
raked up into ridge and furrow, and the chamber is filled with chlorine.
At the end of about twenty-four hours, the greater part of this chlorine
will have been absorbed by the lime. The chamber is then opened, the
lime is raked over to expose a fresh surface, and the process of
chlorination is repeated. Generally this is sufficient; the bleaching
powder should then contain about 35 per cent. of available chlorine.

The demand for bleaching powder is great and steadily increasing. The
price of 35 per cent. bleaching powder has never been less than about £5
a ton,[3] so that it is perhaps unnecessary to add that the absorption
of hydrogen chloride gas is now made so complete that it is well within
the requirements of the second Alkali Act.

Chlorides. The salts of hydrochloric acid are called chlorides, and the
most important of these is sodium chloride or common salt—a body that is
so well known that it need not be described here.

Although the quantity of this substance required for domestic purposes
is very large, it is, nevertheless, small by comparison with that which
is used for industrial purposes. It has already been mentioned that salt
is the starting-point for the manufacture of washing soda by the Leblanc
process, and, in addition to this, it is employed in the glass industry
to produce whiteness and transparency in certain kinds of glass; in
pottery, for glazing earthenware; in soap-making, for salting out the
crude soap; and in the dye trade as a mordant, and also for improving
the quality of certain colours. A full account of the salt industry is
given in another volume of this series.

Hydrofluoric Acid. When calcium fluoride (fluorspar, Derbyshire spar, or
blue-john) is warmed with concentrated sulphuric acid in a leaden dish,
hydrogen fluoride gas is evolved, and this, when dissolved in water,
gives hydrofluoric acid.

The peculiar property of this substance is that it has a very marked
corrosive action on glass. It cannot, therefore, be kept in glass
vessels, but must be stored in bottles made of hardened caoutchouc. On
the other hand, it is this same property which gives it its place in
commerce. As far back as 1670 it was used for etching on glass. The
process is a very simple one. The article is first coated with wax,
which is then removed in places by a sharp pointed tool. When exposed to
the action of the gas or its solution, corrosion takes place only where
the glass has been laid bare, the other parts being protected by the
wax. After a short interval, the wax can be melted off, and the design
made more distinct by rubbing in some opaque cement. For general trade
purposes, such as the stamping of lamp chimneys or electric light bulbs,
a quicker method is required. In this case, a preparation of
hydrofluoric acid which can be applied with a rubber stamp is used.

Fluorspar or calcium fluoride is the most important salt of hydrofluoric
acid. It is a commonly occurring mineral, and besides its use for the
preparation of the acid, it is employed in many metallurgical operations
to form a fusible slag.

Hydrobromic and Hydriodic Acids are not much used, but their salts, the
bromides and iodides respectively, are of great technical importance.
Silver chloride, bromide, and iodide, are sensitive to light, and mixed
with gelatine they form the emulsion which is spread over photographic
plates and papers. Potassium bromide and iodide are also well known to
photographers.

When the halogen salts of silver are exposed to light, an extremely
subtle chemical change takes place, which is only made apparent when the
plate or paper is developed. Then the silver salts on which the light
has fallen are reduced to metallic silver, and this reduction is
greatest where the light was most intense, and in other places is
proportional to the light intensity. A very faint image may appear on
the plate while it is in the developer, but generally the image is only
brought out clearly when the plate, film, or paper is placed in “hypo”
solution, which dissolves out the silver salts which have not been
changed, leaving the metallic silver unaffected.



                               CHAPTER V
                      CARBONIC ACID AND CARBONATES


Carbon. When any product of animal or vegetable life is strongly heated
in a vessel from which all air currents are excluded, a mixture of gases
and liquids is driven off, and a charred mass remains. This residue,
from whatever source obtained, is composed mainly of the element carbon.
It sometimes happens that a loaf of bread or a cake is left in the oven
and forgotten. In popular language it is then said to be “burnt to a
cinder”; in reality, the surface layers have been converted into carbon.

Carbonic Acid. If carbon is heated in an open vessel provided with a
good draught, it glows and in time disappears, because it combines with
oxygen to form an invisible gas, carbon dioxide or carbonic acid gas,
which, when dissolved in water, forms carbonic acid.

Compared with the acids which have been described in the foregoing
chapters, this is a very feeble acid; it changes the colour of litmus to
a wine red, not a bright pink; its taste is just pleasantly acid, and
its solvent action on metals and limestone is very small indeed. The
solution of the acid, obtained by passing carbon dioxide into water, is,
of course, very dilute, and it cannot be concentrated by evaporation,
since this only results in expelling the carbon dioxide from solution,
leaving pure water.

Soda Water. In the case of most gases, the weight which dissolves in a
given quantity of water is proportional to the pressure. This is true
for carbonic acid gas. Under a pressure of 4 atmospheres, the weight of
gas which dissolves is four times as great as under a pressure of one
atmosphere.

Soda water is water charged with carbon dioxide under pressure. This
pressure is maintained from the time it leaves the manufacturer to the
time it reaches the consumer by the strong walls of the syphon or
bottle. Immediately this pressure is released, the greater part of the
excess gas escapes, producing effervescence. It is, however, curious to
note that all the gas which ought to escape when the pressure is reduced
does not do so at once. If soda water is allowed to stand in an open
glass until it becomes “flat,” a brisk effervescence can be started
again by dropping a lump of sugar into the quiescent liquid. Soda water
remains supersaturated with gas for some time after the pressure has
been released.

Calcium Carbonate. The salts of carbonic acid are called carbonates.
Calcium carbonate is one of the most abundant substances in Nature. The
white cliffs of the east and south coasts of England, and those of
France across the intervening sea, are the exposed parts of enormous
beds of chalk or calcium carbonate. Whole mountain ranges in various
parts of the world are composed of limestone, which in some cases is
mainly calcium carbonate, and in others a mixture of this substance with
magnesium carbonate. Marble, whether white, black, or variegated, is
almost pure calcium carbonate, the differences of colour being due to
insignificant traces of iron and other foreign matter. In Iceland spar
and calc spar, sometimes called dog-tooth spar, we have two transparent
crystalline forms of this same substance.

Connected with the animal kingdom there are forms of calcium carbonate
no less varied in appearance. Egg shells are composed of this substance,
and so are oyster shells and the hard external coverings of some of the
lower animals. The mother-of-pearl lining of the oyster shell, and also
the pearl itself, are secretions of calcium carbonate. The beauty of the
last-named variety is due to the external form and to minute
inequalities of the surface, which cause the resolution of white light
into colours seen in the spectrum or in the rainbow. The coral reefs or
_atolls_ of the Southern oceans, which may be miles in breadth and
hundreds of miles in length, are all composed of calcium carbonate,
which a tiny marine animal has formed for its own support and
protection.

It is perhaps somewhat surprising at first to be told that all these
forms are composed of the same chemical substance, yet on this point the
evidence is definite and unmistakable. All the varieties dissolve
readily in dilute hydrochloric acid with effervescence caused by the
escape of carbon dioxide gas; moreover, if any of the purer forms, such
as pearl, marble, or Iceland spar, are heated to redness for some time,
they all lose about 44 per cent. by weight, leaving a residue which is
pure lime.

Quicklime. The making of lime from limestone or chalk is called lime
burning. The operation is carried out in a structure called a lime kiln,
which is usually a barrel-shaped vertical shaft surrounded by
substantial brickwork. There are two main methods of procedure, the one
continuous and the other intermittent. In the continuous process, the
kiln is filled up with limestone and fuel (generally coke) in alternate
layers. Combustion is started at the bottom and maintained by a
regulated draught. As the charge works down, the addition of limestone
and fuel is continued from the top, while the lime is removed from the
bottom of the kiln. The lime produced by this method has the ashes of
the fuel mixed with it. To avoid this, the more modern type of kiln has
four lateral fire grates outside the actual kiln.

For the intermittent method, a kiln is required which has a fireplace at
the bottom. Over this a rough arch is built of large pieces of
limestone, laid dry, and then the kiln is filled up with pieces of
limestone which decrease in size from below upwards. The fire is kindled
beneath the arch and urged by a regulated draught. The heating is
maintained for three days and nights, after which time the charge is
allowed to cool down.

Carbonic Acid Gas in Nature. Although the solvent action of carbonic
acid is very small compared with that of strong acids, it is
nevertheless great in comparison with that of water. This is shown
especially in its action on limestone, an action from which several
important consequences arise. Rain, as it falls through the air,
dissolves a little carbon dioxide and, although this is only an
exceedingly dilute solution of a very weak acid, its cumulative effect,
especially in limestone districts, is very great; it hollows out
enormous caves and causes the formation of those fantastic creations in
stone known as stalactites and stalagmites.

When a drop of water charged with carbonic acid gas falls on limestone,
it dissolves a little of that substance, forming calcium bicarbonate,
which may be regarded as a compound of calcium carbonate, carbon
dioxide, and water. Little by little, the solid rock is hollowed out and
a cave, or perhaps an underground watercourse, is formed.

Again, the drop of water charged with calcium bicarbonate may find its
way to the roof of a cave. As it hangs from the roof while it gathers
strength to fall, a little of the carbon dioxide escapes, and a minute
quantity of calcium carbonate is deposited. In this way, a stalactite
looking like an icicle in stone gradually grows downwards.

When the drop reaches the floor of the cave, a little time elapses
before it sinks into the ground; again a little carbon dioxide escapes,
and a small quantity of calcium carbonate is formed. Little is added to
little, and in the course of ages the stalagmite grows upward from the
floor and ultimately meets the stalactite to form a continuous column of
glistening crystallized calcium carbonate.

Hard and Soft Water. Water that is used for domestic or manufacturing
purposes is described as either hard or soft. Soft water produces a soap
lather almost at once; hard water forms at first a scum or curd which
has no detergent properties, and only after a time gives the soap lather
which is required. The difference is due to the relative amount of
dissolved solid contained in the water.

Only distilled water or rain water collected in the open country is
perfectly soft, for this is the only kind of water which on being
evaporated to dryness leaves no solid residue. In districts where the
underlying strata are composed of hard insoluble rock, such as granite
or millstone grit, the water contains very little dissolved matter and
is relatively soft. In a limestone or chalk country, water is very hard
and in many cases has to be softened either before delivery or before
use.

The chief impurities which cause hardness are the chlorides, sulphates,
and bicarbonates of magnesium and calcium. The chlorides and sulphates
are not affected in any way by boiling, and the hardness which is due to
them is said to be “permanent.” The bicarbonates, on the other hand, are
decomposed when the water is boiled, and then they cease to cause the
water to be hard. This part of the hardness is spoken of as “temporary”
hardness.

Let us now consider what calcium bicarbonate is and how it is formed. It
is a compound of calcium carbonate and carbonic acid, and is formed by
the solvent action of carbonic acid on limestone or chalk. The compound
is soluble in water; but when the solution is boiled, the carbonic acid
is broken up, carbonic acid gas is expelled from the solution, and
calcium carbonate is formed.

