OLIN 
 
 QD 
 
 43 
 
 .C44 
 
 1919 
 
Cornell University 
 Library 
 
 The original of tliis book is in 
 tine Cornell University Library. 
 
 There are no known copyright restrictions in 
 the United States on the use of the text. 
 
 http://www.archive.org/details/cu31924087818203 
 
THE 
 
 CHEMCRAFT BOOK 
 
 FOB 
 
 tTHr THtMiCAL OOTriT- 
 
 No. 2 
 
 (FIFTH EDITION) 
 
 Directions 
 
 • I I , I I II II- 
 
 Explan a tion of Chemical Science and Industriea 
 Chemical Magic * 
 
CORNELL UNIVERSITY LjBRARV 
 
 203 
 
 Diamond Binding and Printing Co, 
 
 intelligent service 
 Hagerstown, Maryland 
 
THE 
 CHEMCRAFT BOOK 
 
 FOR OUTFIT NUMBEiR 2 
 FIFTH EDITION 
 
 Directions 
 
 Explanation of Chemical Science and Indu stries 
 
 Chemical Magic 
 
 Copyright, 1915 
 
 Copyriglit, 1916 
 
 Copyright, 1917, Third Edition 
 
 Copyright, 1918, Fourth Edition 
 
 Copyright, 1919, Fifth Edition 
 
 The Porter Chemical Co. 
 
 Hagerstown, Md. 
 
TABLE OF CONTENTS 
 
 Page 
 
 Introduction ^ 
 
 General Directions ' 
 
 PART I 
 
 CHEMISTRY AND ITS APPLICATION TO THE INDUSTRIES 
 
 Chemical Elements 
 Experiment Page 
 
 1. Combination of Elements 9 
 
 2. Breaking up a Chemical Compound 10 
 
 3. An Exchange of Elements 10 
 
 indicators 
 
 4. Phenolphthaleln 11 
 
 5. Litmus 11 
 
 6. Household Indicators 11 
 
 Air-Oxygen 
 
 7. Suffocating a Fire 12 
 
 8. Flre-Prooflng 12 
 
 (a) Cloth 12 
 
 (b) Wood 13 
 
 9. Fire Ink • ■ 13 
 
 10. Making a Fuse 13 
 
 11. The Reduction of Logwood 14 
 
 12. Bleaching with Sulphur Dioxide 14 
 
 Hydrogen 
 
 13. Preparation of Hydrogen 15 
 
 Water 
 
 14. Solution 15 
 
 15. Diffusion 16 
 
 16. The Effect of Solution on Chemical Reaction 16 
 
 17. The Effect of Solution on Temperature 16 
 
 18. Undercooled Water 16 
 
 19. The Effect of Temperature on Solubility 16 
 
 20. The Formation of Crystals 17 
 
 21. Water of Crystallization 17 
 
 22. Dissolving Solids in Their Water of Crystallization...... 18 
 
 23. Testing for Traces of Moisture Ig 
 
 24. Sympathetic Ink ' jg 
 
 25. The Dehydration of Cobalt Chloride 19 
 
 26. Permanent Sympathetic Ink ' j^g 
 
 27. A Supersaturated Solution -^g 
 
 The Halonen Family 
 
 28. Preparation and Properties of Chlorine 20 
 
 (a) Preparation 20 
 
(b) Tests of Chlorine 20 
 
 (c) Bleaching with Chlorine 20 
 
 29. Hydrogen Chloride ■ ■ 21 
 
 30. Another Method of Preparing Chloride and Chlorine 21 
 
 Carbon — Combustion — Carbonates 
 
 31. A Test for Carbon Dioxide in Products of Combustion. ... 22 
 
 32. The Structure of Flame — A Cas Factory 22 
 
 33. The Structure of Flame — Manufacturing Lampblack.... 22 
 
 34. Making Water from Fire • • 23 
 
 35. Test for Carbon Dioxide in the Breath — "Bugs in the 
 
 Breath" 23 
 
 36. The Distillation of Wlood 24 
 
 37. The Manufacture of Carbon Dioxide — Chemical Boiling. . 25 
 
 38. Some Properties of Carbon Dioxide 25 
 
 39. Acid Properties of Carbon Dioxide 26 
 
 40. Testing Household Materials for Carbonates ■• 26 
 
 41. Limestone Ice 27 
 
 Nitrogen 
 
 42. The Manufacture of Ammonia. ^. . • 27 
 
 43. Another Method of Preparing Ammonia 27 
 
 44. Making Ammonia in Your Hand 27 
 
 45. Volatilization of Ammonium Compounds 28 
 
 46. Nitrogen Compounds 28 
 
 Sulphur 
 
 47. The Properties of Sulphur 28 
 
 48. FJastic Sulphur 29 
 
 49. Preparation and Properties of Hydrogen Sulphide 29 
 
 (a) Preparation 29 
 
 (b) Properties 29 
 
 50. Test for Hydrogen Sulphide 30 
 
 51. The Oxidation of Lead Sulphide to Lead Sulphate 31 
 
 52. Silver Sulphide 31 
 
 53. The Manufacture of Lime-Sulphur Solution 31 
 
 Silicon — Silicates 
 
 54. Silicon Dioxide 32 
 
 55. Sodium Silicate (Water Glass) . . • • 32 
 
 56. Strontium Silicate 33 
 
 57. Zinc Silicate 33 
 
 58. Aluminum Silicate 33 
 
 59. Nickel Silicate 33 
 
 60. Ferric and Ferrous Silicates (Iron Silicates) 33 
 
 (a) Ferrous Silicate 33 
 
 (b) Ferric Silicate 33 
 
 61. Cobalt Silicate 34 
 
 62. Manganese Silicate • 34 
 
 Boron — Borates 
 
 63. A Test for Boric Acid 34 
 
 64. Borax Glass 34 
 
65. Cobalt Borax Glass ^^ 
 
 66. Iron Borax Glass °^ 
 
 67. Manganese Borax Glass ^5 
 
 68. Nickel Borax Glass 35 
 
 The Fire-Works Industry 
 
 69. Tlie Manufacture of Colored Fire 35 
 
 (a) Red Fire 35 
 
 (b) Yellow Fire • ■ 35 
 
 The Ink Industry 
 
 70. The Manufacture of Writing Ink 36 
 
 71. The Manufacture of Blue Ink 36 
 
 72. The Manufacture of Violet Ink 36 
 
 73. The Manufacture of Red Ink 36 
 
 The Paint Industry 
 
 74. The Manufacture of Iron Pigments , 37 
 
 75. The Manufacture of I.akes 37 
 
 76. The Manufacture of Zinc Whit© 37 
 
 The Soap Industry 
 
 77. The Manufacture of Soap 37 
 
 78. Testing for Free Alkali in Soap 38 
 
 The Dyeing Industry 
 
 79. Dyeing Fabrics Light Blue 39 
 
 80. Dyeing Fabrics Dark Blue 39 
 
 81. Dyeing Fabrics Red 39 
 
 82. Dyeing Fabrics Black 39 
 
 83. Dyeing Fabrics Brown 39 
 
 84. Dyeing with a Mordant 39 
 
 85. Some Naturally Occurring American Dye-StufCs 40 
 
 86. The Effect of Acids and Alkalies on Logwood 40 
 
 87. Logwood Black 40 
 
 88. Dark Red Logwood Color 41 
 
 Organic Chemistry 
 
 89. The Manufacture of Sulphur Colors 41 
 
 90. The Decomposition of Sugar 42 
 
 91. The Preparation of Casein 42 
 
 92. The Chemistry of Tanning 42 
 
 The Chemistry of Foods 
 
 93. A Test for Starch 43 
 
 94. Testing for Proteids 43 
 
 95. Testing Baking Powder 44 
 
 96. Testing Flour ' ' 44 
 
 97. Testing Butter 44 
 
 98. Testing Canned Goods for Copper 44 
 
 99. The Manufacture of Baking Powder 45 
 
 100. A Test for Acid Mouth ■...'...' 45 
 
 Testing Soil 
 
 101. A Test for Acid Soil ^g 
 
PART II 
 CHEMICAL MAGIC 
 
 Magic Inks and Papers 
 
 102. Magic Writing 47 
 
 103. Magic Inks 47 
 
 104. Magic Writing Paper 47 
 
 Magic Changes 
 
 105. Changing Red, Wiite and Blue to Blue 48 
 
 106. Changing Water to Wine and Wine to Water 48 
 
 (a) Pouring Water and Wine out of the Same Pitcher 48 
 
 (b) Changing Water to Wine and Wane to Water 49 
 
 107. Changing Water to Milk 49 
 
 108. Changing Water to Blood and Blood to Stone 49 
 
 Magic Colors 
 
 109. Pouring Many Colors from the Same Vessel 49 
 
 110. Pouring Ink and Milk from the Same Vessel 50 
 
 111. Pouring Red, WJilte and Blue from the Same Vessel — 
 
 Patriotic Colors 50 
 
 112. Pouring Wine and Water into the Same Glass 50 
 
 113. Pouring White and Red into the Same Glass 51 
 
 Chemical Sorcery 
 
 114. Chemical Ice . ■ ■ 51 
 
 115. Chemical Soda Water 51 
 
 116. Chemical Plants 51 
 
 117. Chemical Snow 52 
 
 118. A Chemical Clock 52 
 
 Chemical Colors 
 
 119. Clots of Color 52 
 
 120. A Potpourris of Colors 52 
 
 121. Green Alcohol 53 
 
 122. A Color Chase •• 53 
 
 123. Changeable Colors 54 
 
 124. A Fugitive Color ■ • 54 
 
 125. A Magic Pitcher of Ink 54 
 
 Miscellaneous 
 
 126. Chameleon Paper 55 
 
 127. Chameleon Liquid 55 
 
 128. Rainbow Streamers 55 
 
 129. Changing Rainbow Streamers into Moss 55 
 
 130. The Magic Handkerchief 55 
 
INTRODUCTION 
 
 Before beginning the experiments described in this 
 book let us consider for a moment the broader aspects of 
 the science of chemistry. The whole great universe about 
 us from its uppermost heights to its lowest depths is built 
 up of chemicals and chemical compounds. Earth, sky and 
 water are all passing constantly through chemical chan- 
 ges. Deep down in the ground, coal is being formed from 
 the remains of prehistoric forests. Precious metals and 
 ores are being smeltered under the heat and pressure of 
 millions of tons of earth and rock. On the surface of the 
 earth, air and water are continually producing chemical 
 changes in everything they touch. 
 
 All nature is but a series of wonderful chemical re- 
 actions; plants, forests, birds, animals and people are all 
 complex chemical engines. 
 
 Chemistry is more closely interwoven with the indus- 
 tries of the world than any other science, and the country 
 which leads in chemical industries will ultimately be the 
 richest and most powerful. It will have the fewest waste 
 materials, it will have the best manufactured articles, its 
 foods will be the most nourishing and the cheapest, it will 
 possess the secrets of the most powerful explosives, the 
 hardest steels and the mightiest engines. 
 
 Surely a population educated in the science of chemis- 
 try is the greatest asset your country can have. 
 
 To-day, no matter what profession a man follows, he 
 is greatly handicapped without a knowledge of chemistry. 
 The manufacturer, the farmer, the tradesman, the pro- 
 fessional man, the scientist, all have constant need of 
 chemical knowledge. In the home the housewife who 
 knows nothing of the chemistry of the food which she 
 prepares or of the materials which she daily uses is ser- 
 iously handicapped. 
 