Temporary hardness is the more troublesome. In the first place, the
bicarbonates, especially that of calcium, often form the greater part of
the dissolved impurity. Moreover, when the water is boiled, although the
hardness is removed, the insoluble calcium carbonate is a source of
trouble, for it gradually settles down into the hard mass known as “fur”
in kettles and “scale” in boilers.

It is perhaps necessary at this point to emphasize the fact that matter
_suspended_ in water does not make it hard, and it is only matter which
is _dissolved_ which makes any difference in this respect.

Since the softening of temporary hard water by boiling has the
undesirable feature of introducing solid matter into the boiler, it is
customary now to treat this water chemically. The following is the
process most generally used. Quicklime or slaked lime is stirred into
the water until the mixture gives a faint brown coloration when a drop
of silver nitrate is added to a small test portion. Unsoftened water is
then added until a sample just ceases to give this test. The temporary
hardness has then been removed, and it is only necessary to allow the
suspended matter to settle.

The explanation of the method is as follows. The lime which is added
neutralizes the carbonic acid combined with the calcium bicarbonate, and
the result is the same as in the former case where this carbonic acid
was decomposed by heating, for calcium carbonate is thrown out of
solution.

For domestic purposes, water is softened by the addition of washing
soda. Since this reacts with all the calcium and magnesium compounds
forming the insoluble carbonates, all hardness, both temporary and
permanent, is removed.



                               CHAPTER VI
                  PHOSPHORIC, BORIC, AND SILICIC ACIDS


The acids which are grouped in this chapter are not in themselves of
much interest, though some of their salts are extremely important
compounds.

Bone. Much of the refuse bone, sooner or later, reaches the marine
store, and from that point starts on a career of usefulness in the
industrial world.

“Green bone,” as it is then called, may have fat adhering to it or
confined in its hollow interior as marrow. This is recovered by
treatment with benzine, and after that the bone is subjected to the
action of superheated steam in order to convert cartilage into glue. In
some cases, the residue is then ground up to make bone meal, which is
valuable as a manure because of the calcium phosphate which it contains.
In this way, the phosphate returns again to the animal kingdom, for it
supplies plants with the phosphates that they require, and from the
vegetable kingdom it passes to animals and helps to build up bone again.

Calcium Phosphate and Bone Black. Instead of being ground up, bone may
be heated in a retort in much the same way as coal is treated for the
manufacture of coal gas; bone oil is distilled off, and a non-volatile
residue, called bone black or animal charcoal, remains. This contains
about 90 per cent. of calcium phosphate and 10 per cent. of finely
divided carbon disseminated throughout the mass. It has the peculiar
property of absorbing colouring matter, and is used for this purpose in
the sugar industry and in the preparation of fine chemicals.

Phosphoric Acid. After being some time in use, bone black loses the
property of absorbing colouring matter; and though it can be “revived”
several times by heating it strongly in a closed retort, it ultimately
becomes spent and of no further use to the sugar refiner. It is then
heated again, this time in an open vessel, until all the carbon is burnt
away. The residue is now a greyish solid consisting mainly of calcium
phosphate. This, supplemented with native phosphate, which is probably
fossilized bone, is used for the preparation of phosphoric acid.

The salt is decomposed by sulphuric acid in wooden vats; calcium
sulphate is formed, and ultimately settles on the bottom of the vat,
leaving a clear supernatant liquid, which is a dilute solution of
phosphoric acid. This liquid is drawn off and evaporated to a syrup.
This is “syrupy” phosphoric acid. On being still more strongly heated,
the syrup loses still more water, and a semi-transparent glassy-looking
substance, called metaphosphoric acid, remains.

Superphosphate. All fertile soils, especially those on which wheat is to
be grown, must contain a certain amount of phosphate. With this, as with
all other plant foods, the actual percentage weight required in the soil
is very small indeed, but it is necessary that it should be disseminated
throughout the soil. Even distribution is very difficult to secure in
the case of a substance like calcium phosphate, which is practically
insoluble in water.

To get over this difficulty, calcium phosphate is converted into a
mixture known as “superphosphate” by the following process. Bone ash or
the mineral phosphate is finely ground and thoroughly mixed by machinery
with two-thirds its weight of sulphuric acid from the lead chambers.
After a time, this mixture sets to a hard mass, containing principally
gypsum and calcium tetrahydrogen phosphate. It is then ground up finely
and is ready for use.

The special modification of calcium phosphate contained in
superphosphate is soluble in water. It is, therefore, carried into the
soil in solution, and in this way very evenly distributed. In the soil
it reacts with the lime or chalk which is present, and is gradually
reconverted into insoluble calcium phosphate.

The manufacture of superphosphate is a very important industry. The
weight of the substance produced annually in Great Britain alone is not
far below a million tons.

Basic Slag. In the Bessemer process for converting iron into steel, cast
iron is melted up in a vessel called a converter and, by the aid of a
powerful blast blown through the molten iron, most of the impurities are
burnt off. If, however, phosphorus and sulphur are present, they are not
removed if the converter has a silica (acid) lining. The original
Bessemer process was, therefore, modified by Thomas and Gilchrist, and
the converter for this kind of iron is lined with dolomite and lime
(basic lining). Phosphorus is then converted into phosphate and retained
by the lining, which is subsequently removed, ground up finely, and sold
as “basic slag.”

Boric Acid, or boracic acid, is familiar because it is used in medicine
as a mild antiseptic; it is also employed as a preservative for food. It
is a white crystalline compound, sparingly soluble in water. It has no
well-marked taste, and causes only a partial change in the colour of
litmus solution; it is, therefore, one of the weak acids. It does not
dissolve metals, but it displaces carbon dioxide from carbonates,
forming salts.

Borax, the best known salt of boric acid, is used in laundry work and
also for making some enamels, for when it is strongly heated it loses
water, and ultimately melts down to a clear “glass” in which the oxides
of metals will dissolve, yielding transparent substances which are
beautifully coloured according to the nature of the oxide used. This
property is often made use of in chemical analysis in what is known as
the “borax-bead” test.

    [Illustration: Fig. 9. BORIC ACID]

Boric acid is a natural product; the method by which it is obtained is
of some interest, because it is so simple, and because it shows how mere
traces can be gradually accumulated until a very fair total is
ultimately obtained. Moreover, the method is copied directly from
Nature.

In the early years of the nineteenth century, certain jets of natural
steam, called _suffioni_, which issue from the earth in Tuscany, were
found to contain the vapour of boric acid. These jets of steam are of
volcanic origin. The quantity of boric acid in the vapour is very small
indeed; nevertheless, by the method which is adopted, it can be
profitably recovered, and more than a ton of the solid is daily
produced.

In the same country there are many lagoons, the water of which contains
boric acid. It was rightly conjectured that this boric acid came from
jets of steam which issued from the earth in the bed of the lagoon. This
suggested the idea of building up an artificial lagoon around a group of
jets.

Series of about five of these collecting basins (Fig. 9) are formed,
each one at a slightly lower level than the one which precedes it. The
first basin is filled with water from an adjacent spring, and this is
allowed to remain for twenty-four hours. A sluice is then opened and the
liquid contained in the first basin flows down to the second, where it
remains for another day, and so on until it reaches the last basin of
the series. The liquid by this time is almost fully charged with boric
acid, but it contains only about 2 per cent., because the acid is so
sparingly soluble in water.

From the last basin (A), the liquid runs into large vats (B, D), where
the suspended impurities settle down. The solution of boric acid is then
concentrated by causing it to flow over a broad inclined plane made of
corrugated lead or through a series of shallow vessels heated by jets of
natural steam. The hot liquid flows into another vat (C), and, as it
cools, boric acid crystallizes out and is removed by perforated ladles.

The mother liquor from which the crystals have been withdrawn is, of
course, a cold saturated solution of the acid, and this is returned to
the top of the incline to flow down again and lose more water. The boric
acid is finally transferred to drying chambers, which are also heated by
the natural steam.

Native borax or “tinkal” comes from Thibet and also from Ceylon. In
California, a large quantity of borax is obtained from a borax lake, and
also from the mud of marshes in its neighbourhood.

Silica. The element silicon does not occur in the free state in Nature,
neither has any particular use been found for it, and therefore it is
not often isolated except to provide a lecture specimen. The compounds
of silicon, however, are both plentiful and important, especially
silica, the oxide, and the silicates or salts of silicic acid.

The commonest forms of silica are sand, flint, and quartz. Silver sand
is composed of small crystals of pure silica, while flint is the
amorphous variety of the same substance. Quartz, or rock crystal, is a
very hard and transparent mineral. It forms six-sided prisms ending in
pyramids. It is distinguished from other common transparent minerals,
such as calcspar, by the fact that it cannot be scratched even with a
good knife or file, and that a drop of hydrochloric acid has no action
on it. The melting point of silica is very high.

Sometimes silica is very delicately coloured with minute traces of
metallic oxides and other substances, and these forms, because of their
rarity and beauty, are more highly valued. Smoky quartz, cat’s-eye, and
amethyst are some of the coloured varieties of quartz. Opal, agate,
jasper, onyx, and chalcedony are, in the chemist’s classification,
merely coloured flints.

In recent years, chemical apparatus has been made from pure fused
silica. This can only be worked in the oxy-hydrogen blow-pipe flame or
in the electric furnace; nevertheless, crucibles, flasks, beakers, and
retorts can be made. Silica ware has several advantages over glass,
notably, that water has no action upon it at all; moreover, its
coefficient of expansion is so very small that a piece of apparatus made
of silica can be suddenly heated or cooled without risk of fracture;
indeed, it can be made red-hot and cooled immediately by plunging into
cold water.

Quartz or silica fibres, used for suspending magnets and other bodies in
very delicate physical apparatus, are made in the following way. Molten
silica is attached to the bolt of a crossbow, which is then released
above a carpet of black velvet. As the bolt flies forward, it draws out
the silica into a filament, which is so fine that it would be difficult
to find were it not for the velvet background.

Silicic Acid itself is only of theoretical interest. It is obtained by
adding hydrochloric acid to a solution of potassium or sodium silicate.
It is a gelatinous substance of somewhat indefinite composition. It has
no effect on litmus, no taste, and no solvent action; in fact, it is
only recognizable as an acid because it dissolves in alkalis, forming
salts called silicates. It is one of the weakest acids known.

The natural silicates are very abundant and varied; orthoclase or potash
felspar, and albite or soda felspar, are those which most commonly
occur. The former is potassium aluminium silicate, and the latter,
sodium aluminium silicate. Iron is generally present in both as an
impurity. The weathering of the felspars, in conjunction with the action
of water, has produced the clays. In this way, pure white China clay has
been formed from felspars which contain little or no iron, and the
coarser kinds of clay from others containing a greater proportion of
foreign substances.

Mica, which is used for making lamp chimneys, is a potassium aluminium
silicate. Asbestos, meerschaum, beryl, garnet, jade, and hornblende are
all silicates of various metals.

Glass is a complex mixture of insoluble silicates with excess of silica.
The varieties in common use are soda glass, Bohemian glass, and lead
glass (which is also called flint glass). Soda glass is mainly a mixture
of calcium and sodium silicates, and is distinguished by its low melting
point, which makes it easy to work at moderate temperatures. It appears
in commerce as plate glass, window glass, and common bottles. Bohemian
glass contains calcium and potassium silicates, and has a high melting
point. It is used for making chemical apparatus. Lead or flint glass
contains the silicates of lead and potassium; this is a dense glass, but
at the same time rather soft. It takes a high polish and is used for
making ornamental or cut-glass ware.

Remembering that glass is composed of the salts of silicic acid, the
reader will readily understand that the mixture from which it is made
must contain acidic and basic constituents. The acidic or acid-forming
material is in every case silica or sand. This must be pure, and for all
but the commonest kind of bottle or window glass, it must be free from
iron, otherwise the glass will have a more or less pronounced greenish
colour. It must also be fine and even grained. Formerly, the glass sands
used in this country came from Holland and Belgium, but now supplies
from several British sources are being successfully used.

The basic portion of the glass mixture differs according to the kind of
glass required. An average mixture for soda glass contains sand, 20
parts; salt cake (sodium sulphate), 10 parts; quicklime, 5 parts;
charcoal, 1 part. For Bohemian glass, pearl ash (potassium carbonate)
takes the place of salt cake, and no charcoal is necessary because the
materials used are finer. For lead glass, the mixture is still further
modified by the use of litharge, or more often red lead, in place of
lime.

The ingredients are well mixed and thoroughly dried. Waste glass from a
previous batch is also added. The mixture is heated to about 1200° C. in
large pots made of Stourbridge clay, and the heating is continued for as
much as sixteen hours, and until the whole of the material in the pot is
molten and fairly mobile. Scum or glass-gall is removed, and when gas
bubbles have disappeared, the temperature is allowed to fall to
700°-800°, when the glass becomes sufficiently viscous for subsequent
working. The semi-fluid mass is then blown, moulded, or drawn, according
to the kind of article that is required.

The physical properties of glass will now be considered in order that we
may be able to account for its extended use. Such an inquiry as this,
especially in the case of materials in common use, is often interesting,
because it frequently happens that the special property upon which we
set so much value is an abnormal one and, consequently, the feature
which we take for granted is precisely the one into which we should
inquire most closely.

The most striking feature of glass is its transparency. This property is
abnormal, if glass is a solid. Consider what happens in most cases. A
substance like nitre melts easily and in the molten state is perfectly
transparent; when it cools, crystals form and, though these individually
may be transparent, yet the solid mass is opaque. The reason for this is
that the solid is not optically homogeneous, and therefore a ray of
light cannot pass through it in a straight line. At each facet of a
crystal light is deviated and reflected, and in the end is almost wholly
scattered. Consequently, an object, even if it can be seen at all, can
be discerned only in a blurred and indistinct fashion through such a
medium.

There are very good reasons, however, for supposing that glass is not a
true solid but an extremely viscous liquid. If glass is heated, it
softens and begins to flow very sluggishly at first, but afterwards more
readily. There is no abrupt change, as there generally is in passing
from the solid to the liquid state. Similarly in cooling, there is no
point at which it is possible to say that the glass is solidifying. The
view that this substance is really a liquid is perhaps a little
startling at first, but it becomes less so when we observe that a long
glass rod supported at its ends in a horizontal position sags in the
middle and is permanently deformed.

To avoid that change which would be technically called solidification by
a scientist, the article which has been fashioned in glass is cooled
down very slowly and gradually. This part of the process is called
annealing; it may occupy some days in extreme cases, and it points to
the fact that experience has shown that it is necessary to guard against
some change which would normally take place if this precaution were
neglected.

The change in glass which annealing is intended to prevent is known as
devitrification. In spite of all precautions, this does occur sometimes,
and specimens of old window glass are often seen to have lost their
transparency completely and to have an opalescent sheen. In these cases,
the silicates have crystallized.

An extreme case of badly annealed glass is illustrated by Rupert’s
drops, a scientific curiosity of very old standing. These are “tears” of
glass made by dropping the molten substance into water. When the tail of
the drop is nipped off, the whole thing is shattered to powder with
something like explosive violence. Clearly there is a very great
internal strain, due to the fact that the outer parts have solidified
and contracted, while the inner part is still warm and dilated.

Another remarkable feature of glass is the ease and simplicity with
which it can be fashioned into articles of various shapes. As a plastic
material, molten glass almost ranks with clay. This again is due to the
property of passing through a viscous state, that is, one which is
intermediate between a solid and a liquid.

Water Glass, or soluble glass, is mainly sodium silicate. It is made by
fusing sand or powdered flint with caustic or with mild soda; sometimes,
by digesting crushed flint or chert with caustic soda solution under
considerable pressure in autoclaves or specially constructed boilers. In
the latter case, no extraction is necessary; but in the former, the
residue is treated with water and the solution evaporated until it
becomes a viscous transparent liquid.

This liquid is used in various ways in industry. It is added to the
cheaper varieties of yellow soap, and is employed as a mordant in dyeing
and printing calico. An artificial sandstone is made by mixing sand,
calcium chloride, and sodium silicate; the two last-named substances
interact to form calcium silicate, which is insoluble in water. For
domestic purposes, water glass is best known in connection with the
preserving of eggs. When the film of water glass dries on the surface of
the egg shell, the latter becomes impervious to air.



                              CHAPTER VII
                             ORGANIC ACIDS


Organic Chemistry. About a century ago, when the science of Chemistry
was still in its infancy, several substances were known which could then
only be obtained from animals or plants. The composition of these
substances was not understood, and they were not classified; moreover,
since none of them had ever been prepared artificially, it was supposed
that it was impossible to do this—the reason given was that “vital
force” was necessary for their production. In time, however, some of the
most typical animal and vegetable products were prepared in the
laboratory, and the belief in vital force disappeared.

In later times it was proved that substances like sugar, starch, urea,
indigo, and a great many more, all contain the element carbon. At the
present time, more than 100,000 compounds of this element are known; and
since they resemble one another, and at the same time differ in several
important respects from the compounds of other elements, it is both
natural and convenient that they should be classed together and studied
separately. This branch of Chemistry is called organic. It must not,
however, be supposed that all organic compounds are necessarily produced
by some living organism. A great many are, but there are many more which
are purely synthetic products.

Inorganic Chemistry includes all the other elements and their
derivatives. The _element_ carbon, and also some of its simpler
compounds, such as carbon monoxide, carbon dioxide, carbonic acid, and
carbonates, are more appropriately placed in the inorganic section.

The acids which have been considered up to this point are all inorganic
acids, and those which follow are organic. Sulphuric, nitric, and
hydrochloric acids are often distinguished as the mineral acids in
contradistinction to oxalic, citric, tartaric, and some others which
were first obtained from unripe fruits and therefore called vegetable
acids.

Organic acids have all the general properties of the class, but they are
much weaker than the mineral acids mentioned above. This is shown by
their solvent action on metals, oxides, and carbonates, which is in all
cases slight.

Vinegar is the trade name for what is essentially a dilute solution of
acetic acid which has been made by the acetous fermentation of
saccharine fluids containing weak alcohol. In addition to acetic acid,
vinegar contains minute quantities of a large number of compounds. Some
of these help to produce that agreeable flavour and aroma which
distinguishes vinegar from diluted acetic acid. The nature and quantity
of the flavouring constituents depend mainly upon the nature of the
alcoholic solution used.

Since the acetic acid in vinegar is always produced by fermentation, all
processes for the manufacture of vinegar are essentially arrangements
for promoting the vigorous growth and development of _Mycoderma aceti_,
the organism which produces the vinegar ferment.

Like all other plants, _Mycoderma aceti_ will flourish only under
certain favourable conditions. In the first place, it requires
nourishment, and therefore certain nitrogen compounds and salts must be
present in the alcoholic solution. These are contained in wines, beer,
cider, and malt liquors, but not in spirits of wine, which is pure
alcohol distilled from liquids which have undergone vinous fermentation.
If the plant is placed in dilute spirits of wine, only a very little
acetic acid is formed, and then the action ceases because the solution
does not contain the necessary food substances. Temperature also has a
very marked effect on growth, the most favourable range being between
68° and 95° F.

Alcohol is changed to acetic acid by the process of oxidation, and
therefore, in making vinegar, arrangements have to be made to bring
together weak alcohol and air in the presence of the plant. The ferment
which is secreted by the plant then causes an acceleration of the
reaction. There is a considerable amount of similarity between
fermentation and contact action. In this connection, it is interesting
to note that the conversion of alcohol into acetic acid can also be
brought about by exposing a mixture of alcohol vapour and air to the
action of platinum black; in fact, there is one process for making
vinegar in this way.

French Vinegar. New wine, especially that which contains a low
percentage of alcohol, is liable to many kinds of “sickness.” It may
turn bitter, it may turn sour, or it may undergo what is called lactic
fermentation. In either case, it becomes unsaleable as a beverage. Wine
which has turned sour is the best material for making vinegar, and when
this is done by the French or slow process, a product with a very fine
_bouquet_ is obtained.

The methods adopted are very simple. Formerly, the wine was poured into
barrels leaving the top portion empty, and providing for a current of
air over the surface. The barrels were often set up in rows in the open
air in an enclosure which was then known as a “vinegar field.” The
process of souring which had already begun went on naturally, and in the
course of a few months, nearly the whole of the alcohol was converted
into acetic acid.

The process now in use in some of the French factories is somewhat
similar. Large casks holding about 100 gallons are set up in a room, and
provision is made for keeping the temperature uniform. Each cask is
first acidulated by allowing strong vinegar to stand in it until the
vinegar plant has developed on the surface. The casks are then filled up
very gradually by adding a few gallons of wine every eight or ten days.
When the cask is full, a fraction of the contents is drawn off and
replaced by wine. The process then becomes continuous, until it is
necessary to clean out the generator and start again.

In recent times, the manufacture of wine vinegar has been carried out on
more scientific principles. The vinegar plant is actually cultivated and
examined microscopically before being used, in order to make sure of the
absence of moulds and bacteria, which set up other fermentations,
producing substances which affect adversely the taste and aroma of the
finished product. The cultivated ferment is then added to the wine in
shallow vessels and the process is carried on as described above.

Malt Vinegar. A dilute solution of alcohol which is made from malt by
fermentation with yeast contains the nutritive substances necessary for
the growth of the vinegar plant, and can therefore be used as a
starting-point for the manufacture of vinegar. Sprouted barley or malt
is mixed with oats, barley, rice, or other starch-containing material.
The mixture is mashed with warm water and then fermented with yeast,
giving what is called “raw spirit.” This is converted into vinegar by
the “quick” process.

The vinegar generator (Fig. 10) is a large barrel divided into three
compartments by two perforated partitions. The lower disc is fixed about
one-third of the way up the barrel, and near it holes are bored to admit
air. The upper disc, fixed near the top of the barrel, is perforated
with a large number of small holes which are partially stopped up with
short threads or wicks, which hang from the under side. The space
between the two discs is packed with specially prepared beech shavings,
which have been left to stand in strong vinegar until they are covered
with the vinegar plant.