 Chemistry is also a spectacular science and many 
 chemical phenomena are most starthng and mystifying 
 to the layman. The science of chemistry plays an impor- 
 tant part in enabling sleight-of-hand performers and 
 magicians to perform their tricks. 
 
 In CHEMCRAFT, the various phases of chemistry 
 have been combined into a series of fascinating experi- 
 ments which will furnish amusement for the young peo- 
 ple during many profitable hours, and as the exnerimen- 
 
THE CHBMCRAPT BOOK 7 
 
 ter gains in skill and knowledge he can by means of the 
 numbers 3 and 4 CHEMCRAFT sets extend still further 
 his acquaintance with this most fascinating science. 
 
 Chemistry is sometimes looked upon as a dangerous 
 profession, but this is not the case. Contrary to an old 
 popular idea, a chemical experiment does not necessarily 
 result in an explosion. 
 
 Chemicals, as a class, are not intended for use as food 
 and should not be eaten, but very few of them are violent 
 poisons. CHEMCRAFT, in particular, does not contain 
 any dangerous poisons or otherwise harmful substances. 
 
 The quantities of chemicals furnished with the outfit 
 are sufficient to allow each experiment to be performed a 
 number of times. An additional supply of any chemical or 
 extra apparatus can be obtained by sending direct to the 
 manufacturer. See the price list at the end of this book. 
 THE PORTER CHEMICAL CO., 
 
 Hagerstown, Md. 
 
 GENERAL DIRECTIONS 
 
 Before performing the experiments given in this 
 book the following paragraphs should be carefully read. 
 
 MEASURING CHEMICALS 
 
 One measure of a chemical means the quantity which 
 can be held on the end of a small measure. One-half mea- 
 sure calls for one-half of the amount, two measures for 
 twice the amount, etc. The spoon is not intended for 
 measuring chemicals except where especially mentioned. 
 
 STIRRING ROD 
 
 A solid can be dissolved in a liquid much more quickly 
 if the mixture is stirred or shaken. Always clean the rod 
 after taking out of one liquid and before putting it into 
 another. 
 
 TEST TUBES 
 
 Test tubes are made of hard, thin glass specially an- 
 nealed to stand heating. Liquids may be boiled, and solids 
 heated to a high temperature in these tubes, but care 
 
THE CHEMCRAFT BOOK 
 
 should be taken never to wet a dry hot test tube as this is 
 almost sure to 'break it. If you have been heating a solid 
 let your test tube cool before washing it, or adding liquid. 
 
 GAS DELIVERY TUBE 
 
 The Gas Delivery Tube is used for the purpose of con- 
 ducting a gas which is being generated in a test tube, 
 into any desired vessel. Its use is specified wherever 
 necessary. 
 
 TEST TUBE HOLDER 
 
 When heating mixtures in a test tube it sometimes 
 becomes too hot to hold with the fingers, in which case a 
 test tube holder is necessary. To make one of these hold- 
 ers cut a piece of fairly heavy paper six inches square, 
 and fold it over three times, making a strip six inches 
 long and three-quarters of an inch wide. Put this around 
 the test tube and fasten securely with a paper clip. 
 
 HEATING 
 
 A candle is included in each outfit 
 and will give all the heat necessary in 
 most of the experiments, if it is set in 
 a place which is free from draught so it 
 will burn with a steady flame. In a very 
 few cases the use of some other com- 
 mon method of heating has been sug- 
 gested so as to obtain a little higher 
 e~ temperature. When heating a test tube 
 by a candle, hold it just over the top 
 of the flame to avoid the deposit of soot. 
 Never point the mouth of a test tube at yourself, or 
 at anyone nearby, when heating a liquid. It may boil over 
 suddenly, thereby causing burns or spotting the clothing. 
 Always remove a test tube or other vessel from the flame 
 before bringing it near the face to smell the evolved gas. 
 
 REMAINING EQUIPMENT 
 
 A spoon for measur- 
 ing liquids and heating 
 compounds and a length 
 of glass tube are included, 
 their use being mentioned 
 in the experiments in which they are needed. 
 
THE CHEMCRAFT BOOK 9 
 
 A number of experiments call for the upe ^f glasses ; 
 these should be'orctmary jelly glasses or iteavy tumblers. 
 
 All bottles should be kept tightly corke^, as many of 
 the chemicals gradually Iq^e their strength, if exposed to 
 the air. v 
 
 When performing experiments, be sure to spread a 
 thick layer of newspaper or other protecting materials 
 over the table so that the hot liquids, candle grease, etc., 
 cannot injure the surface. 
 
 Always read' an experiment entirely through before 
 ►Starting to perform it. By following this rule, many mis- 
 talcs' wiH' be avoided. 
 
 PART 1 
 
 CHEMISTRY AND ITS APPLICA- 
 TION TO THE INDUSTRIES 
 
 CHEMICAL ELEMENTS 
 
 Chemistry is the science which tells us what things 
 are made of. Everything that we handle has in some way 
 to do with chemistry. The ground we walk on, the clothes 
 we wear, and the food we eat, are all chemicals or mix- 
 tures of chemicals. 
 
 Chemistry teaches us that all matter is made of ele- 
 ments. There are only about 85 elements, but they may 
 be combined in all sorts of ways so that the number of 
 chemical compounds possible is enormous. 
 
 Experiment 1 — Combination of Elements. 
 
 Zinc is an element; there is nothing in it hut zinc. Sulphur is 
 another element; there is nothing in it but sulphur. 
 
 Take 1 measure of Powdered Zinc (No. 11) and an equal 
 amount of Sulphur (No. 1). Mix on a sheet of paper. The mix- 
 ture is not a compound, and the sulphur can be again separated 
 from the zinc. 
 
 Now put half a measure of the mixture of zinc and sulphur in 
 the spoon, and heat over a candle or alcohol lamp for 3 or 4 min- 
 utes, keeping your face at a little distance. After the mass be- 
 comes hot, the sulphur will take flre and burn. The niixture mean- 
 while swells to a bulky, porous mass. Suddenly there is a small 
 flash, and the sulphur and zinc unite chemically, forming zinc sul- 
 phide. 
 
10 THE CHBMCRAFT BOOK 
 
 Examine tlie zinc sulphide closely. You will find no traces of 
 the original zinc <m sulphur. If treated with acid this substance 
 gives off a gas having the smell of rotten eggs, hydrogen sulphide. 
 
 Put the zinc sulphide in a test tube, add 1 measure of Sodium 
 Bisulphate (No. 7), a few drops of water, and warm over a flame 
 for a moment. Smell the gas given off at the mouth of the tube. 
 
 Some chemical* compounds are broken up on heating. 
 
 Experiment 2 — Breaking Up a Chemical Compound. 
 
 Place 2 measures of Sodium Thiosulphate (No. 16) in a test 
 tube; using a test tube holder so as not to burn your fingers, heat 
 over a •flame. Notice that the solid first becomes moist and steam 
 is given off. This is because sodium thiosulphate contains water of 
 crystallization which is driven off when the substance is heated. 
 Continue heating for a few minutes longer and you will find that 
 sulphur is given off and is deposited on the upper part of the test 
 tube. Remove the tube from the flame and smell the gas which is 
 given off at the mouth of the tube. You will recognize the odor of 
 hydrogen sulphide, the same gas which was given off in Experi- 
 ment 1. 
 
 We see from this experiment that by heating sodium thiosul- 
 phate it is broken up into several different substances. First — 
 water whicjh was driven off as steam. Second — sulphur which was 
 deposited around the upper part of the test tube. Third — hydrogen 
 sulphide gas which you could smell at the mouth at the test tube. 
 Fourth — a reddish mass left in the bottom of the tube which con- 
 sists of sodium sulphate and sodium sulphide. 
 
 Most common substances are compounds of two or 
 more elements, and the art of the chemist lies in his abili- 
 ty to add or subtract elements, and change them around 
 in various ways. Such a change in the elements in sub- 
 stances is called a reaction. Reactions may be of various 
 kinds. Experiment 1 illustrates a reaction of combina- 
 tion. Experiment 2 is an example of a reaction of decom- 
 position. One of the most common kinds of reaction is 
 the exchange, in which the elements in two or more sub- 
 stances change places with each other. 
 
 Experiment 3 — An Exchange of Elements. 
 
 Fill a test tube half full of water and add % measure of Ferric 
 (Iron) Ammonium Sulphate (No. 21) close the mouth of the test 
 tube with your thumb and shake to dissolve the solid. Now add Vz 
 measure of Calcium Oxide (No. 20) and shake again. A brown pre- 
 cipitate will be formed. 
 
 The iron (ferric) in the ferric ammonium sulphate changed 
 places with the calcium in the calcium oxide, forming calcium sul- 
 phate and ferric oxide, which is insoluble in water and appeared 
 as a brown precipitate. 
 
THE CHEMCRAPT BOOK 11 
 
 INDICATORS 
 
 There are many classes of chemical compounds, but 
 the most common are Acids, Alkalies and Salts. Acids 
 are substances which have a peculiar "acid" taste, are 
 capable of dissolving many other substances, and can 
 unite with alkalies to form neutral substances called salts. 
 Alkalies have an "alkaline" taste and unite with acids. 
 Common table salt is a good example of a salt. Its chemi- 
 cal name is Sodium Chloride. 
 
 There are certain substances which are known as in- 
 dicators and which have the property of turning one color 
 in the presence of acids and another color in the presence 
 of alkalies. They can thus be used to show whether any 
 liquid is acid or alkaline. 
 Experiment 4 — Phenolphthalein. 
 
 Put 1 or 2 drops of Phenolphthalein Solution (No. 22) into halt 
 a glass of water. Drop In 1 measure of Sodium Carbonate (No. 4) 
 which is an alkali and stir. Next drop in 1 measure, or possibly 1% 
 measures of Tartaric Acid (No. 14) or a few drops of vinegar (which 
 contains acetic acid) and stir again. 
 
 Phenolphthalein is an indicator which is red in the presence of 
 llkalies, and colorless in the presence of acids. Some water sup- 
 plies are alkaline and hence give the red color as soon as the phen- 
 olphthalein is added. 
 
 Experiment 5 — Litmus. 
 
 Put a piece of Blue Litmus Paper (No. 18) into a glass half full 
 of water. Add % measure of Tartaric Acid (No. 14) (or a few drops 
 of vinegar) and stir. Next add 1 measure of Sodium Carbonate 
 (No. 4) and stir again. Note the color changes. 
 
 Litmus is a dye-stuff obtained from a kind of lichen. It is red 
 in the presence of acids and blue in the presence of alkalies. 
 
 Litmus paper is prepared by staining white unsized paper with 
 a strong solution of litmus in hot water. 
 
 Experiment 6 — Household Indicators. 
 
 An indicator may be prepared by soaking red cabbage leaves in 
 water, and pouring off the clear purple liquid. This liquid will be 
 colored red by acids and green by alkalies. The petals of dahlias 
 and violets also contain a coloring matter, which is one color in the 
 presence of acids and another in the presence of alkalies. 
 
 AIR-OXYGEN 
 
 Air is a mixture of two elements, oxygen and nitro- 
 gen, both of which are gases. Of all the elements, oxygen 
 is the most abundant, and most widely diffused. One-fifth 
 of air is free oxygen, and eight-ninths of water is com- 
 bined oxygen. Common materials like sandstone, lime- 
 stone, brick and mortar contain about fifty per cent oxy- 
 
12 
 
 THE CHEMCRAPT BOOK 
 
 gen. It has been estimated that fully two-thirds of our 
 world is oxygen. 
 