    [Illustration: Fig. 10. QUICK VINEGAR PROCESS]

The weak spirit is delivered into the upper portion of the barrel and is
distributed in very small drops by the threads; it then passes slowly
over the vinegar plant, to which the air also has free access. When it
reaches the bottom, it overflows into a reservoir and is again passed
through the generator; this is repeated until the product contains the
desired amount of acetic acid.

The principle of the quick vinegar process is the same as that employed
in making wine vinegar. The speed of the reaction is, however, greatly
increased by having the ferment spread over a very large surface and by
the free circulation of air. It is possible to make wine vinegar by the
quick process, but it is not done, because the product is inferior in
taste and aroma to that made by the slow process.

Both wine vinegar and malt vinegar when freshly prepared have a
stupefying and unpleasant odour. Before the product is ready for the
market, it has to be matured in barrels. During this process, a small
quantity of alcohol which still remains in the vinegar combines slowly
with some of the acetic acid, producing acetic ester, a substance which
has a pleasant fruity odour.

The colour of wine vinegar is natural, but vinegar which is produced by
the quick process is colourless or only faintly coloured. Since the
public has a preference for vinegar which is brown in colour, the
product of the quick process is coloured artificially, either by adding
caramel or by preparing the weak spirit from malt which has been
slightly charred in drying.

Industrial Acetic Acid. The solutions of acetic acid dealt with above
would be too dilute for any industrial purpose; moreover, the acid can
be obtained much more cheaply by the distillation of wood. When wood is
subjected to a high temperature, it is converted into charcoal and, at
the same time, an inflammable gas, an acid liquid, and tar are given
off, and can be collected in suitable vessels. The following table, on
page 73, gives the relative amounts of the various substances obtained
from wood by dry distillation. The quantities are those derived from one
cord, that is, 125 cu. ft.

            _Charcoal   _Alcohol   _Calcium   _Tar in   _Wood oil  _Turpentine
                in         in      acetate   gallons._      in       gallons._
            bushels._  gallons._  in lbs._              gallons._
  Hard        40-50      8-12      150-200     8-20
    woods
  Resinous    25-40       2-4      50-100      30-60      30-60    Heavy woods
    woods                                                            12-25
                                                                   Light woods
                                                                     2-10
  Sawdust     25-35       2-4       45-75

The aqueous liquid that distils over contains methyl alcohol (wood
spirit), acetone, and acetic acid. The crude mixture is known as
pyroligneous acid. This is neutralized with milk of lime or soda ash,
which converts acetic acid into calcium or sodium acetate, but has no
action on the methyl alcohol and acetone which are also present. The
mixture is then distilled, when methyl alcohol, acetone, and water pass
over into the distillate, leaving the acetate in the retort.

To obtain the free acid from the acetate, the latter is well dried and
then distilled with concentrated sulphuric acid. Acetic acid, being the
more volatile of the two acids, distils over, and is nearly pure.

The method of removing the last traces of water depends upon the fact
that acetic acid solidifies at 17° C. The acid, which is nearly, but not
quite, free from water, is cooled until a portion solidifies. The part
which still remains liquid is poured away, and the process is repeated
until a residue is obtained which solidifies as a whole. This is glacial
acetic acid, so called because it is a mass of glistening plates which
look like newly-formed ice.


                              The Acetates

Aluminium Acetate, made by dissolving alumina in acetic acid, is the
“red liquor” which is used as a mordant in dyeing. It is a colourless
liquid, but is called “red liquor” because it is used with dyes which
give a red colour.

Ferrous Acetate, made in a similar way from scrap iron and acetic acid,
is the “black liquor” used in dyeing.

Verdigris, or basic copper acetate, is a valuable pigment. It is made by
interposing cloths soaked in vinegar between plates of copper. After the
action has been allowed to go on for a long time, the plates are washed
with water and the verdigris is scraped off. The finest verdigris is
made in France in the wine-producing district around Montpellier. Here,
instead of cloths soaked in vinegar, the solid residue from the wine
presses is spread in layers between the copper plates. The product made
in this way is called _vert de Montpellier_.

    [Illustration: Fig. 11. DUTCH PROCESS FOR WHITE LEAD]

Verdigris, like all the copper compounds, is extremely poisonous. It is
very liable to be formed on the surface of copper utensils used for
cooking purposes.

Lead Acetate, or sugar of lead, is used in large quantities in the
colour industry for making various reds and yellows. It is prepared by
dissolving the metal or its oxide (litharge) in acetic acid.

The slow action which acetic acid vapour has upon the metal lead finds a
very interesting application in what is known as the Dutch process for
the manufacture of white lead[4] for paint. The metal is cast into grids
or spirals, which are placed on the shoulders of the specially made pots
sketched in Fig. 11. A little dilute acetic acid is poured into each of
the pots, which are then arranged side by side on a thick layer of tan
bark, stable manure, or other material which will heat by fermentation.
The first layer of pots is then boarded over; another layer of pots is
placed upon this, and so on, tier upon tier, until the shed is quite
full. The heat developed by the fermenting material vaporizes the acetic
acid, and this vapour corrodes the lead, forming basic lead acetate. The
carbon dioxide which is also produced during fermentation converts the
acetate into the carbonate, which falls as a heavy white powder into the
pots.

Future Supply of Acetic Acid. When all the operations involved in the
production of acetic acid from wood, from the felling of the tree to the
final separation of the glacial substance, are taken into consideration,
it will be readily understood how it is that this acid has never been
cheap when compared with other acids used on an equally large scale. In
addition to this, the competition for wood for paper-making and for the
very numerous cellulose industries is rapidly increasing. It is,
therefore, not surprising to learn that chemists have turned their
attention towards the discovery of newer and cheaper methods of making
acetic acid.

Such a process seems to have been worked out in Germany. The
starting-point is acetylene gas made by the action of water on calcium
carbide. When this gas is passed through sulphuric acid containing
suspended mercuric oxide or dissolved mercury salt, the acetylene is
oxidized first to aldehyde and then to acetic acid.

If this process should prove to be successful, it will form the
starting-point of a new and important industry, for, apart from the
large amount of acetic acid which is used in commerce, there is the
production of the very important solvent known as acetone, which can be
made from acetic acid by a very simple operation.

Tartaric Acid. Grape juice contains a large quantity of potassium
hydrogen tartrate dissolved in it; when the liquid is fermented and
alcohol is formed, this salt crystallizes out because it is not soluble
in alcohol. After the new wine has been poured off, the salt is found as
a brownish crystalline residue adhering to the sides of the vat. Also
the salt goes on crystallizing after the wine is put into barrels, and
forms an incrustation on the sides. This is called the _lees_ or
sediment of wine. In commerce, the substance is known as _argol_
(sometimes spelt _argal_), and also _tartar_ of wine.

Crude argol is purified by dissolving it in water and destroying the
colour by boiling with animal charcoal. When the clear liquid obtained
from this mixture by filtration is evaporated, a white crystalline
substance separates out. This is potassium hydrogen tartrate or _cream
of tartar_.

Tartaric acid is obtained from cream of tartar. The salt is dissolved in
water and nearly neutralized with milk of lime. Insoluble calcium
tartrate is precipitated, and potassium tartrate remains in solution. A
further quantity of calcium tartrate is obtained by adding calcium
chloride to the solution just mentioned. The two precipitates of calcium
tartrate are then mixed and decomposed by dilute sulphuric acid, and
after the calcium sulphate is filtered off, tartaric acid is obtained as
a solid by evaporating the clear liquid.

The general properties of tartaric acid are well known. It is soluble in
water, giving a solution which has a pleasantly acid taste.

Citric Acid. The sharp flavour of many unripe fruits is due to the
presence of citric acid; the juice of lemons contains 5-6 per cent. of
the acid. The free acid is obtained in a manner precisely similar in
principle to that described for tartaric acid.

Oxalic Acid. Oxalic acid and its salts, the oxalates, are very widely
distributed in the vegetable kingdom. These compounds are present in
wood sorrel (_Oxalis acetosella_), in rhubarb, in dock, and in many
other plants. The acid is made on a large scale by mixing pine sawdust
to a stiff paste with a solution containing caustic soda and potash. The
paste is spread out on iron plates and heated, care being taken not to
heat the mixture to the point at which it chars. The mass is then
allowed to cool, and is mixed with a small quantity of water to dissolve
out the excess of alkali. This is recovered and used again.

Sodium oxalate, which is the main product of the reaction described
above, is dissolved in water and treated with milk of lime, whereby
insoluble calcium oxalate is obtained, which is subsequently decomposed
with sulphuric acid, yielding oxalic acid.

Potassium hydrogen oxalate is sometimes called _salts of sorrel_, and
potassium quadroxalate, _salts of lemon_. The most familiar use of the
latter substance is in the removal of ink stains.

Oxalic acid and its salts are poisonous. The free acid has sometimes
been mistaken for sugar with fatal results.

Formic Acid (_L. formica_, an ant) is found both in the vegetable and in
the animal kingdom. If the leaf of a stinging nettle is examined with a
microscope, it is seen to be covered with long pointed hairs having a
gland at the base. This gland contains formic acid. When the nettle is
touched lightly, the fine point of the hair punctures the skin, and a
subcutaneous injection of formic acid is made, which quickly raises a
blister.

The inconvenience which arises from the stings of bees and wasps, also
from the fluid ejected by ants when irritated, is due to formic acid.
The remedy in each case is the same; the acid must be neutralized as
quickly as possible with mild alkali, such as washing soda.

Formic acid was first made by distilling an infusion of red ants. It is
now made from glycerine and oxalic acid.

The Fatty Acids. Animal fats and vegetable oils are similarly
constituted bodies. They are composed mainly of three chemical compounds
known as stearin, palmitin, and oleïn. Of these, stearin and palmitin
are solids at ordinary temperatures, while oleïn is a liquid. Hard fats
like those of mutton and beef are composed mainly of stearin; fats of
medium hardness contain stearin, palmitin, and some oleïn; while oils
such as cod-liver oil and olive oil are nearly pure oleïn.

Stearin, palmitin, and oleïn are analogous in composition to salts.
Their proximate constituents are glycerine and certain organic acids,
stearic, palmitic, and oleïc respectively.

In order to obtain the fat free from tissue which it contains in its
natural state, it is tied up in a muslin bag and heated in boiling
water. The fat is squeezed out through the meshes of the fabric and
floats on the surface of the water as an oil which solidifies on
cooling. This clarified fat is called tallow.

All fats and vegetable oils can be resolved into their two constituents,
the acid and the glycerine. This can be brought about by heating the fat
with water to about 200° C. This operation must be carried out in a
vessel capable of withstanding pressure and closed with a safety valve;
otherwise, the requisite temperature could not be obtained. After this
treatment, there is left in the vessel an oily layer which solidifies on
cooling and an aqueous layer which contains the glycerine. The
solidified oily layer is the fatty acid. In the case of mutton or beef
tallow, it would be mainly a mixture of stearic and palmitic acids. This
mixture is used to make “stearin” candles. The acids themselves are
wax-like solids without any distinctive taste. Stearic acid melts at 69°
C. and palmitic at 62° C. They have no perceptible action on the colour
of litmus, neither have they any solvent action on metals or carbonates.
We should not recognize these substances as acids at all were it not for
the fact that they combine with alkalis, forming salts.

The salts of the fatty acids are called soaps. To make soap, the fat is
boiled with caustic alkali or caustic lye, as it is more often called.
This breaks the fat up primarily into the acid and glycerine; but in
this case, instead of obtaining the acid as the final product as we did
above by heating with water under pressure, we get the sodium or
potassium salt of the acid according to the alkali used. When caustic
soda is used, the product is a hard soap; when caustic potash is used,
it is a soft soap. The treatment of fats in this way with caustic
alkalis is called “saponification.”



                              CHAPTER VIII
                              MILD ALKALI


Caustic and Mild. There are two classes of alkalis distinguished by the
terms caustic and mild. If a piece of all-wool material is boiled with a
solution of caustic soda or potash, it dissolves completely, giving a
yellow solution. Mild alkali will not dissolve flannel, though it may
have some slight chemical action causing shrinkage. Partly for this
reason, and partly because commercial washing soda often contains a
little caustic soda, woollen garments must not be boiled or even washed
in hot soda water.

The disintegrating action of the caustic alkalis is also illustrated by
the use of caustic soda in the preparation of wood pulp for paper
making. Tree trunks are first torn up and shredded by machinery; but
notwithstanding the power of modern machinery, the fibre is not nearly
fine enough for the purpose until it has been “beaten” with a solution
of caustic soda, whereby the pulp is brought to a smooth and uniform
consistency like that of thin cream.

Mild Soda and Potash. Until the middle of the eighteenth century, it was
thought that the soluble matter extracted from the ashes of all plants
was the same. In 1752 it was shown that the substance obtained in this
way from plants which grew in or near the sea differed from that from
land vegetation by producing a golden yellow colour when introduced into
the non-luminous flame of a spirit lamp, while that from land plants
gave to the flame a pale lilac tinge. The former substance is now known
as mild soda, and the latter as mild potash.

At this point it is well to make it clear to the reader that there are
two bodies commonly called soda, and two called potash. One of each pair
is caustic and one mild.

By a simple chemical test it is easy to distinguish a mild from a
caustic alkali. When a little dilute acid is added to the former, there
is a vigorous effervescence caused by the escape of carbon dioxide, but
no gas is given off when a caustic alkali is treated in the same way.
The liberation of carbon dioxide on the addition of acids shows that the
mild alkalis are carbonates.

Washing Soda is so well known, that very little description of its
external characteristics is necessary. It is a crystalline substance,
easily soluble in water. The crystals, when freshly prepared, are
semi-transparent; but after exposure to air for some time, they are
found to lose their transparency and to become coated with an opaque
white solid which crumbles easily. This change in appearance is
accompanied by a loss in weight.

Crystals of soda melt very easily on the application of heat and, on
continued heating, the liquid seems to boil. When this operation is
carried out in a vessel attached to a condenser, the vapour that is
given off from the melted soda condenses to a clear colourless liquid
which, on examination, proves to be water. When no more water collects
in the receiver, the vessel contains a dry, white solid, which by any
chemical test that may be applied is shown to be the same as washing
soda, but it contains no water of crystallization and has a different
crystalline form. This substance is anhydrous sodium carbonate, or soda
ash as it is called in commerce. When soda ash is mixed with water, it
combines with about twice its own weight of that liquid, forming soda
crystals again.

Washing soda, then, contains nearly two-thirds of its weight of water.
Some of this water is given off spontaneously when the soda is exposed
to air; the water may even be said to evaporate. This accounts for the
loss of weight observed and also for the formation of the white layer of
partially dehydrated soda over the surface of the crystal. The property
of losing water in this way is common to most crystals containing a high
percentage of water of crystallization. The phenomenon is known as
“efflorescence.” It may here be observed that crystals of washing soda
which have become coated over in this way contain relatively more soda
than those which are transparent.

Natural Soda. In Egypt, Thibet, and Utah, there are tracts of country
where the soil is so impregnated with soda that the land is desert. The
separation of the soda from the earth is a simple operation, for it is
only necessary to agitate the soil with water and, after the insoluble
matter has settled down, to evaporate the clear solution until the soda
crystallizes out.

In addition to alkali deserts, there are also alkali lakes. Those in
Egypt are small, nevertheless, about 30,000 tons of soda per annum are
exported from Alexandria. Owens Lake in California is said to contain
sufficient soda to supply the needs of North America; while in the East
African Protectorate, beneath the shallow waters of Lake Magadi
(discovered in 1910), there is a deposit of soda estimated at
200,000,000 tons.

The Leblanc Process. At the present time, the greater part of the
world’s supply of soda is made from common salt by two processes. The
older of these, which is known as the Leblanc process, was introduced in
France towards the end of the eighteenth century. In those days soda was
very dear, for the main supply came from the ashes of seaweeds;
wherefore the French Academy of Sciences, in 1775, offered a prize for
the most suitable method of converting salt into soda on a manufacturing
scale. The prize was won by Nicholas Leblanc, who in 1791 started the
first soda factory near Paris. These were the days of the French
Revolution; the “Comité de Sûreté Général” abolished monopolies and
ordered citizen Leblanc to publish the details of his process.

    [Illustration: Fig. 12. SALT CAKE FURNACE]

The first alkali works were established in Great Britain in 1814. The
total amount of soda now made in this country every year is about
1,000,000 tons, of which nearly one-half is still made by the Leblanc
process.

Salt Cake. The first stage of the Leblanc process consists in mixing a
charge of salt weighing some hundredweights with the requisite amount of
“chamber” sulphuric acid. The operation is carried out in a circular
cast-iron pan (D, Fig. 12) about 9 ft. in diameter and 2 ft. deep. The
pan is covered over with a dome of brickwork, leaving a central flue (E)
for the escape of hydrochloric acid gas which is produced. At first, the
reaction takes place without the application of heat, but towards the
end the mass is heated for about one hour. The contents of the pan are
then raked out on to the hearth of a reverberatory furnace (_a_, _b_)
and more strongly heated. More hydrochloric acid gas is given off, and
the reaction is completed. The solid product which remains is impure
Glauber’s salt (sodium sulphate), and is known in the trade as “salt
cake.”

Black Ash. In the second stage of the Leblanc process, salt cake is
converted into black ash. The salt cake is crushed and mixed with an
equal weight of powdered limestone or chalk and half its weight of coal
dust. This mixture is introduced into a reverberatory furnace (Fig. 13)
by the hopper K, and heated to about 1000° C. by flames and hot gases
from a fire at _a_. During this operation, the mass is kept well mixed,
and after some time it is transferred to _h_ where the temperature is
higher. The mixture then becomes semi-fluid and carbon monoxide gas is
given off.

    [Illustration: Fig. 13. BLACK ASH FURNACE]

The formation of carbon monoxide within the semi-solid mass renders it
porous. This is an advantage, because it greatly facilitates the
subsequent operation of dissolving out the soluble sodium carbonate. The
appearance of the flames of carbon monoxide at the surface of the black
ash indicates the end of the process. The product is then worked up into
balls and removed from the furnace.

The chemical changes which take place in making black ash are probably
as follows: Carbon (coal dust) removes oxygen from sodium sulphate,
which is thus changed to sodium sulphide. This substance then reacts
with the limestone (calcium carbonate), forming sodium carbonate (soda)
and calcium sulphide.

Extraction of Soda. It now only remains to dissolve out the soda from
the insoluble impurities with which it is mixed in the black ash. It is
evident that the smaller the amount of water used for this purpose the
better, because the water has subsequently to be got rid of by
evaporation. The process of extraction is, therefore, carried out
systematically. The black ash is treated with water in a series of tanks
which are fitted with perforated false bottoms. The soda solution, which
is heavier than water, tends to sink to the bottom and, after passing
through the perforations, is carried away by a pipe to the second tank,
and so on throughout the series. The fresh water is brought first into
contact with the black ash from which nearly all the soda has been
extracted.

The method of finishing off the black ash liquor differs according to
the final product which the manufacturer desires to obtain, for the
liquor contains caustic soda as well as mild soda. For the present, we
will suppose that the end product is to be washing soda. In this case,
carbon dioxide is passed into the liquor to convert what caustic soda
there is into mild soda.

The clarified soda liquor is then evaporated until crystals of soda
separate out. The first part of this process is carried out in large
shallow pans (P. Fig. 13), using the waste heat of the black ash
furnace, and finally in vats containing steam-heated coils. As the
crystals separate out, they are removed, drained, and dried.

Alkali Waste. Black ash contains less than half its weight of soda, so
that for every ton of soda produced there is from a ton and a half to
two tons of an insoluble residue which collects in the lixiviating and
settling tanks. This residue is known as alkali waste.

Alkali waste is of no particular value. It is not even suitable as a
dressing for the land, and since it is not soluble in water there is no
convenient means of disposing of it. Consequently, it is just
accumulated at the works and, as the heap grows at an alarming rate, it
cumbers much valuable ground. Moreover, it contains sulphides from
which, under the influence of air and moisture, sulphuretted hydrogen is
liberated. Alkali waste, therefore, has a very unpleasant odour.

The whole of the sulphur which was contained in the sulphuric acid used
in the first stage of the process remains in the alkali waste, mainly as
calcium sulphide. A plant for the recovery of this sulphur is
established in some of the larger works. The alkali waste is mixed with
water to the consistency of a thin cream, in tall, vertical cylinders.
Carbon dioxide under pressure is forced into the mixture, and this
converts the calcium sulphide into calcium carbonate and sets free
hydrogen sulphide, which, when burnt with a limited supply of air,
yields sulphur.

By this process, the most unpleasant feature of alkali waste, namely,
the smell, is removed. The calcium carbonate which remains is of very
little value. Some of it is used in making up fresh charges for the
black ash process and some for preparing Portland cement, for which
finely-ground calcium carbonate is required; the remainder is thrown on
a heap.

Bicarbonate of Soda. Bicarbonate of soda can be easily distinguished
from washing soda. It is a fine, white powder similar in appearance to
the efflorescence on soda crystals. It does not contain any water of
crystallization.

When bicarbonate of soda is heated, it does not melt, and, as far as its
external appearance is concerned, it does not seem to undergo any
change. If, however, suitable arrangements are made, water and carbon
dioxide gas can be collected, and the sodium bicarbonate will be found
to have lost 36·9 per cent. of its weight. The substance which remains
is identical with that obtained by heating soda crystals, that is,
anhydrous sodium carbonate. Sodium bicarbonate is, therefore, a compound
of sodium carbonate and carbonic acid.

The most familiar use of this compound is indicated by its common names
“baking-soda” and “bread-soda.” It is mixed with dough or other similar
material in order to keep this from settling down to a hard solid mass
in baking. The way in which bicarbonate of soda prevents this will be
readily understood when it is remembered that an ounce of this substance
liberates more than 2,300 cu. in. of carbon dioxide when it is heated.
When the bicarbonate of soda is well mixed with the ingredients of the
cake or loaf and disseminated throughout the mass, each particle will
furnish (let us say) its bubble of gas. Since these cannot escape, a
honey-combed structure is produced.