 It is the oxygen of the air which we breathe into our 
 lungs from whence it is carried by the blood throughout 
 our tissues to combine with waste materials. Carbon 
 dioxide is formed by the reaction, is carried back to the 
 lungs by the blood and finally reaches the air in our 
 breath. If the air should be deprived of oxygen we could 
 not live, but on the other hand, if we were forced to 
 breathe pure oxygen the reaction would consume our tis- 
 sues too rapidly, we would soon expend our energy and 
 die. Pure oxygen is often used as a stimulant for sick 
 people who are in an extremely weak condition. 
 
 Oxygen is necessary for ordinary combustion. Fire 
 will not burn unless fresh air is constantly supplied, so 
 that it can have oxygen. Air will not keep fire burning 
 after the oxygen in it has been used up, and stoves are 
 provided with chimneys so that there will be a draft or 
 current of air passing through the fuel. Fire can be 
 smothered by keeping fresh air away from it, as by 
 throwing a blanket over it. 
 
 Experiment 7 — Suffocating a Fire. 
 
 Set a candle In the middle of an ordinary milk or baking pan, 
 first allowing a few drops of molten grease to fall on the pan to 
 stick the candle tightly. Next pour 
 about 2 inches of water into the pan. 
 
 Now light the candle and set over 
 It an inverted milk bottle or fruit jar. 
 The bottle or jar must be high enough 
 so that the bottom will not come too 
 close to the candle flame. 
 
 Note that almost at once the 
 candle flame grows dim, and that after 
 a few minutes it dies out, the oxygen 
 of the air inside the bottle having 
 been used up. 
 
 Note further that after the flame 
 has gone out, the water begins to rise inside the bottle, and flnally 
 stands at a considerably higher level in the bottle than' in the pan 
 
 This is due to the removal of the oxygen from the air inside the 
 bottle, thus leaving a partial vacuum which is flUed by the water 
 In the flame, the oxygen unites with the candle forming carbon 
 dioxide (See Experiment 31), a gas which dissolves in water and 
 steam which condenses to water (See Experiment 34). 
 Experiment 8 — Fire Proofing. 
 
 (a)^Cloth. 
 
 Cloth, wood or other inflammable substances may be flre- 
 
THE CHEMCRAPT BOOK 13 
 
 proofed by treating them with chemicals *hich when heated give 
 off vapors that smotlier the flame. 
 
 Dissolve 12 measures of Ammonium Chloride (No, 9) in a test 
 tube 1-3 full of water. Put a piece of cotton cloth 2 or 3 inches 
 square in the bottom of a glass and pour the liquid in the test tube 
 over it. Stir the clcth around until it is wet through, then let it dry 
 and try to light it with a match. You will find that it will burn 
 while held in the flame, but just as soon as the match flame is re- 
 moved it will go out. 
 
 Because fabrics treated in this manner cannot be set on fire by 
 sparks or overturned caudles this process of fire-proofing is quite 
 generally used in connecticn with the curtains and scenery for 
 theatres. All the woodwork on battleships is also treated in this 
 manner, so that it will not take flre from the explosion of shells. 
 Other chemicals than ammonium chloride are frequently used, one 
 of the best being sodium tungstate, which, however, is rather ex- 
 pensive. 
 
 (b)— Wood. 
 
 Hold a match by the head and dip the other end into No. 19 
 which contains Water Glass (Sodium Silicate Solution). Let the 
 coating which is obtained dry for about 15 minutes, then light the 
 match. There will be no danger of burning your fingers, for the 
 flame will go out as soon as it reaches the water glass. 
 
 A reaction which adds oxygen to a substance is called 
 oxidation. Some compounds contain oxygen in such a 
 form that it is easliy given up to other compounds. Such 
 compounds are called oxidizin.g agents. A reaction of oxi- 
 dation usually gives out much heat and sometimes fire. 
 Experiment 9 — Fire Ink. 
 
 Place 6 measures of Potassium Nitrate (No. 8) in a test tube 
 and add % inch of water. Heat over the candle for a moment to 
 dissolve all of the solid. 
 
 Now use the liquid as ink, writing with a clean pen (or still 
 better using a small brush) on unglazed paper. Make your strokes 
 heavy and connect all lines. 
 
 Allow the marks to dry thoroughly and then apply a lighted 
 match or better a glowing spark, to some portion of the writing. 
 Blow out any flame which results. If properly started a spark will 
 travel along the lines where the liquid has been applied without 
 burning the rest of the paper. Thus the writing is brought out in 
 burning lines. 
 
 Drawings made with this ink are invisible until brought out by 
 the moving spark of flre. The effect is most mysterious. The best 
 results are obtained by using soft paper which absorbs the liquid 
 fairly well and by making the lines rather heavy. 
 
 Potassium nitrate is an oxidizing agent and oxidizes the paper 
 when the reaction has been started by the application of heat. 
 
 Experiment 10 — Making a Fuse. 
 
 Prepare a solution of Potassium Nitrate according to the direc- 
 tions in Experiment 8. Obtain a piece of ordinary white string two 
 or three feet long, place it in the solution in a test tube, and let it 
 
14 
 
 THE CHBMCRAPT BOOK 
 
 soak fcr three or four minutes. Remove the string, hang it up anl 
 when thoroughly dry, light cne end. It will burn just like a fuse, 
 and by regulating the length of the string it can be made to burn 
 for any desired length of time. 
 
 Save a few pieces of fuse for use in following experiments. 
 
 A reaction which takes oxygen away from a sub- 
 stance is called reduction, and substances which have a 
 strong attraction for oxygen so that they can take it 
 away from other substances are called reducing agents. 
 
 Experiment 11 — The Reduction of Logwood. 
 
 Place 1 measure of Logwood (No. 29) In a test tube % full of 
 water and warm the solution for a few moments until it becomes 
 a deep red color. Now pour the red solution into another test tube 
 and add 4 measures of Sodium Bisulphite (No. 5). 
 
 Upon shaking this solution you will find that it is bleached and 
 turned nearly colorless. The sodium bisulphite has removed 
 oxygen from the logwood, thus converting it into a nearly colorless 
 substance. 
 
 Experiment 12 — Bleaching with Sulphur Dioxide. 
 
 Place about 5 measures of Sodium Bisulphite (No. 5) and an 
 equal amount of Tartaric Acid (No, 14), or some vinegar, in a glass. 
 Pour in a few drops of water, smell cautiously and note the odor of 
 sulphur dioxide. 
 
 Hang in the glass some colored (red or blue) flowers and cover 
 the top with a saucer. In about 30 minutes the colored flowers will 
 be turned white. 
 
 Most yellow flowers do not bleach well and the experiment 
 works best on red, pink or blue flowers. If the flowers are dipped 
 in water to moisten them before being hung in the glass it helps 
 the action. 
 
 Some colored fabrics can also be bleached in this manner, but 
 not all dyes are bleached by this particular compound. 
 
 Sodium bisulphite when treated with acids gives off sulphur 
 dioxide, a gas which is a powerful reducing agent, and hence an 
 exce'lent bleaching agent for many colored compounds. 
 
 HYDROGEN 
 
 Hydro,2:en is a color- 
 less, odorless gas. It is 
 more than fourteen times 
 as light as air and about 
 eleven thousand times as 
 light as water. Because 
 of its lightness it is fre- 
 quently used in ballons 
 and airships to make 
 them rise in the air. 
 Small amounts of hydro- 
 
THE CHEMCRAFT BOOK 15 
 
 gen occur in the atmosphere in the free state, but in com- 
 bination it occurs almost everywhere, being found in 
 water, in petroleum and in all animal and vegetable sub- 
 stances. 
 
 Experiment 13 — Preparation of Hydrogen. 
 
 Put 4 measures of Sodium Bisulphate (No. 7) and 5 measures 
 of Ammonium Cliloride (No. 9) in a test tube and fill Vi full of 
 water. Heat the solution over a candle flame for a few minutes, 
 allowing it to boil until the solids are completely dissolved and the 
 liquid appears perfectly clear. 
 
 Now add 1 measure of Powdered Zinc (No. 11) to the solution 
 in the test tube. Notice the violent action which occurs due to 
 the ©volution of a gas. This gas is hydrogen. 
 
 Hydrogen gas is inflammable. WTien burned it unites with the 
 oxygen of the air, forming water, which passes away as vapor, 
 steam. 
 
 When sodium bisulphate and ammonium chloride are boiled 
 together, a solution of hydrochloric acid is formed. Acids react 
 with many metals, liberating hydrogen and forming salts. Thus in 
 the case of the zinc, we had formed zinc chloride, a salt, which re- 
 mained dissolved in the water, and hydrogen which came off as a 
 gas. 
 
 WATER 
 
 The great quantity of water which occurs in natura 
 makes it one of the most familiar chemical substances. 
 Like oxygen, water is essential to the existence of life. 
 It is present in the air, in the ground, and in animal and 
 vegetable tissues. Water is a compound of two elements, 
 oxygen and hydrogen, both of which are gases. 
 
 A great many substances may be dissolved in water. 
 A body is dissolved or "in solution" when it is so finely 
 divided, and its particles are so completely scattered 
 through a liquid that they can neither be seen nor sep- 
 arated from the liquid by filtering. The substance may 
 in most cases be recovered in its original state by evap- 
 orating off the liquid. 
 
 Experiment 14 — Solution. 
 
 Dissolve a spocnful of common table salt (not included in out- 
 fit) in half a glass of water. 
 
 Now j)0ur this solution into a small pan or similar cooking 
 utensil and heat on the stove until the water is all driven off. Taste 
 what you find remaining in the pan and satisfy yourself that it is the 
 same salt with which you started. 
 
 Unless the pan is heated very gently when the salt is near'.y dry 
 you will find there will be some violent popping due to the expan- 
 
16 THE CHEMCRAPT BOOK 
 
 sion of steam in the crystals of salt. This does no harm except to 
 throw about some of the salt. 
 
 Experiment 15 — Diffusion. 
 
 Fill a clean glass nearly full of water and let it stand for a 
 minute or two to become quiet. Now add a small particle of Mixed 
 Dyes (No. 30) and watch closely what occurs. 
 
 As the dye dissolves the color seelns to flow out of the mass 
 in a stream until it finally reaches the bottom of the glass. After 
 a few moments the color will begin to diffuse through the liquid 
 until finally after several hours the entire solution will be a uni- 
 form color. 
 
 Most chemicals I'eact much more readily if they are 
 dissolved in water, as this permits the particles to come 
 into closer contact. 
 
 Experiment 16 — The Effect of Solution on Chemical 
 Reaction. 
 
 Mix together on a sheet of paper 1 measure of Sodium Bicarbo- 
 nate (No. 25) and 1 measure of Tartaric Acid (No. 14). The dry 
 mixture shows no sign of any chemical reaction. 
 
 Now put this mixture in a test tube and add a drop or two of 
 water. Immediately a violent reaction occurs, liberating much gas. 
 
 Many salts absorb heat when they dissolve. Thus it 
 is possible to lower the temperature of water by dissolv- 
 ing certain salts. 
 
 Experiment 17 — The Effect of Solution on Temperature. 
 
 Fill a test tube half full of water and note the temperature by 
 feeling the outside of the glass. Now add 5 measures of Potassium 
 Nitrate (No. 8) to the water in the test tube again and notice the 
 change in temperature. 
 
 Water normally freezes at zero degrees Centigrade 
 (32 degrees Fahrenheit), but under certain conditions 
 it may be cooled considerably below this temperature 
 without freezing. 
 
 Experiment 18 — Undercooled Water. 
 