    [Illustration: Fig. 14. THE SOLVAY PROCESS]

Baking powder is a mixture of bicarbonate of soda and ground rice; the
latter substance is merely a solid diluent.

The Solvay Process. Soda ash is one of the principal forms of mild
alkali used in commerce. Large quantities of this substance are made by
heating bicarbonate of soda. We shall now consider another alkali
process in which this substance is the primary product.

For the greater part of the first century of its existence, the Leblanc
soda process had no rival, although another method, known as the
ammonia-soda process, was patented as early as 1838. In this case,
however, as in many others, expectations based on the experiments
carried out in the laboratory were not realized when the method came to
be tried under manufacturing conditions. It was not until 1872 that
Ernest Solvay, a Belgian chemist, had so far solved the difficulties,
that a new start could be made. In that year, about 3,000 tons of soda
were produced by the ammonia-soda or Solvay process, as it has now come
to be known. Since then, however, the quantity produced annually has
been steadily increasing, until at the present time it amounts to more
than half of the world’s supply.

The Solvay process is very simple in theory. Purified brine is saturated
first with ammonia gas and then with carbon dioxide. Water, ammonia, and
carbon dioxide combine, forming ammonium bicarbonate, which reacts with
salt (sodium chloride), producing sodium bicarbonate and ammonium
chloride.

The principal reaction is carried out in a tower (Fig. 14 (1), _a_, _a_)
from 50 to 65 ft. in height and about 6 ft. in diameter. At intervals of
about 3½ ft. throughout its length, the tower is divided into sections
by pairs of transverse discs, one flat with a large central hole, and
one hemispherical and perforated with small holes (Fig. 14 (2)). The
discs are kept in position by a guide rod G. Fig. 14 (3) shows a better
arrangement of the guide rods. In modern works, the space between the
discs is kept cool by pipes conveying running water. The ammoniated
brine is led into the tower near its middle point. The carbon dioxide is
forced in at E in the lowest segment, and as it passes up the tower it
is broken up into small bubbles by the sieve plates. Sodium bicarbonate
separates out as a fine powder, which makes its way to the bottom of the
tower suspended in the liquid.

The perforated plates are necessary for the proper distribution of
carbon dioxide through the brine. They are, however, a source of
trouble, because the holes quickly become blocked up with sodium
bicarbonate, and every ten days or so it is necessary to empty the tower
and clean it out with steam or boiling water.

Recovery of Ammonia. The production of 1 ton of soda ash by the Solvay
process involves the use of a quantity of ammonia which costs about
eight times as much as the price realized by selling the soda. It is
evident that the success of the process as a commercial venture depends
largely on the completeness with which the ammonia can be recovered.

During the process, ammonia is converted into ammonium chloride, which
remains dissolved in the residual liquor. From this ammonia gas is set
free by adding quicklime and by blowing steam through the mixture. It is
now claimed that 99 per cent. of the ammonia used in one operation is
recovered.

Soda Ash. The bicarbonate of soda produced by the Solvay process is
moderately pure. For all ordinary purposes, it is only necessary to wash
it with cold water to remove unchanged salt, and after drying, it is
ready to be placed on the market if it is to be sold as bicarbonate. The
greater part of the Solvay product, however, is converted into soda ash
by the application of heat. If soda crystals are required, the soda ash
is dissolved in water and crystallized.

In many ways, the Solvay process compares very favourably with the older
method. It is an advantage to start with brine, for that is the form in
which salt is very often raised from the mines. The end product is
relatively pure; moreover, it is quite free from caustic soda, which for
some purposes for which soda ash is used is a great recommendation.
There is no unpleasant smelling alkali waste. On the other hand, the
efficiency of the Solvay process is not high, for only about one-third
of the salt used is converted into soda. This would make the process
impossible from the commercial point of view were it not for the
cheapness of salt.

The Leblanc process, too, has its advantages. In the next chapter we
shall see that it is adaptable for the production of caustic as well as
mild alkali. The chlorine which is recovered in the Leblanc process is a
very valuable by-product. In the Solvay process, chlorine is lost, for
hitherto no practicable method has been found for its recovery from
calcium chloride.

The position with regard to the future supply of alkali is very
interesting. The competition between the Leblanc and the Solvay
processes for supremacy in the market is very keen. At the same time,
both processes are in some degree of danger of being supplanted by the
newer electrical methods, which will be mentioned in the last chapter.

The following table shows very clearly the rapid progress made by the
Solvay process in ten years. The quantities are given in _tonnes_ (1
tonne = 0·9842 ton).

                                  1884.                   1894.
                          _Leblanc     _Solvay    _Leblanc     _Solvay
                           soda._      soda._      soda._       soda._
  Great Britain           380,000      52,000     340,000      181,000
  Germany                  56,500      44,000      40,000      210,000
  France                   70,000      57,000      20,000      150,000
  United States                 —       1,100      20,000       80,000
  Austria-Hungary          39,000       1,000      20,000       75,000
  Russia                        —           —      10,000       50,000
  Belgium                       —       8,000       6,000       30,000
                          545,500     163,100     456,000      776,000

Mild Potash. Potassium carbonate (mild potash) was formerly obtained
from wood ashes. The clear aqueous extract was evaporated to dryness in
iron pots, and the substance was on this account called _potashes_;
later, potash. A whiter product was obtained by calcining the residue,
and this was distinguished as _pearl-ash_. Chemically pure potassium
carbonate was formerly obtained by igniting cream of tartar (potassium
hydrogen tartrate) with an equal weight of nitre. It is for this reason
that potassium carbonate is sometimes called “salt of tartar.”

About the middle of last century, natural deposits of potassium chloride
were discovered in Germany. The beds of rock salt near Stassfurt are
covered over with a layer of other salts, and for many years these were
removed and cast aside as “waste salts” (_abraumsalze_). When at a later
date they were examined more carefully, they were found to contain
valuable potassium compounds, notably the chloride. After that
discovery, mild potash was made by the Leblanc process., and Germany
controlled the world’s markets for all potassium compounds.

At the outbreak of war, the German supplies of potassium compounds
ceased as far as the allied nations were concerned, and an older method
of making potassium chloride from _orthoclase_ or potash-felspar was
revived. This involves the heating of the powdered mineral to a high
temperature after mixing it with calcium chloride, lime, and a little
fluorspar. The potassium chloride is then extracted from the fused mass
with water. This method has been worked with great success in America,
and it is claimed that potassium chloride can be made in that country at
a cost which is lower than that formerly paid for the imported article.

Mild potash and soda are so very similar in chemical properties that in
most cases it is immaterial which compound is used. In all cases in
which there is this choice, soda is employed, both because it is cheaper
and because it is more economical, for 106 parts of soda ash are
equivalent to 138 parts of potash. There are, however, some occasions
when soda cannot be substituted, notably for the manufacture of hard
glass and soft soap, and for the preparation of caustic potash,
potassium dichromate, and other potassium salts.

Potassium Bicarbonate. This resembles the corresponding sodium salt in
nearly every respect. It is, however, much more readily soluble in
water, so much so, that it is not possible to obtain this substance by
the Solvay method. It is made from potassium carbonate by saturating a
strong aqueous solution of that substance with carbon dioxide.



                               CHAPTER IX
                            CAUSTIC ALKALIS


The Alkali Metals. The discovery of current electricity in 1790
furnished the chemist with a very powerful agency for bringing about the
decomposition of compounds. Hydrogen and oxygen were soon obtained by
passing an electric current through acidulated water; and in 1807, Sir
Humphry Davy, who is perhaps better remembered for his invention of the
miners’ lamp, isolated the metals sodium and potassium by subjecting
caustic soda and caustic potash respectively to the action of the
current.

Sodium and potassium are very remarkable metals. They are only a little
harder than putty, and can easily be cut with a knife or moulded between
the fingers. When exposed to the air, they rust or oxidize very rapidly,
so much so that they have to be preserved in some mineral oil or in
airtight tins. They are lighter than water, which they decompose with
the liberation of hydrogen, and under favourable circumstances the
hydrogen takes fire so that the metals appear to burn on the surface of
the water. After the reaction is over and the sodium or potassium has
disappeared, a clear colourless liquid remains which has a strongly
alkaline reaction, and when this is evaporated until the residue
solidifies on cooling, caustic soda or potash is obtained. For very
special purposes, the caustic alkalis are sometimes made by the action
of the metals on water, but for production on a large scale, less
expensive methods are adopted.

Caustic Alkali is obtained from the corresponding mild alkali in the
following way. The substance—washing soda, for example—is dissolved in
water and the solution is warmed. Lime is stirred into this solution,
and from time to time a small test portion of the _clear_ supernatant
liquid is removed and mixed with a dilute mineral acid. When this ceases
to cause effervescence, the change is complete. The clear liquid is now
separated from the solid matter (excess of lime together with calcium
carbonate) and evaporated in a metal dish. Since the caustic alkalis are
extremely soluble in water, they do not crystallize as do most of the
compounds previously described. Evaporation is, therefore, carried on
until the liquid which remains solidifies when cold.

Caustic Soda. To describe the process by which caustic soda is
manufactured, we must return to the making of black ash. The mixture
from which black ash is made contains limestone. It is heated to 1000°
C., which is a sufficiently high temperature to convert limestone into
lime. When the black ash is subsequently treated with water, the lime
which is present converts some of the mild alkali to caustic;
consequently, black ash liquor always contains both alkalis.

When the manufacturer intends to make caustic soda and not soda
crystals, the composition of the black ash mixture is varied by adding a
larger proportion of limestone, so that there may be an excess of lime
in the black ash produced. The treatment with water is carried out as
described under washing soda, and then more lime is added to convert the
mild soda into caustic soda. After the excess of lime and other
suspended matter has settled down, the clear caustic liquor is
evaporated in iron kettles until it becomes molten caustic, which will
solidify on being allowed to cool.

There are various grades of caustic soda on the market differing one
from another in purity. The soap manufacturer uses caustic liquor or lye
containing about 40 per cent. of caustic soda. For other purposes, the
solid containing from 60 to 78 per cent. is used. Sometimes the product
is whitened by blowing air through the strong caustic liquor or by the
addition of a little potassium nitrate. Finally, for analytical
purposes, caustic soda is purified by dissolving it in alcohol and
subsequently evaporating the clear liquid.

Caustic Potash. The methods for the preparation of the corresponding
potassium compound are precisely the same as those described for caustic
soda; in fact, wherever the words sodium and soda occur in this chapter,
the reader can always substitute potassium and potash respectively.

Caustic Lime. Apart from its use in making mortar and cement, lime is
very often employed to neutralize acids. For this purpose, a suspension
in water, called milk of lime, is generally used, for lime itself is not
very soluble. Probably it is only the soluble part which reacts;
nevertheless, as soon as this is used up, more of the solid dissolves,
and in this way the action goes on as if all the lime were in solution.

Lime is also a very valuable substance in agriculture, especially on
damp, boggy land, where there is much decaying vegetable matter, and on
land which has been liberally manured. The soil in these cases is very
likely to become acid and is then unproductive. Lime is added to
“sweeten” the soil; in other words, to neutralize the acid.