 Obtain a tumbler full of crushed ice and mix in 2 or 3 spoon- 
 fuls of ordinary table salt. Now place a clean test tube about % 
 full of pure water in this mixture. Do not allow any of the salt or 
 ice to get Into the test tube. 
 
 If kept perfectly quiet the water in the test tube may be cooled 
 to minus 4 to 5 degrees Centigrade (25 degrees Fahrenheit) or 
 
THE CHEMCRAPT BOOK 17 
 
 even to minus 10 degrees Centigrade (15 degrees Pahrenlieit) with- 
 out solidifying. If this undercooled water is stirred, or if a tiny 
 crystal of ice is added, it immediately freezes and the temperature 
 rises to zero degrees Centigrade (32 degrees Fahrenheit). 
 
 Most substances are very much more soluble in hot 
 water than in cold water. This fact is made use of by 
 the chemist in many ways. 
 
 Experiment 19 — The Effect of Temperature on Solubility. 
 
 Put 6 measures of Nickel Ammonium Sulphate (No. 13) in a 
 test tube % full of water. Close the end of the test tube with your 
 thumb and shake for a few minutes. Notice that the nickel ammo- 
 nium sulphate will not completely dissolve in this amount of cold 
 water. Now heat the test tube for a few minutes and the solid will 
 entirely dissolve. 
 
 Set the test tube aside and allow the solution to cool slowly. 
 After one or two hours crystals of nickel ammonium sulphate will 
 form in the solution and gradually grow larger. 
 
 It is an invariable rule that the more slowly crystals 
 are formed the larger they will be. 
 
 Experiment 20 — The Formation of Crystals. 
 
 Put 6 measures of Boric Acid (No. 2) in a test tube and fill % 
 full of water. Boil for a minute to dissolve the boric acid, then 
 set aside and let the solution cool slowly. After 15 or 20 minutes 
 a heavy deposit of white frost-like crystals will be formed in the 
 test tube. 
 
 Repeat the experiment, but cool the solution rapidly, as soon as 
 the boric acid has all dissolved, by setting the test tube in a glass 
 half full of cold water. The crystals obtained this time will be 
 much smaller than in the first case where the solution was cooled 
 slowly. 
 
 Water is contained in many solid dry substances in 
 a state of chemical combination. For example, some 
 crystals contain what is called "water of crystallization." 
 
 Experiment 21 — Water of Crystallization. 
 
 Drop 1 measure of Nickle Ammonium Sulphate (No. 13) into 
 a clean dry test tube and heat the bottom of the tube with a ilame, 
 using the test tube holder so as not to burn your fingers. Do not 
 hold the tube in the flame, as this will cause soot to deposit. Rather 
 hold it about Vz inch above the top of the flame. 
 
 Note that the green powder becomes wet and water is driven 
 off in the form of steam. Heat until all the water is driven off. 
 The substance remaining will be a dark yellow color, which 
 gradually turns yellow tinged with green. 
 
 Aluminum Sulphate (No. 12), Ferric Ammonium Sulphate (No. 
 21), Ferrous Ammonium Sulphate (No. 17), and ordinary washing 
 soda also contain water of crystallization. Heat small quantities of 
 
18 THE CHEMCRAPT BOOK 
 
 some of these substances and notice the change which occurs when 
 the water of crystallization is driven oft. 
 
 Ordinary washing soda is a good example of a substance con- 
 taining water of crystallization. If you are familiar with this ma- 
 terial you know that it sometimes comes in clear, nearly trans- 
 parent crystals, while other times it is covered with white powder 
 and is very dusty. This is because washing soda loses part of its 
 water of crystallization when it is exposed to the air, and the white, 
 dusty powder has probably been stored so long that much of the 
 water has been lost. It is just as well to remember, however, that 
 a pound of washing soda which has lost part of its water contains 
 much more soda than a pound of the big, good looking crystals 
 which still have water in them. 
 
 Experiment 22 — Dissolving Solids in Their Water of 
 Crystallization. 
 
 Put 1 measure of Ammonium Chloride (No. 9) and 1 measure 
 of Sodium Thiosulphate (No. 16) in the palm of your hand and 
 rub them together with your fingers. In a few minutes the solids 
 will become moist, and will gradually dissolve in their water of 
 crystallization. Be sure to wash your hands immediately after 
 working this experiment. 
 
 Experiment 23 — Testing for Traces of Moisture. 
 
 A convenient method of testing for small traces of moisture 
 is as follows: 
 
 Prepare a solution of 2 measures of Ferric Ammonium Sul- 
 phate (No. 21) in a test tube half full of water. Saturate some 
 strips of smooth white paper with this solution and dry the strips. 
 When you are ready to use them place half a measure of Sodium 
 Ferrocyanide (No. 6) on one of the dry strips and spread it over 
 the surface by means of a soft brush or wad of cotton. 
 
 The slightest trace of moisture produces dark blue spots on 
 these strips. Hold a strip over the mouth of the test tube in Ex- 
 periment 21. 
 
 Experiment 24 — Sympathetic Ink. 
 
 Dissolve 1% measures of Cobalt Chloride (No. 27) in a test 
 tube Vz full of water. Wj'iting done with this solution shows blue 
 when the paper is heated and disappears again on cooling. 
 
 Write with a clean pen on white paper. To bring out the writ- 
 ing warm the paper. If heated too hot so that the paper is scorched 
 the ink will not disappear on cooling because of the formation of 
 cobalt oxide. 
 
 Cobalt Chloride is blue, but in the presence of moisture it takes 
 up water of crystallization and becomes pale pink in color. Even 
 the small amount of water in the air is sufficient to cause the blue 
 color to become more or less pale and pinkish. 
 
 On heating the writing the water is driven away and the cobalt 
 chloride in the ink shows blue. On cooling, it absorbs moisture 
 from the air and turns pale pink, so that it is not easily seen. Soma- 
 
THE CHEMCRAFT BOOK 19 
 
 Jimes when the air is quite hot and dry, as in heated houses in the 
 winter time, the blue requires a very long time to fade away. 
 
 This same substance is often used as a sort of chemical baro- 
 meter. A sheet of white paper is moistened with a conoentrated 
 solution and allowed to dry. It is then hung up some place where 
 the outside air will circulate freely around it, but where the rain 
 will not reach it. 
 
 When it looks bluish it is an indication of dryness and usually 
 of continued fair weather. When it is pink in color it indicates 
 wet or moist weather. 
 
 Experiment 25 — The Dehydration of Cobalt Chloride. 
 
 To illustrate more clearly the change which takes place in 
 Experiment 24, try the following: 
 
 Place 1 measure of Cobalt Chloride (No. 27) in the spoon, notice 
 that the color is pink. Now heat the spoon very gently until the 
 cobalt chloride just changes to a blue color. The water of crystal- 
 lization has been driven off, or in other words, it has been dehy- 
 drated. 
 
 Now add 1 to 2 drops of water to the blue cobalt chloride in 
 the spoon, mix it around and notice that the mass becomes pink 
 again. The cobalt chloride has taken up water of crystallization 
 or has been rehydrated. This change can be repeated as often as 
 you like. 
 
 Experiment 26 — Permanent Sympathetic Ink. 
 
 Dissolve 4 measures of Sodium Bisulphate (No. 7) in a test 
 tube half full of water. 
 
 Using a clean pen, write with this solution on white paper. 
 The writing cannot be seen until the paper is heated, when it ap- 
 pears in dark brown lines. This writing is permanent and will not 
 disappear. 
 
 It is possible to prepare supersaturated solutions of 
 some substances, that is, solutions which contain more 
 of the substances than is normal for the temperature 
 of the solution. Such solutions are very unstable and 
 will crystalize suddenly if given a proper start. 
 
 ExI^eriment 27 — A Supersaturated Solution. 
 
 Fill a test tube 1-3 full of Sodium Thiosulphate (No. 16). Add 
 exactly 2 drops of water and warm gently. The sodium thiosul- 
 phate will melt in its own water of crystallization, and the warm- 
 ing should be continued until the crystals are completely dissolved 
 and the solution is almost boiling. Now close the end of the tesi, 
 tube with a plug of cotton and allow it to stand without moving 
 or shaking until cool. 
 
 You now have a supersaturated solution. To start crystalliza- 
 tion drop in a crystal of Sodium Thiosulphate the size of a pin head 
 and watch carefully for a few minutes to see the crystals grow. 
 
20 THE CHBMCRAPT BOOK 
 
 THE HALOGEN FAMILY 
 
 There are four elements whose chemical properties 
 resemble each other very closely, and which the chemist 
 has named the Halogen family. The elements belonging to 
 this family are: Fluorine, Chlorine, Bromine and Iodine. 
 Fluorine is a colorless gas, Chlorine is a greenish gas. Bro- 
 mine is a reddish brown liquid or gas and Iodine is a gray 
 sohd which when heated changes into a purple gas. 
 
 Chlorine is a heavy unbreathable gas with a suffocat- 
 ing odor and astringent taste. It is the most interesting 
 as well as the most useful of the Halogens. It is used as 
 a bleaching and disinfecting agent, and in the extracting 
 of gold from its ores. Chlorine gas also played an im- 
 portant part early in the 
 recent war. The gas was 
 generated on a very large 
 scale and liberated when 
 conditions were favorable 
 for blowing it into the 
 trenches of the enemy. The 
 only protection from an at- 
 tack of this sort is obtain- 
 ed by wearing respirators which prevent the breathing 
 of the gas into the lungs. Later, other, even more deadly 
 gases were used. 
 
 Experiment 28 — Preparation and Properties of Chlorine. 
 
 (a) — Preparation. 
 
 Put 3 measures of Sodium Bisulphate (No. 7), 3 measures of 
 Potassium Nitrate (No. 8) and 3 measures of Sodium Chloride 
 (common table salt) in a test tube and heat the mixture over a 
 flame for a few minutes. Cautiously smell the gas which is evolved. 
 
 (b) — Tests for Chlorine. 
 
 Obtain a small lump of starch about the size of a pea (or 1 
 measure of powdered starch) and mix thoroughly with a few drops 
 of water in a glass. Pour the mixture into a test tube half full of 
 hot water, add 3 or 4 drops of Sodium Iodide Solution (No. 23) and 
 boil for a minute. Now dip a strip of white paper into this solution 
 and hold it over the mouth of the test tube in which you are gen- 
 erating chlorine gas. Heat the te?t tube to drive off the gas freely, 
 and notice the blue coloration which appears on the paper. The 
 color will disappear if the paper is exposed to the chloride gas very 
 long. This is a very delicate test for chlorine. 
 
 (c) — Bleaching with Chlorine. 
 
 Obtain a few pieces of different colored paper and cloth; wet 
 them with water and put them In a glass. Cut a piece of heavy 
 paper large enough to cover the top of the glass and make a small 
 hole in the center. 
 
THE CHEMCRAPT BOOK 21 
 
 Now fit the test tube in which chlorine is being generated with 
 the perforated corlt and delivery tube. Heat the test tube and pass 
 chlorine gas through the hole in the paper into the glass contain- 
 ing the pieces of wet cloth and paper. In a short time the colors 
 will be bleached. 
 
 Chlorine is one of the most powerful bleaching agents known. 
 
 Experiment 29 — Hydrogen Chloride. 
 
 Place in a test tube 1 measure of Sodium Bisulphate (No. 7) 
 and 2 measures of Ammonium Chloride (No. 9). Heat the mixture 
 over a candle flame for a few minutes. When a quantity of fumes 
 is given off moisten a piece of Blue Litmus Paper (No. 18) and 
 hold it at the mouth of the tube for a moment. Notice that It is 
 turned red, showing the presence of an acid. Take the test tube 
 away from the flame and cautiously smell the gas which is coming 
 off. It is hydrogen chloride. 
 
 This gas when dissolved in water forms hydrochloric or muri- 
 atic acid. 
 
 If you have some household ammonia dip your glass rod into 
 it and then hold the rod at the mouth of the test tube. The white 
 fumes are ammonium chloride and are an example of smoke with- 
 out flre. 
 
 Hydrochloric acid is a compound of hydrogen and chlorine. It 
 is manufactured commercially by heating sodium chloride (common 
 table salt) with sulphuric acid. 
 
 Experiment 30 — Another Method of Preparing Hydrogen 
 
 Chloride and Chlorine. 
 
 Heat together in a test tube 1 measure of Sodium Bisulphate 
 (No. 7) and 2 measures of Ammonium Chloride (No. 9) as in ex- 
 periment 29. When fumes of hydrochloric acid are given off stop 
 heating for a moment and add 2 measures of Patassium Nitrate 
 (No. 8). Continue heating for a minute or so longer and smell cau- 
 tiously. Notice that hydrogen chloride is no longer coming off, but 
 instead, chlorine gas is being evolved. 
 
 CARBON— COMBUSTION— CARBONATES 
 
 Carbon is an element which is found in all living mat- 
 ter and in all substances which are made from living or 
 growing things. Your food, your clothing and you, your- 
 self, are largely made of carbon compounds. Carbon and 
 many of "its compounds unite readily with oxygen and 
 give off heat in doing so, in other words they burn. It is 
 because wood and coal consist mainly of carbon that they 
 are so valuable as fuels. 
 
 When carbon burns it unites with oxygen to form 
 the compound c arbon dioxide , which is gas. 
 
22 THE CHEMCRAFT BOOK 
 
 Experiment 31 — A Test for Carbon Dioxide in Products 
 of Combustion. 
 
 Place 5 measures of Calcium Oxide (No. 26) in half a glass of 
 water and stir for several minutes. Let stand until the powder has 
 settled to the bottom and then pour off the clear liciuid into another 
 glass. This liquid is lime water. 
 
 Now repeat Experiment 7, but after the candle has gone out 
 remove the jar or bottle from the water and quickly pour In a little 
 of the clear lime water. Put your hand over the mouth and shake 
 violently for a moment. 
 
 If you will look closely you will see that the lime water is now 
 turbid with white particles. Carbon dioxide unites with lime water 
 to form calcium carbonate which is white and is not soluble in 
 water. Hence the formation of this white turbidity is a test for 
 carbon dioxide and shows that this gas is formed by the burning 
 of the carbon of the candle. 
 
 Experiment 32 — The Structure of Flame — A Gas Factory. 
 
 If you will look closely at a candle flame you will see 
 that it consists of three parts. /y, 
 
 First, a dark zone just around the wick. 
 
 Second, a bright yellow zone which gives the light. 
 
 Third, a transparent zone of heat around the outside. 
 
 The first or inner zone consists of unburned gas given 
 off from the wick of the candle. The melted grease is 
 drawn up by capillary action into the wick and is there 
 converted into gas by the heat of the flame. With care a '.\[ ' 
 portion of this gas can be drawn off through a tube. 
 
 Hold one end of the glass tube in the flame and directly 
 over the wick. Hold the tube slanting upwards so that the 
 other end is out at the side and a little above the flame. If 
 held correctly smoke will come from the end of the tube 
 and can be lighted with a match. 
 
 That it is relatively cool inside of the flame can be shown by 
 thrusting a match stick into this zone for a few seconds. The por- 
 tion of the stick which was held in the dark zone will not be burned 
 so soon as that portion passing through the sides of the flame. 
 
 Experiment 33 — The Structure of I'lame — Manufactur- 
 ing Lampblack. 
 
 The second or bright yellow zone of the flame contains particles 
 of carbon heated to a white heat so that they glow brightly. The 
 carbon is formed by the action of the heat on the gas of the inner 
 zone. 
 
 The presence of this carbon can be shown by holding a cold 
 spoon or piece of glass tubing in the flame for about a minute. You 
 will notice that when you take it out it is covered with a black de- 
 posit of lampblack or soot which is one form of carbon. The cold 
 spoon chills the flame and prevents the carbon from being com- 
 pletely burned. 
 
 Lampblack is made on a large scale in just this way except that 
 
THE CHEMCRAFT BOOK 23 
 
 natural gas is burned instead of candles and the cooling is done by 
 means of iron pipes with water circulating through them. 
 
 The third or outside zone of the flame consists of the gases 
 formed by the complete burning of the carbon particles. If you will 
 hold the cold spoon in this outer zone you will find that it gets very 
 hot but that no soot or only a very small amount will be deposited. 
 This zone is above the luminous part. 
 
 Wood, oil and many other fuels contain hydrogen com- 
 bined with carbon and when burned this hydrogen unites 
 with oxygen from the air to form water, hydrogen oxide 
 
 Experiment 34 — Making Water from Fire. 
 
 Take a cold, dry glass and invert it over a lighted candle, holding 
 the mouth just above the flame. After a few seconds remove the 
 glass and examine the inside. You will find that a film of moisture 
 has been deposited on the inside of the cold glass. 
 
 Water is liberated from the flame in the form of steam, and in 
 order to make it visible it must be condensed on some cold object. 
 
 Breathing is a form of combustion. The oxygen of 
 the air that we take into our lungs combines with the 
 carbon and hydrogen of the food we have eaten, and the 
 heat that is generated by this combustion serves to keep 
 our bodies warm. Just as in the case of the burning 
 candle, carbon dioxide is formed by this reaction and is 
 therefore present in the breath we expel. 
 
 Experiment 35 — Test for Carbon Dioxide in the Breath 
 —"Bugs in the Breath." 
 
 Prepare half a glass of clear lime water according to the direc- 
 tions given in Experiment 31. 
 
 Using the piece of glass tubing blow through the lime water. 
 You will flnd that as your breath bubbles through the liquid it 
 causes it to turn white and turbid, thus showing the presence of 
 carbon dioxide. 
 
 The white precipitate is calcium carbonate, which is soluble in 
 most acids. Stir in a little vinegar, or 3 measures of Tartaric Acid 
 (No. 14) and see the turbidity disappear. 
 
 I remember one time seeing a "Medicine Man" who made use 
 of this reaction in selling a so-called consumption cure to ignorant 
 people. After getting a crowd about him he would pick out some 
 poor fellow and say: 
 
 "Friend, you have consumption. You don't know it but I see 
 it in your face. Now I'll prove it to you. Your breath is just chuck 
 full of germs. You come here and I'll show them to you. Here, 
 blow through this and we will catch them in the glass." 
 
 He has his victim blow through some lime water until it turns 
 white. Then he goes on: 
 
 "See here, folks, the liquid's white with consumption germs. 
 
24 THE CHEMCRAFT BOOK 
 
 Now I'll show you how Smither's Specific kills the dread disease." 
 Then pouring some diluted acid into the glass, the turbidity 
 disappears and he says: "There, clear as crystal! Smither's 
 Specific just naturally eats those germs right up. Now, friend, you 
 don't want to die in the prime of your young manhood. Buy a bot- 
 tle and cure yourself. One dollar please. Thank you — who's next?" 
 The experiment carried out along these lines makes a very 
 good trick on credulous people, and is very perplexing to anyone 
 not familiar with its chemistry. 
 
 When wood, coal and similar substances are heated, 
 and no air or oxygen is permitted to get to them they do 
 not burn, but the hydrogen, nitrogen, and portion of the 
 carbon which they contain are driven off in the form of 
 gas and tar, while most of the carbon is left behind as 
 charcoal or coke. This process of heating without access 
 of air is the means of obtaining many valuable chemicals 
 and forms the basis of enormous industries. 
 
 When coal is heated in this way, coal gas, tar and 
 crude ammonia are obtained. The gas is used for light- 
 ing and heating; the crude ammonia is purified and used 
 in various ways, while from the tar are obtained all ani- 
 line dyes, many drugs used in medicine, disinfectant com- 
 pounds such as creosol and carbolic acid, the materials 
 from which many of the modern high explosives are 
 m.ade, and a multitude of other valuable products. 
 
 When wood is distilled in this way, gas, tar and a 
 liquid containing acetic acid (wood vinegar) , wood alcohol 
 and other valuable products are obtained. 
 
 Experiment 36 — The Distillation of Wood. 
 
 Break the heads off of 5 or 6 matches and put the sticks in the 
 bottom of a test tube. Now heat, using your test tube holder, over 
 an alcohol lamp or gas flame (a candle flame is not hot enough to 
 give the best results in this experiment). 
 
 . When smoke begins to come off from the wood hold a piece of 
 moistened Blue Litmus Paper (No. 18) in the mouth of the tube. 
 Note that it is turned red, showing that there is acid in the gas. 
 Now fit the test tube with your gas delivery tube, continue heating 
 and light the gas as it comes from the end of the tube. You will 
 find that the gas is inflammable and after the distillation has con- 
 tinued for a few minutes it will burn as it comes out of the tube. 
 
 Continue heating until gas no longer comes off, then let the 
 test tube cool and empty out the charcoal which remains, using 
 your stirring rod to loosen it from the sides if necessary. Char- 
 coal is practically pure carbon. 
 
 Many chemicals contain carbon in such a form that it 
 is easily liberated as carbon dioxide. Such compounds are 
 
THE CHBMCRAPT BOOK 25 
 
 known as carbonates. When carbonates are brought in 
 contact with acids and carbon dioxide is given off as gas. 
 
 Experiment 37 — The Manufacture of Carbon Dioxide — 
 Chemical Boiling. 
 
 Place 2 measures of Sodium Bicarbonate (No. 25) in a test tube 
 and fill 1-3 full of water, shaking well to dissolve all the solid. In 
 another test tube containing an equal volume of water put 1% mea- 
 sures of Tartaric Acid (No, 14) and shake well. Now pour the con- 
 tents of the second tube into the first. 
 
 The liquid will boil violently due to the evolution of carbon 
 dioxide gas. 
 
 Smell the gas. It is the same as that used in soda water to 
 make it foam and give it the sparkling taste. 
 
 Ordinary baking soda is sodium bicarbonate. When heated it 
 gives off part of the carbon dioxide gas which it contains, so when 
 used in biscuit, cake, etc., the gas coming off "raises" the dough 
 and makes it porous and light. 
 
 Experiment 38 — Some Properties of Carbon Dioxide. 
 
 Carbon Dioxide gas is heavier than air and may be poured al- 
 most like water. It will not support combustion. 
 
 Obtain a small quantity of baking soda and half a glass of vine- 
 gar. Place a candle in a tumbler or other similar vessel, so that 
 when lighted the top of the flame will be just below the top of the 
 tumbler or vessel. Now put a teaspoonful of baking soda in a glass 
 and add a small quantity of vinegar. There will be a violent boil- 
 ing or effervescence and carbon dioxide gas will be given off. While 
 this action is going on, hold the glass over the vessel in which the 
 candle is burning and pour the carbon dioxide gas over the candle. 
 Tilt the glass as though you were pouring water from it, but do not 
 allow any of the liquid to come out. In a short time the candle will 
 be extinguished although it may be necessary to add a little more 
 vinegar to the glass in which the carbon dioxide is being generated. 
 
 The relatively great weight of carbon dioxide as compared with 
 air is responsible for its accumulation in abandoned mines, old 
 wells, etc., and such places should always be tested by lowering a 
 lighted candle into them before 'people descend, as otherwise suf- 
 focation may result. 
 