Ammonia. The pungent smelling liquid popularly known as “spirits of
hartshorn” is a solution of ammonia gas in water. It is a caustic alkali
and, as such, is sometimes used to remove grease spots. Here, however,
we shall consider ammonia only in connection with ammonium salts, some
of which are used in very large quantity as fertilizers.

The principal source of ammonia at the present time is the ammoniacal
liquor obtained as a by-product in the manufacture of gas for heating
and lighting. Coal contains about 1 per cent. of nitrogen, and when it
is distilled, some of this nitrogen is given off as ammonia, which
dissolves in the water produced at the same time. This liquid is
condensed in the hydraulic main and in other parts of the plant where
the gas is cooled down.

Gas liquor contains chiefly the carbonate, sulphide, sulpho-cyanide, and
chloride of ammonia, together with many other substances, some of which
are of a tarry nature. It would not be practicable to evaporate this
liquid with a view to obtaining the ammonium salts, because it is only a
very dilute solution. Hence, after the removal of tar, the liquor is
treated in such a way that ammonia is set free.

In some cases the liberation of ammonia is accomplished by blowing
superheated steam into the liquor, which sets free the ammonia which is
combined as carbonate, sulphide, and sulpho-cyanide, but not that which
is present as chloride. In other works, the gas liquor is mixed with
milk of lime, which liberates all the combined ammonia. The ammonia is
then expelled from the mixture by a current of steam or air and steam.
In both cases, the gas which is given off is passed into sulphuric acid,
whereby ammonium sulphate is formed in solution and afterwards obtained
as a solid by evaporation.


                             Ammonium Salts

Ammonium Chloride. Like all other alkalis, ammonia solution neutralizes
acids, forming salts. With hydrochloric acid, it produces the white
solid known as _sal ammoniac_ or ammonium chloride. This compound is
familiar as the one required to make the liquid used in a Leclanché
cell, which is generally used as the current generator for electric
bells.

Ammonium Carbonate, which is also called stone ammonia and salt of
hartshorn, is made by subliming a mixture containing two parts chalk and
one part ammonium sulphate. It is a white solid which gives off ammonia
slowly and is, therefore, used as the basis for smelling salts.

Ammonium Nitrate is obtained by passing ammonia gas into nitric acid
until it is neutralized. It is a white solid, which melts easily on
being heated, and breaks up into water and nitrous oxide (laughing gas),
which is the “gas” administered by dentists. Ammonium nitrate is also
used in the composition of some explosives: for example, “ammonite” is
said to contain 80 per cent. of this substance.

Ammonium Sulphate is used chiefly as an artificial manure; the amount
required for this purpose throughout the world is over 1,500,000 tons
every year.

Synthetic Ammonia. Though the soluble compounds of nitrogen are fairly
abundant, the supply is by no means equal to the demand, because such
enormous quantities are required for agricultural purposes. It has been
already said that ammonia is obtained as a by-product in the
distillation of coal, and it has been repeatedly pointed out that our
coal supplies are far from inexhaustible; moreover, coal gas may not
always be used for lighting and heating. It, therefore, becomes a very
important question as to how the future supply of ammonium salts is to
be maintained.

Ammonia is a very simple compound formed from the elements nitrogen and
hydrogen, and, as before mentioned, the supply of free nitrogen in the
air is literally inexhaustible. In recent years, the efforts of chemists
have been directed towards finding a method of converting the free
nitrogen of the air into some simple soluble compound. This problem is
usually spoken of as the “fixation of nitrogen.”

In the Haber process, nitrogen obtained by the fractional distillation
of liquid air is mixed with three times its volume of hydrogen, and this
mixture is heated to between 500°C. and 700°C. under a pressure of 150
atmospheres (nearly 1 ton to the square inch) and in the presence of a
contact agent. Under these conditions, nitrogen and hydrogen combine to
form ammonia, which is condensed by passing the mixed gases into a
vessel cooled with liquid air, any unchanged nitrogen and hydrogen being
passed back again over the contact substance.

The problem of making ammonia from the air is closely connected with
that of making nitric acid from the same source. In some experiments the
two are combined, and ammonium nitrate is produced directly. Ammonia
made by the Haber process, or some modification, is mixed with
atmospheric oxygen and passed through platinum gauze heated to low
redness. This results in the formation of nitric oxide, which is further
oxidized by atmospheric oxygen; and finally, from a mixture of oxides of
nitrogen, water vapour, and ammonia, synthetic ammonium nitrate is
obtained.



                               CHAPTER X
                          ELECTROLYTIC METHODS


One of the most noteworthy developments of modern chemical industry has
been the increasing use of electricity as an agent for bringing about
changes in matter. This has followed naturally from the reduction in the
cost of electricity, due in great measure to the utilization of natural
sources of energy which for untold ages had been allowed to run to
waste.

This last achievement is likely to produce such a change in economic
conditions that it is worth while giving a little thought to what may be
called a newly-discovered asset of civilization. One example will make
this clear. In the bed of the Niagara river, which flows from Lake Erie
to Lake Ontario, there is a sudden drop of 167 ft. over which the water
rushes with tremendous force and expends its energy in producing heat
which cannot be utilized. This is a waste of energy, but it cannot be
circumvented because no method has yet been found to control the waters
of the Falls themselves. Nevertheless, by leading the head waters
through suitable channels from the high level to the low, it is possible
to use the energy to drive turbines, which, in their turn, drive dynamos
which produce the current. This is merely the conversion of the energy
of running water into electrical energy; and while the sun remains, this
supply of energy will be forthcoming in undiminished quantity, because
by the heat of the sun the water is lifted again as vapour, which
descends as rain to replenish the sources from which the Niagara flows.

Electricity is employed in chemical industry in two ways. In the first
place, it may be used to produce very high temperatures required for the
reduction of some metallic ores, for melting highly-refractory
substances, and for making steel. It is, however, rather with the second
method, called electrolysis, that we are here mainly concerned.

    [Illustration: Fig. 15. THE ELECTROLYSIS OF SALT SOLUTION]

Solutions of acids, bases, and salts, and in some cases the fused
substances themselves, conduct the electric current; but at the same
time they suffer decomposition. This method of decomposing a substance
is known as _electrolysis_, or a breaking up by the agency of
electricity.

The apparatus required in a very simple case is shown in Fig. 15. It
merely consists of some suitable vessel to contain the liquid; two
plates—one to lead the current into the solution, the other to lead it
away again—and wires to connect the plates to the poles of a battery,
storage-cell, or dynamo. Each plate is called an _electrode_, and
distinguished as positive or negative according as it is joined to the
positive or negative pole of the current generator. By convention,
electricity is supposed to “flow” from the positive pole of the battery
to the positive electrode or _anode_, and then through the solution to
the negative electrode or _cathode_, and so back to the negative pole of
the generator, thus completing the circuit external to the battery.

When acids, alkalis, and salts are dissolved in water, there is strong
evidence to show that they break up to a greater or less extent into at
least two parts called _ions_. These are atoms, or groups of atoms,
which have either acquired or lost one or more _electrons_.[5] They move
about quite independently of one another and in any direction until the
electrodes are placed in the liquid. Then they are constrained to move
in two opposing streams—those which have acquired electrons all move
towards the negative electrode, and those which have lost electrons
towards the other. At the electrodes themselves, the former give up and
the latter take up electrons, and become atoms again. Let us now
consider a concrete example. Common salt is composed of atoms of sodium
and atoms of chlorine paired. When a small quantity of this substance is
dissolved in a large quantity of water, the pairing no longer obtains.
The chlorine atoms move away independently accompanied by an extra
satellite or electron, and the sodium atoms move away also but with
their electron strength one below par. When the current is introduced
into the liquid, the sodium ions travel towards the cathode and chlorine
ions towards the anode, and when they reach the goal, sodium ions gain
one electron and chlorine ions lose one, and both become atoms again.
Chlorine atoms combine in pairs forming molecules and escape from the
solution in the greenish yellow cloud that we call chlorine gas. The
sodium atoms react immediately with water, forming caustic soda with the
liberation of hydrogen.

To return now to practical considerations. The electrolysis of salt
solution appears to be an ideally simple method of obtaining caustic
soda and chlorine from sodium chloride. As a manufacturing process, it
would seem to be perfect, for the salt is broken up directly into its
elements and a secondary reaction gives caustic soda automatically.
There is no “waste” as in the Leblanc process, and it does not require
the use of any expensive intermediary substance afterwards to be
recovered, as in the Solvay process. But, as very often happens when
working on a large scale, difficulties arise, and these up to the
present have only been partially overcome.

Some of the chlorine remains dissolved in the liquid and reacts with the
caustic soda, forming other substances which, though valuable, are not
easy to separate from the caustic soda. It is possible to get over this
difficulty to some extent by placing a porous partition between the
anode and the cathode, and in that way dividing the cell into cathodic
and anodic compartments. As long as the partition is porous to liquids,
it will allow the current to pass, but at the same time it will greatly
retard the mixing of the contents of the two compartments. Porous
partitions or cells which are in common use for batteries are made of
“biscuit” or unglazed porcelain.

It must be remembered, however, that porous partitions only retard the
mixing of liquids; they do not prevent it. Moreover, a further
difficulty arises from the fact that chlorine is a most active
substance, and therefore it is difficult to find a material which will
resist its corrosive action for any length of time, and the same
difficulty arises in the case of the anode where the chlorine is given
off.

Castner Process for Caustic Soda. The following is the most successful
electrical process for the manufacture of caustic soda yet devised. It
was introduced in 1892, and is known as the Castner process. It should
be noted that the use of the porous partition has been avoided in a very
ingenious way.

    [Illustration: Fig. 16. THE CASTNER PROCESS]

The cell (see Fig. 16) is a closed, rectangular-shaped tank divided into
three compartments by two non-porous partitions fixed at one end to the
top of the tank, while the other end is free and fits loosely into a
channel running across the tank. The floor of the tank is covered with a
layer of mercury of sufficient depth to seal the separate compartments.
The two end compartments contain the brine in which are the carbon
anodes; the middle compartment contains water or very dilute caustic
soda in which the cast-iron cathode is immersed.

The current enters the end compartments by the carbon anodes and passes
through the salt solution to the mercury layer which in these
compartments are the cathodes. The current then passes through the
mercury to the middle compartment, and then through the solution to the
cathode, thence back to the dynamo. It is important to note that in the
middle compartment the mercury becomes the anode.

Chlorine is liberated at the carbon electrodes, and when no more can
dissolve in the liquid it escapes and is conveyed away by the pipe P.
Sodium atoms are formed at the surface of the mercury cathodes in the
outside compartments and dissolve instantly in the mercury, forming
sodium amalgam.

While the current is passing, a slight rocking motion is given to the
tank by the cam E. This is sufficient to cause the mercury containing
the dissolved sodium to flow alternately into the middle compartment,
and there the sodium amalgam comes into contact with water; the sodium
is dissolved out of the mercury and caustic soda is formed. Water in a
regulated stream is constantly admitted to the middle compartment, and a
solution of caustic soda of about 20 per cent. strength overflows.

The production of caustic soda by an electrical method still remains to
be fully developed. A process which gives only a 20 per cent. solution
cannot be looked upon as final. In the meantime, other methods have been
tried, in some of which fused salt is used in place of brine in order to
give caustic soda in a more concentrated form. For a description of
these methods, the reader must consult some of the larger works
mentioned in the preface. Here we can only say that very great
difficulties have been encountered, particularly in the construction of
a satisfactory porous diaphragm or, alternately, in devising methods in
which this can be dispensed with.

Another interesting application of electrolysis is furnished by the use
of copper sulphate in industry. When this salt is dissolved in water, it
breaks up into copper ions (positive) and an equal number of negative
ions, composed of 1 atom of sulphur and 4 atoms of oxygen (SO″4). Under
the influence of the current copper ions travel to the cathode, and
there by the gain of two electrons become copper atoms. Now, since
copper is not soluble in copper sulphate solution, and is not volatile
except at very high temperatures, it is deposited on the cathode in a
perfectly even and continuous film when the strength of the current is
suitably adjusted. This film continues to grow in thickness as long as
the conditions for its deposition are maintained. If the current
employed is not suitable, the metallic film is not coherent, and the
copper may appear as a red powder at the bottom of the cell. Any other
metal or impurity which might be present in the unrefined copper falls
to the bottom of the tank.

Other metals are deposited electrolytically in exactly the same way. The
metal to be deposited is joined to the positive pole and the article to
be plated to the negative pole of the battery. Both are suspended in a
solution of salt, generally the sulphate, of the metal which is to be
deposited. Thus, for nickel plating, a piece of sheet nickel would be
used in conjunction with a solution of sulphate of nickel or, better, a
solution of nickel ammonium sulphate, made by crystallizing ammonium and
nickel sulphates together. The current required is small; indeed, if it
is too strong, the deposit adheres loosely to the article, and the
result is, therefore, not satisfactory.

Electrotype blocks are also made by a similar process. An impression of
the article to be reproduced is made in wax, or some suitable plastic
material, and polished with very fine graphite or black lead, in order
to give a conducting surface. It is then suspended in a solution of
copper sulphate and joined to the negative pole of the battery; a plate
of copper connected with the positive pole is suspended in the same
solution. When a weak current is passed, copper is deposited on the
black-leaded surface and grows gradually in thickness, until at length
it can be stripped off, giving a positive replica of the object.



                                 INDEX


                                   A
  Acetic acid (glacial), 73
  Acids, early notions of, 1
  ——, fatty, 78
  ——, mineral, 68
  ——, vegetable, 68
  Agate, 61
  Air-saltpetre, 42
  Alkali Acts, 44
  ——, caustic, 96
  ——, metals, 95
  ——, mild, 80
  —— waste, 87
  Alkalis, properties, 3
  Aluminium acetate, 73
  Alums, the, 26
  Amethyst, 61
  Ammonal, 36
  Ammonia, 97
  ——, synthetic, 99
  Ammonite, 99
  Ammonium carbonate, 99
  —— chloride, 98
  —— nitrate, 99
  —— sulphate, 99
  Anhydride, an, 21
  Anode, 103
  Argol, 76
  Asbestos, 63
  ——, platinized, 19
  Ash, black, 84
  ——, pearl, 93
  ——, soda, 10, 92
  Atolls, 51
  Atomized water, 18


                                    B
  Bacon, Roger, 32
  Basic slag, 58
  Basil Valentine, 12
  Beryl, 63
  Black liquor, 74
  Blasting gelatine, 35
  Bleaching powder, 46
  Blue-john, 47
  Boiler scale, 54
  Bonbonnes, 31
  Bone, 56
  —— ash, 57
  —— black, 56
  —— meal, 56
  Borax, 59
  Bordeaux mixture, 7
  Boric acid, 58
  Boyle, Robert, 2
  Burgundy mixture, 6


                                    C
  Calcium acetate, 5
  —— bicarbonate, 54
  —— carbonate, 50
  —— fluoride, 47
  —— nitrate, 29
  —— phosphate, 56
  —— sulphate, 27
  Calc spar, 50
  Caliche, 29
  Calico printing, 26
  Carbon, 49
  Carbonic acid, 49
  —— —— gas, 49
  Castner process, 105
  Catalytic action, 20
  Cathode, 103
  Cat’s-eye, 61
  Cavendish, H., 40
  Cellulose, 46
  Chalcedony, 61
  Chalk, 50
  Chert, 66
  Chili-saltpetre, 29, 39
  China clay, 62
  Citric acid, 77
  Chlorides, 47
  Chlorine, 46
  Chrome yellow, 28
  —— red, 28
  Compound, 7
  Compounds, binary, 8
  Contact action, 20
  —— process, 18
  Copper refining, 107
  —— sulphate, 5, 27
  Coral reefs, 51
  Cordite, 34
  Cream of tartar, 76
  Crops, rotation of, 37
  Crystallization, water of, 9
  Crystals, 9


                                    D
  Davy, Sir Humphry, 95
  Derbyshire spar, 47
  Devitrification, 65
  Dynamite, 35


                                    E
  Efflorescence, 82
  Electrode, 103
  Electrolysis, 102
  Electrons, 103
  Electrotype blocks, 107
  Element, definition of, 7
  Elements, list of, 8
  Explosives, 32


                                    F
  Felspars, 62
  Ferrous acetate, 74
  —— sulphate, 25
  Flint, 61
  Fluorspar, 48
  Formic acid, 78
  Fur in kettles, 54


                                    G
  Garnet, 63
  Gas, laughing, 99
  —— lime, 12
  —— liquor, 98
  Gay Lussac tower, 16
  Glass, 64
  ——, annealing of, 65
  ——, Bohemian, 63
  ——, etching on, 47
  ——, flint, 63
  ——, lead, 63
  ——, soda, 63
  ——, water, 66
  Glauber’s salt, 10
  Glover tower, 17
  Glue, 56
  Graphite, 108
  Greek fire, 32
  Guncotton, 34
  Gunpowder, 32
  Gypsum, 27


                                    H
  Haber process, 100
  Halogen, 43
  Hardness, permanent, 53
  ——, temporary, 53
  Hartshorn, salt of, 99
  ——, spirits of, 97
  Hornblende, 63
  Hydriodic acid, 48
  Hydrobromic acid, 48
  Hydrochloric acid, 43
  Hydrofluoric acid, 47


                                    I
  Iceland spar, 50
  Ions, 103
  Iron pyrites, 11


                                    J
  Jade, 63
  Jasper, 61


                                    K
  Key industries, 10


                                    L
  Lake, 26
  Lead acetate, 75
  —— chambers, 17
  —— chamber process, 14
  ——, sugar of, 75
  —— sulphate, 27
  ——, white, 75
  Leblanc soda process, 82
  Leguminosae, 37
  Lemon, salts of, 77
  Lime burning, 51
  ——, caustic, 97
  —— kiln, 51
  Limestone, 50
  Litmus, 2
  Lupin root, 37


                                    M
  Marble, 50
  Marking ink, 28
  Meerschaum, 63
  Mica, 63
  Mordants, 26
  Mycoderma aceti, 68


                                    N
  Neutralization, example of, 4
  ——, explanation of, 3
  Niagara, 101
  Nitre, 29
  —— pots, 14
  Nitric acid, 30
  —— ——, from air, 40
  —— ——, importance of, 28
  —— —— manufacture of, 30
  —— ——, properties, 31
  —— ——, red fuming, 31
  —— oxide, 16
  Nitrogen cycle, 37
  ——, fixation of, 100
  —— peroxide, 16
  Nitroglycerine, 34


                                    O
  Olein, 78
  Onyx, 61
  Opal, 61
  Orthoclase, 62
  Oxalic acid, 77


                                    P
  Palmitin, 78
  Pearls, 51
  Peregrine Phillips, 21
  Philosopher’s stone, 2
  Phosphoric acid, 57
  Plaster of Paris, 27
  Potash, caustic, 97
  ——, mild, 93
  Potassium, 95
  —— bicarbonate, 94
  —— nitrate, 29
  Propellants, 33
  Prussian blue, 25
  Pyrites burners, 14
  Pyroligneous acid, 73


                                    Q
  Quartz, 61
  —— fibres, 62
  ——, smoky, 61
  Quicklime, 5, 51


                                    R
  Red liquor, 73
  Rock crystal, 61
  Rupert’s drops, 65


                                    S
  Sal ammoniac, 99
  —— prunella, 29
  Salt cake, 84
  ——, common, 47
  ——, formation of a, 4
  Saltpetre, 29
  Salts, from carbonates, 5
  ——, from oxides, 5
  ——, from metals, 4
  ——, insoluble, 6
  Sandstone, artificial, 66
  Saponification, 79
  Schweinfurt green, 27
  Shells, egg, 51
  ——, oyster, 51
  Silica, 61
  —— ware, 62
  Silicic acid, 62
  Silver bromide, 48
  —— chloride, 48
  —— iodide, 48
  —— nitrate, 28
  —— sand, 61
  Soap, hard, 79
  ——, soft, 79
  Soda, baking, 88
  ——, bicarbonate of, 6, 88
  ——, bread, 88
  ——, caustic, 96
  ——, mild, 80
  ——, natural, 82
  ——, washing, 3, 5, 81
  —— water, 49
  Sodium, 95
  —— nitrate, 29
  —— sulphate, 27
  Soil bacteria, 38
  Solvay process, 90
  Sorrel, salts of, 77
  Spent oxide, 11
  Stalactite, 53
  Stalagmite, 53
  Stearin, 78
  —— candles, 79
  Stone ammonia, 99
  Suffioni, 60
  Sulphur, 11
  —— dioxide, 11
  —— trioxide, prep. of, 19
  Sulphuric acid, properties, 20, 24
  —— anhydride, 21
  Sulphurous acid, 11
  Superphosphate, 57


                                    T
  Tallow, 79
  Tartaric acid, 76
  Tinkal, 61
  Trinitrotoluene, 35


                                    V
  Verdigris, 74
  Vert de Montpellier, 74
  Vinegar, 68
  ——, malt, 70
  ——, wine, 70
  Vitriol, blue, 5
  ——, nitrated, 16
  ——, oil of, 12


                                    W
  Ward, Dr., 12
  Water, hard, 53
  ——, soft, 53
  ——, softening of, 54
  Wood ashes, source of potash, 3
  —— ——, used  as  soap, 2


                                    Z
  Zinc chloride, 5


                                 THE END



                               Footnotes


[1]An anhydride is a substance which unites with water to form an acid.

[2]See Frontispiece.

[3]Now £13 a ton.

[4]Basic lead carbonate.

[5]An electron is probably an “atom” of negative electricity detached
    from matter.


        _Printed by Sir Isaac Pitman & Sons, Ltd. Bath, England_
                               (v—1468c)



                          Transcriber’s Notes


—Silently corrected several palpable typographical errors.

—Retained publication information from the original source.

—In the text versions, included italicized text in _underscores_.





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