 Some hand iire-extinguishers and most chemical fire-engines 
 make use of carbon dioxide. They contain sodium bicarbonate 
 (baking soda) and sulphuric acid held in separate containers and 
 are so arranged that when the extinguisher is turned upside down 
 the chemicals are mixed and carbon dioxide is generated. Because 
 of the weight of this gas it may be directed by a nozzle on to the 
 fire and thus made to extinguish the flame. 
 
 The small, hand fire-extinguishers which are so largely used on 
 automobiles and in homes contain a liquid called Carbon Tetra- 
 chloride. This liquid when heated is converted into a heavy gas. 
 which will not burn. When Carbon Tetra-Chloride from these small 
 fire-extinguishers is squirted on to a fire, the liquid is turned into 
 this heavy gas which smothers the flame in the same manner as 
 Carbon Dioxide. 
 
26 THE CHEMCRAFT BOOK 
 
 Experiment 39 — Acid Properties of Carbon Dioxide. 
 
 Prepare a solution of 1 measure of Sodium Carbonate (No. 4) 
 in half a glass of water. Add 1 drop of Phenolphthalein Solution 
 (No. 22), which will turn the water red, proving it to be alkaline. 
 Now fiill a test tube about % full with the solution in the tumbler. 
 
 In another test tube put 4 measures of Sodium Bicarbonate 
 (No. 25) and 4 measures of Sodium Bisulphate (No. 7). Fill the 
 tube 1-3 full of water and quickly fit with the gas delivery tube and 
 stopper. Now place the end of the gas delivery tube In the solution 
 in the first test tube which is colored pink, and let the carbon 
 dioxide gas bubble through this solution. After several minutes 
 you will find that the pink color has disappeared and the solution 
 is now colorless, due to the fact that carbon dioxide when dissolved 
 in water forms carbonic acid and this changes phenolphthalein solu- 
 tion from red to colorless. It may be necessary to renew the so- 
 dium bicarbonate and sodium acid sulphate in the carbon dioxide 
 generator before the phenolphthalein solution is made completely 
 colorless. 
 
 Experiment 40 — Testing Household Materials for Car- 
 bonates. 
 
 Test the materials suggested below for carbonates by placing 
 4 measures of the specified material in a test tube and adding 3 
 measures of Sodium Bisulphate (No. 7) and a little water. Warm 
 the mixture gently. If necessary, to start the reaction, and when a 
 gas is given off, test for carbon dioxide by means of lime water 
 made as described in Experiment 31. 
 
 The test may be performed in either of two ways. It is con- 
 veniently carried out by dipping the glass tube into clear lime 
 water. Place your finger over the upper end to prevent the liquid 
 from running out and then hold the liquid in the tube a short dis- 
 tance above the mixture in the test tube. If the lime water be- 
 comes cloudy or white it shows the presence of carbon dioxide gas. 
 
 The other method of testing may be carried out as follows: 
 
 Fit the test tube in which the gas is bein? generated with the 
 gas delivery tube and stopper. Fill another clean test tube about 
 A full of clear lime water and pla.ce the end of the sas delivery 
 tube in the lime water so that the gas will bubb'e through it. If 
 the solutkn of lime water becomes cloudy or white it shows that 
 the gas is carbon dioxide. 
 
 Test in the manner described above, any of the following sub- 
 stances: 
 
 Bakins S"da (sodium bicarbonate), Washing Soda (sodium car- 
 bonate). Baking Powder (a mixture of sodium bicarbonate with 
 calcium acid tartrate, calcium acid phosphate or alum), oyster 
 shells (whxh consist chiefly of calcium carbonate), chalk, tooth 
 powder, plaster (which also contain calcium carbonate). 
 
 The same test may be applied to the gas given oft by foaming 
 beverages, such as soda water, ginger ale, etc. 
 
 Since carbon dioxide is formed when fuels burn, and 
 is given off in our breathing, we might expect to find a 
 
THE CHEMCRAPT BOOK 27 
 
 small quantity present in the air about us. That the air 
 does contain carbon dioxide is readily shown by the fol- 
 lowing experiment. 
 
 Experiment 41 — Limestone Ice. 
 
 Make up ha]f a glass of lime-water according to the directions 
 given in Experiment 31, Pour (his into a saucer, and let it stand 
 over night. Do rot put a cover over the saucer. In the morning 
 ycu will find that a thin v/hite crust has formed over the surface 
 of the liquid. 
 
 This crust crnsists of calcium carbonate and is the same thing 
 cheraical'y as limestone rock. It is formed by the action of the 
 carbon dioxide in the air en the lime-water. 
 
 NITROGEN 
 
 The elem.ent nitrogen is an inert gas. It occurs in the 
 air mixed with oxygen. The compounds of nitrogen are 
 among the most interesting and valuable known to the 
 chemist. With h^/drogen and oxygen, nitrogen forms 
 nitric acid, from which is made most of our high explo- 
 sives. Nitrogen is essential to the growth of plants and 
 its compounds are used largely in fertilizers. Animal life 
 also contains a large portion of nitrogen. 
 
 Nitrogen combines with hydrogen to form the com- 
 pound ammonia. Crude ammonium salts are obtained 
 from the distillation of coal and from these pure ammonia 
 is made by treatment with hme or other alkali. 
 
 Experiment 42 — The Manufacture of Ammonia. 
 
 Place 2 measures of Ammonium Chloride (No, 9) and 2 mea- 
 sures of Calcium Oxide (No. 20) in a test tube. Notice that neither 
 of these chemicals has any smell before they are mixed together. 
 Gently heat the mixture over a candle flame and after a moment 
 smell cautiously; also test with moistened Red Litmus Paper (No. 
 18). This simple experimeDt illustrates the way in which am- 
 monia is made on a large scale. 
 
 Ammonia gas is very so'uble in water and the liquid or house- 
 hold ammonia which is commonly used, is a solution of this gas in 
 water. 
 
 Experiment 43 — Another Method of Preparing Ammonia. 
 
 Place 2 measures of Ammcnium Ch'oride (No. 9) in a test tube 
 as before, but this time add 2 measures of Sodium Carbonate (No, 
 4). Heat the mixture gently and notice the smell of ammonia in 
 the mouth of the test tube. 
 
 Experiment 44 — Making Ammonia in Your Hand. 
 
 Put 1 measure of Calcium Oxide (No. 20) and 1 measure o£ 
 
28 THE CHEMCRAFT BOOK 
 
 Ammonium Chloride (No. 9) in the palm of your hand and mix the 
 substances together with your fingei". Smell the mixture occa- 
 sionally and notice that ammonia gas is being given off. 
 
 Ammonium Salts are readily volatile, and some of 
 them pass into the form of vapor without first melting. 
 
 Experiment 4.5 — Volatilization of Ammonium Com- 
 pounds. 
 
 Put 1 measure of Ammonium Chloride (No. 9) into a clean dry 
 test tube. Heat gradually over the candle flame, being careful not 
 to get the bottom of the test tube sooty. Notice how the ammonium 
 chloride volatilizes and how the vapor condenses on the upper part 
 of the test tube. 
 
 Experiment 46 — Nitrogen Compounds. 
 
 Take 2 measures of Potassium Nitrate (No. 8), 1 measure of 
 Sulphur (No. 1) and 1 measure of powdered Charcoal (made by 
 crushing up burned match sticks). Mix these substances thoroughly 
 on a sheet of paper, but do not grind or rub hard. 
 
 Now pour the mixed powders into a little pile on a pan and 
 drop a lighted match on it, keeping your hands and face at a. dis- 
 tance. It will go off with a puff. If you have saved some pieces of 
 fuse from Experiment 9, the mixture may be lighted by imbedding 
 one end of the fuse in it and lighting the free end. 
 
 Gunpowder is a mixture of potassium nitrate, sulphur and char- 
 coal finely ground, mixed together and formed into grains. It was 
 originally invented by, the Chinese. Since the discovery of modern 
 high explosives such as nitro-glycerine, gun cotton, picric acid, etc., 
 gunpowder Is used very little except for blasting and fireworks. 
 
 SULPHUR 
 
 Sulphur is a very useful element. From it is made 
 sulphuric acid, one of the most powerful acids, and a 
 necessity in many large industries. In fact, sulphuric 
 acid enters in some way or other into the manufacture of 
 about 90 per cent of the things which we use in our daily 
 life, such as food, clothing, etc. 
 
 Sulphur is obtained from the craters of volcanoes 
 in Italy, Mexico and Japan, and there are also important 
 mines in Louisiana where the sulphur is melted in the 
 ground by superheated steam and pumped out of wells. 
 
 Experiment 47 — The Properties of Sulphur. 
 
 Put 2 measures of Sulphur (No. 1) into a dry test tube and heat 
 gently over a flame. 
 
 Notice that it first melts to a dark liquid and is then converted 
 
THE CHEMCRAPT BOOK 29 
 
 into vapor. The vapor condenses again in the cool upper part of the 
 tert tube. 
 
 Now put 2 measures of sulphur in a spoon and heat this over 
 the flame. While the sulphur is burning smell it cautiously. 
 
 In the test tube the sulphur did not burn because not enough 
 air could get to it, but when heated in the spoon it unites with the 
 oxygen of the air, forming the gas, sulphur dioxide. In Experiment 
 12 you made this same gas by another method. 
 
 Sulphur has no smell; try it. What is usually spoken of as the 
 odor of sulphur or brimstone is the smell of sulphur dioxide. 
 
 Experiment 48 — Elastic Sulphur. 
 
 Put 5 measures of Sulphur (No. ] ) in the spoon and heat over 
 the alcohol lamp flame until the sulphur has melted and is fluid. 
 Now quickly pour the melted sulphur into a glass of water. After a 
 few moments remove the mass of sulphur from the water and ex- 
 amine it. You will find it is an elastic substance resembling rubber 
 more than anything else. 
 
 Sulphur exists in several different physical forms of which the 
 "elastic" or "gamma" sulphur is one. Afler a long time this elastic 
 sulphur will change back into the ordinary form. 
 
 Experiment 49 — Preparation and Properties of Hydrogen 
 Sulphide. 
 
 (a) — Preparation. 
 
 Cut a piece of parafflne about as big as the end of your little 
 finger from your candle and place this, together with 5 measures 
 of Sulphur (No. 1), in a test tube. Heat over the candle flame, 
 and after several minutes smell the gas which is given off. This 
 is the same gas that was prepared in Experiment 1, when sodium 
 bisulphate was added to zinc sulphide. 
 
 (b) — Properties. 
 
 Fit the perforated cork and delivery tube to the test tube in 
 which hydrogen sulphide is being generated. Heat the test tube 
 and when the gas is being given off rapidly, apply a flame to the 
 open end of the delivery tube. The gas will burn with a blue flame. 
 When hydrogen sulphide burns in the air the sulphur and hydrogen 
 unite with oxygen, forming sulphur dioxide and water. If, how- 
 ever, insufficient air is present only the hydrogen burns, and sul- 
 phur is set free. Hold a cold piece of glass in the blue flame for 
 an instant; notice the deposit of sulphur which is formed. 
 
 Put 2 measures of Sodium Bisulphite (No. 5) and an equal 
 amount of Tartaric Acid (No. 14) in another test tube, add a few 
 drops of water. Warm slightly and cautiously smell the gas which 
 is given off. It is sulphur dioxide. Now heat the test tube in which 
 hydrogen sulphide is being generated and using your delivery tube, 
 pass some of the gas into the test tube where sulphur dioxide is 
 being given off. A deposit of sulphur will be formed around the 
 walls of the tube. When hydrogen sulphide and sulphur dioxide 
 are mixed together they react, forming sulphur and water. This is 
 the way in which the great deposits of sulphur are formed in the 
 neighborhood of volcanoes. 
 
30 THE CHEMCRAPT BOOK 
 
 Moisten a bright penny witli water and liold it against the open 
 end of the delivery tube through which hydrogen sulphide is pass- 
 ing. In a short time a black spot will appear on the copper due to 
 the formation of copper sulphide. The same result can be obtained 
 with a silver coin, the stain in this case being silver sulphide. The 
 presence of small traces of sulphur compounds in the air is th^ 
 cause of the tarnishing of household silver. 
 
 Experiment 50 — Test for Hydrogen Sulphide. 
 
 Moisten a piece of Sulphide Test Paper (No. 31) and hold it in 
 the mouth of a test tube in which hydrogen sulphide is being gen- 
 erated (See Experiment 49, part a). The test paper will turn black, 
 due to the formation of lead sulphide. This is a very delicate test 
 for hydrogen sulphide. 
 
 Test your illuminating gas supply for hydrogen sulphide by 
 letting the gas from a jet flow against moistened sulphide test 
 paper. Illuminating gas is supposed to be purified and have all 
 hydrogen sulphide removed from it, but in some cases this is not 
 completely accomplished. 
 
 When cabbage is being cooked the steam arising from the pot 
 contains hydrogen sulphide, which can be detected with sulphide 
 test papers. The odor of boiling cabbage is due to hydrogen sul- 
 phide and other sulphur compounds. 
 
 The dark color in Experiment 50 is due to the action 
 of the hydrogen sulphide on the lead salt with which 
 the paper is impregnated. Lead sulphide, a black com- 
 pound, is formed. 
 
 The presence of small traces of hydrogen sulphide in 
 the air sometimes causes white paint to turn dark. White 
 paint generally contains either lead carbonate or zinc 
 oxide, and in case the paint contains the lead salt it is 
 very apt to turn black due to the small traces of hydrogen 
 sulphide in the air, which may result from sewer gas, 
 coal gas or from cooking vegetables, such as cabbages. 
 Zinc paint cannot be changed black by hydrogen sulphide 
 gas. For this reason zinc paint is always used in chemi- 
 cal laboratories where hydrogen sulphide fumes are com- 
 mon. 
 
 Some oxidizing agents convert lead sulphide into 
 lead sulphate, which is a white compound. 
 
THE CHEMCRAPT BOOK 31 
 
 Experiment 51 — The Oxidation of Lead Sulphide to Lead 
 Sulphate. 
 
 Wet the test paper which was turned dark by hydrogen sul- 
 phide in Experiment 50 with Hydrogen Peroxide (Dioxygen) (not 
 included in outfit). It will turn white again. 
 
 This is the method used to restore old oil paintings which have 
 become darkened by the action of hydrogen sulphide in the air. 
 Many famous paintings have been restored by this method. 
 
 Experiment 52 — Silver Sulphide. 
 
 Sulphur unites directly with most metals to form sulphides. 
 Experiment 1 illustrates the formation of zinc sulphide. 
 
 Place % measure of Sulphur (No. 1) on a bright silver coin and 
 wrap in several thicknesses of paper. After a few days you will 
 find a black spot of silver sulphide on the coin where the sulphur 
 was in contact with it. 
 
 Rubber contains sulphur used in its vulcanization. Wrap a 
 rubber band around a silver coin and you will find it will turn black 
 after a few days due to the formation of silver sulphide. 
 
 A silver coin is turned black in a few hours by a paste of mus- 
 tard and water, as mustard contains sulphur. Eggs also contain 
 sulphur and this is the reason why silver spoons turn black when 
 used for eating eggs. 
 
 Experiment 53 — The Manufacture of Lime Sulphur 
 Solution. 
 
 Put 1 measure of Calcium Oxide (No. 20) and 1 measure of 
 Sulphur (No. 1) in a test tube and fill 1-3 full of water. Boil the 
 mixture for 6 or 7 minutes. A clear yellow liquid will be formed. 
 
 This liquid is commonly known as "Lrime- Sulphur Solution." 
 It has the property of destroying fungi, and is largely used as a 
 spray for fruit trees. 
 
 Pour a drop of the hot solution on a bright silver coin and let 
 it stand for about 15 minutes; a black spot of silver sulphide will 
 be formed. Pour a small quantity of the lime-sulphur solution into 
 a clean test tube and add % measure of Tartaric Acid (No. 14), 
 hydrogen sulphide will be given off and the yellow liquid will be- 
 come colorless. 
 
 SILICON— SILICATES 
 
 The element silicon, in combination with oxygen as 
 silica (quartz, sand, flint), and with the metals and 
 oxygen as metallic silicates (clay, feldspar, mica, etc.), 
 form a large part of the earth's surface. 
 
 The most important artificial silicates are glass and 
 Portland cement. Glass is generally a mixture of sodium 
 
32 
 
 THE CHEMCRAFT BOOK 
 
 and calcium silicates. 
 Water glass (or solu- 
 ble glass) is sodium 
 silicate, which is solu- 
 ble in water. Portland 
 cement is made by 
 strongly heating a 
 mixture of calcium 
 carbonate (limestone) 
 and a siliceous clay. 
 The calcium unites 
 chemically with the 
 silica and alumina of 
 the clay, producing a 
 substance which when 
 
 very finely ground and mixed with water, sets to a solid 
 stone. 
 
 Clay is a combination of silica with oxide of alumi- 
 num and water. It is the combined water which gives 
 it the property of plasticity, and makes it possible to 
 mould it into pottery and bricks. On burning, the com- 
 bined water is driven off and the clay is made perman- 
 ently hard. 
 
 Experiment 54 — Silicon Dioxide. 
 
 Put % inch of Water Glass (No. 19) in a test tube and add 
 water until the tuhe is ^^ full. Shake to mix the liquids. 
 
 In another test tube put 4 measures of Sodium Bisulphate (No. 
 7) and fill the tube 1-3 full of water. Shake until the solid is com- 
 pletely dissolved. 
 
 Pour the liquid in the first tube into the second. A transparent 
 jelly-like precipitate gradually forms and after a tew minutes all 
 the liquid in the tube will have become solid. This is silicic acid. 
 
 Break up this precipitate by means of a stirring rod or piece 
 of wire and empty it into a spoon. Heat the spoon strongly in an 
 alcohol lamp or gas flame for 4 or 5 minutes, or until the precipi- 
 tate is entirely dried and has been reduced to a white solid. This 
 substance is silicon dioxide and is the same thing chemically as 
 pure sand. 
 
 Experiment 55 — Sodium Silicate (Water Glass). 
 
 Paint a thin film of Water Glass (No. 19) on a sheet of paper 
 and let it dry for 15 or 20 minutes. Note the smooth transparent 
 glass-like film which results. 
 
 Pas'e together two sheets of paper or two blocks of wood, using 
 water glass as the adhesive. You will find that it makes an excep- 
 tionally strong paste and it is frequently used for this purpose. 
 
THE CHEMCRAFT BOOK 33 
 
 Silicates of sodium and potassium are tlie only silicates which 
 are readily soluble in water. 
 
 Most metallic silicates are insoluble in water. They 
 are formed as beautiful precipitates when a soluble sili- 
 cate is added to a solution of the metallic salt. 
 Experiment 56 — Strontium Silicate. 
 
 Dissolve 2 measures ot Strontium Nitrate (No. 10) in half a 
 test tube of water and add two or three drops of Water Glass 
 (No. 19). 
 
 A bulky white precipitate will form and upon shaking the test 
 tube the precipitate will fill the whole tube. 
 
 Experiment 57 — Zinc Silicate. 
 
 Place % measure of Powdered Zinc (No. 11) and 2 measures 
 of Sodium Bisulphate (No. 7) in a test tube. Fill the tube half full 
 of water and heat the solution for a few moments to completely 
 dissolve the zinc. Now hold the tube in a glass of cold water for a 
 moment or two until it becomes cool. 
 
 Add to the solution of zinc sulphate thus formed two or three 
 drops of Water Glass (No. 19). A thick precipitate of zinc silicate 
 will be formed. 
 
 Experiment 58 — Aluminum Silicate. 
 
 Place 2 measures of Aluminum Sulphate (No. 12) in a test tube 
 and fill the tube half full of water, shake to completelj' dissolve the 
 solid. Now add two or three drops of Water Glass (No. 19) and 
 note the thick white precipitate of aluminum silicate which is im- 
 mediately formed. 
 
 Experiment 59 — Nickel Silicate. 
 
 Place 2 measures of Nickel Ammonium Suplhate (No. 13) in a 
 test tube and fill the tube half full of water. Heat the solution for- 
 a few moments to completely dissolve the solid, and immerse the 
 tube in cold water to cool it again. 
 
 Add two or three drops of Water Glass (No. 19) to the solution 
 of nickel ammonium sulphate and you will obtain a beautiful green 
 precipitate of nickel silicate. 
 
 Experiment 60 — Ferric and Ferrous Silicates (Iron 
 Silicates). 
 
 (a) Ferrous Silicate. 
 
 Dissolve 2 measures of Ferrous Ammonium Sulphate (No. 17) 
 in a test tube half full of water. To this solution add two or three 
 drops of W(ater Glass (No. 19) and a thick greenish precipitate of 
 ferrous silicate will be formed. 
 
 (b) Ferric Silicate. 
 
 Dissolve 2 measures of Ferric Ammonium Sulphate (No. 21) in 
 a test tube half full of water and add two or three drops of Water 
 Glass (No. 19). A very pretty reddish brown precipitate of ferric 
 silicate will be formed. Compare this ferric silicate with the fer- 
 rous silicate obtained in part (a). 
 
34 THE CHEMCRAPT BOOK 
 
 Experiment 61 — Cobalt Silicate. 
 
 Dissolve 1 measure of Cobalt Chloride (No. 27) in half a test 
 tube of water and add two or three drops of Water Glass (No. 19). 
 
 In this case a beautiful blue precipitate of cobalt silicate is 
 formed. This is one of the prettiest of the entire series of silicates. 
 
 Experiment 62 — Manganese Silicate. 
 
 Place 2 measures of Manganese Sulphate (No. 24) in a test 
 tube half full of water and heat the liquid for a few moments to 
 completely dissolve the solid. 
 
 Now add to this solution two or three drops of Water Glass 
 (No. 19). A pale pink precipitate of manganese silicate will be 
 formed. 
 
 BORON— BORATES 
 
 Boron is found principally in the form of borax (So- 
 dium Pyroborate). 
 
 Large quantities of borax are obtained from certain 
 lakes in foreign countries and also in the western part of 
 the United States. 
 
 Boric Acid may be made by adding acid to a solution 
 of borax. Large quantities of boric acid were formerly 
 used as a preservative for milk, canned meats and vege- 
 tables. It is also used as an antiseptic and most talcum 
 powders contain a certain amount of boric acid. 
 
 Experiment 63 — A Test for Boric Acid. 
 
 Dissolve 2 measures of Boric Acid (No. 2) in a test tube 1-3 
 full of alcohol. Pour a small quantity of the alcohol into the spoon 
 and light it. The alcohol will burn with a bright green flame. This 
 is a characteristic test for Boric Acid. 
 
 Experiment 64 — Borax Glass. 
 
 Mix together on a sheet of paper 1 measure of Sodium Carbon- 
 ate (No. 4) and 1 measure of Boric Acid (No. 2). 
 
 Obtain a small piece (about V2 inch wide by 2 or 3 Inches long) 
 of thin glass. It is very important to have thin glass, as thick glass 
 will break when heated and will also conduct a large amount of 
 heat away from the mixture. A piece of broken test tube is ideal 
 for this experiment. 
 
 Place V2 measure of the mixture of sodium carbonate and boric 
 acid on the piece of glass and heat the glass in an alcohol lamp or 
 gas flame until the mixture melts and forms a clear glass-like film. 
 This is borax glass, and it can hardly be distinguished from the 
 glass on which it is made. 
 
 Many metallic salts have the property of dissolving 
 in melted borax forming various colors, depending on the 
 metal present. 
 
THE CHEMCRAPT BOOK 35 
 
 Experiment 65 — Cobalt Borax Glass. 
 
 Repeat Experiment 64, but just before you heat the mixture 
 of sodium carbonate and boric acid, add to it a small particle of 
 Cobalt Chloride (No. 27). You will And after melting this mixture 
 that the glass film obtained is blue in color. The intenseness of 
 the blue color will depend upon the amount of cobalt which is used. 
 If very much cobalt is used the film will appear to be black, so in- 
 tense is the coloring power, but if only a very slight trace of the 
 cobalt salt is used the film will be a beautiful azure blue. 
 
 Experiment 66 — Iron Borax Glass. 
 
 Iron salts color borax glass yellow. Repeat Experiment 64, 
 adding to the mixture of sodium carbonate and boric acid a very 
 small amount of Ferric Ammonium Sulphate (No. 21). 
 
 Repeat using Ferrous Ammonium Sulphate (No. 17) in place of 
 the ferric ammonium sulphate. 
 
 Experiment 67 — Manganese Borax Glacis. 
 
 Manganese colors borax violet or lilac. Try the experiment, 
 using just a trace of Manganese Sulphate (No. 24). 
 
 Experiment 68 — Nickel Borax Glass. 
 
 Repeat the borax glass experiment, using a trace of Nickel 
 Ammonium Sulphate (No. 13). In this case the borax glass will 
 assume a brown color on being cooled due to the nickel. 
 
 THE FIREWORKS INDUSTRY 
 
 Fireworks depend largely on the use in various ways 
 of colored fire, and the manufacture of colored fire is 
 based on the property possessed by certain metals and 
 their compounds of coloring flame. Copper, zinc and 
 barium color flame green, strontium and lithium color it 
 red, sodium gives a yellow color, and potassium violet. 
 
 •Experiment 69 — The Manufacture of Colored Fire. 
 
 (a)— Red Fire. 
 
 Mix thoroughly on a sheet of paper 1 mea,sure of Strontium 
 Nitrate (No. 10), 2 measures of Potassium Nitrate (No. 8), % mea- 
 sure of Sulphur (No. 1) and 2 measures of powdered Charcoal (No. 
 3). Pour this mixture on a pan, making it into a little pile. Light 
 the pile with a match, or use a short piece of fuse. Keep your face 
 at a little distance. The mass will take fire and burn, giving off a 
 red light due to the presence of strontium. 
 
 (b) — Yellow Fire. 
 
 Repeat, using Instead of strontium nitrate % measure of Sodium 
 Carbonate (No. 4) or V2 measure of ordinary table salt (which is 
 sodium chloride). In this case the light will be yellow owing to the 
 presence of sodium. 
 
36 THE CHEMCRAPT BOOK 
 
 THE INK INDUSTRY 
 
 The manufacture of writing ink dates back to earliest 
 history, and the first inks consisted chiefly of fine soot 
 mixed with a solution of some kind of gum. Today there 
 are many kinds of inks for every conceivable purpose and 
 many formulae are in existence for the manufacture of 
 each kind. 
 Experiment 70 — The Manufacture of Writing Ink. 
 
 Fill a test tube 1-3 full of water and add % measure of Tannic 
 Acid (No. 15). Put an equal amount of water in another test tube 
 and add % measure of Ferric (Iron) Ammonium Sulphate (No. 21). 
 Shake both test tubes to dissolve the solids and then pour the con- 
 tents of the first tube into the second. 
 
 A deep black color will appear, due to very finely divided tan- 
 nate of iron which was formed when the liquids were mixed. 
 
 The manufacture of most of our ordinary writing inks is based 
 ' on this reaction, though many of them contain in addition a certain 
 amount of some aniline dye. Gum is also generally added to thicken 
 the ink slightly and prevent the suspended iron tannate from set- 
 tling out. 
 
 These iron gall inks, as they are called, have the advantage of 
 being permanent, that is, they withstand the action of air and light 
 for many years, and they are very cheap to manufacture. They are, 
 however, very easily erased by the use of certain chemicals and 
 steel pens are more or less corroded by them. 
 
 Experiment 71 — The Manufacture of Blue Ink. 
 
 Dissolve 2 measures of Sodium Ferrocyanide (No. 6) in a teat 
 tube yi full of water. In another test tube Vi full of water dissolve 
 1 measure of Ferric Ammonium Sulphate (No. 21). Pour the second 
 solution into the first. A deep blue liquid will result, due to the 
 formation of Prussian Blue. This is much used as a blue ink. Try 
 writing with it. Prussian Blue is also widely used as a substitute 
 for indigo in laundry blueing. 
 
 Experiment 72 — The Manufacture of Violet Ink. 
 
 Put 2 measures of Logwood (No. 29) in a test tube and fill ^ 
 full of water. Boil for 3 or 4 minutes to extract the color and then 
 add % measure of Aluminum Sulphate (No. 12) to the hot solution. 
 When the aluminum sulphate has dissolved write with the solution, 
 using a clean pen. 
 
 Experiment 73 — The Manufacture of Red Ink. 
 
 Put 2 measures of Logwood (No. 29) in a test tube and fill the 
 tube Vi full of water. Boil for 3 or 4 minutes to extract the color. 
 Then add Vz measure of Aluminum Sulphate (No. 12) and % mea- 
 sure of Sodium Bisulphate (No. 7). When these solids have com- 
 pletely dissolved try writing with the ink, using a clean pen. 
 
 THE PAINT INDUSTRY 
 
 Ordinary paints consist of colors or pigments ground 
 
THE CHEMCRAPT BOOK 37 
 
 up with a "drying oil." By drying oil is meant one which 
 when spread out in a thin layer dries to a solid sheet or 
 film, due to oxidation. Linseed oil is generally used. The 
 pigments used are usually compounds of lead, iron, chro- 
 mium and zinc. 
 Experiment 74 — The Manufacture of Iron Pigments. 
 
 In a test tube 1-3 full ol water dissolve 1 measure of Ferric 
 Ammonium Sulphate (No. 21). In another test tube 1-3 full of 
 ■water dissolve 4 measures of Sodium Carbonate (No. 4). Pour the 
 first solution into the second. The red brown precipitate which is 
 formed is ferric carbonate and hydroxide. This is very similar to 
 the iron compounds used as pigments. 
 
 Experiment 75 — The Manufacture of Lakes. 
 
 Put 1 measure of Logwood (No. 29) in a test tube, fill half full 
 of water and boil for three minutes to extract the color. Add 1 
 measure of Aluminum Sulphate (No. 12) to the colored solution. 
 In another test tube make a solution of 1 measure of Sodium Car- 
 bonate (No. 4) in Vi test tube of water. Add this to the solution 
 of logwood and aluminum sulphate. A deep purple precipitate will 
 form and gradually settle to the bottom of the tube. This belongs 
 to the class of pigments known as lakes. They are very exten- 
 sively used in parting. 
 
 After the pigments have settled from the solutions in which 
 they were precipitated the clear liquid may be poured off and the 
 pigments dried on a sheet of paper if it is desired to save them. 
 
 Experiment 76 — Manufacture of Zinc White. 
 
 Zinc oxide is largely used as a white pigment under the name 
 of "zinc white." This pigment may be prepared by heating one 
 measure of Powdered Zinc (No. 11) in a spoon over a gas or alcohol 
 lamp flame until it catches fire. 
 
 THE SOAP INDUSTRY 
 
 Fats such as lard, butter, and tallow, and also vege- 
 table oils such as olive oil, cotton-seed oil, and linseed oil, 
 are compounds of glycerine with what are known as 
 "fatty acids." If fats and oils are treated with an alkali 
 the glycerine is set free and a compound of the alkali and 
 the fatty acid is formed which is soap. Fine soaps are 
 made from olive oil, cocoanut oil, etc., ordinary white 
 soaps are made largely from cotton-seed oil, while in mak- 
 ing cheap laundry soaps, kitchen grease recovered from 
 garbage, and other impure fats, are used. 
 
 Experiment 77 — The Manufacture of Soap. 
 
 Put 2 measures of Sodium Carbonate (No. 4) and 3 measures 
 of Calcium Oxide (No. 20) into a test tube. Fill 1-3 full of water 
 and boil for two or three minutes. 
 
38 THE CHEMCRAFT BOOK 
 
 Allow it to settle and pour off the clear liquid into another test 
 tube. Add a lump of lard or butter about the size of a pea, and boil 
 the liquid again for a few minutes. 
 
 The fat will first melt, then dissolve in the liquid, forming a 
 soap. Pour out a few drops on your hand and rub it; note the 
 soapy feel. 
 
 The soap can be precipitated from the liquid by adding 2 mea- 
 sures of common table salt and shaking for a few minutes. Let 
 stand and the soap will form a layer at the top. The liquid under- 
 neath contains dissolved in it the glycerine which was in the fat. 
 
 Experiment 78 — Testing for Free Alkali in Soap. 
 
 With a clean knife cut a fresh surface on a piece of dry soap and 
 allow a drop of Phenolphthalein Solution (No. 22) to fall on the 
 exposed surface. If a red color appears where the drop of Phenolph- 
 thalein is in contact with the soap, the soap contains free alkali. 
 
 Try this experiment with laundry and toilet soap. Laundry 
 soap usually contains free alkali. Toilet soap should contain little 
 or no free alkali as it roughens and chaps the skin. This is a very 
 delicate test. 
 
 THE DYEING INDUSTRY 
 
 Textile fibres may be divided into two classes. Vege- 
 table fibres such as cotton and linen consists chiefly of 
 cellulose and are readily attacked by acids. Animal fibres 
 such as wool consist largely of compounds containing nit- 
 rogen. These withstand the action of acids but are 
 readily destroyed by alkalies. 
 
 In the process of dyeing the coloring matter is dis- 
 solved in water (other solvents are not frequently used) , 
 and the material to be dyed is passed through the solu- 
 tion. 
 
 Many dyes unite directly with the fibre of the cloth, 
 forming in some cases colors which are insoluble and will 
 withstand washing, in other cases the colors formed in 
 this manner are not entirely "fast" and will "run" or 
 "bleed" to some extent when the cloth is washed. 
 
 There are also a great variety of coloring matters 
 which are dyed on fabrics by the aid of metallic mor- 
 dants. A mordant is a metallic salt which will combine 
 both with the fibre of the cloth and with the dye-stuif. 
 Salts of aluminum, iron, and tin are generally used. 
 The cloth to be dyed is first passed through a solu- 
 tion of the mordant which unites chemically with the 
 fibre, then through the dye solution, the dye in turn unit- 
 ing with the mordant and forming a "fast" color. 
 
 The same dye-stuflf frequently gives different shades 
 of color when used with various mordants. 
 
THE CHEMCRAPT BOOK 39 
 
 Experiment 79 — Dyeing Fabrics Light Blue. 
 
 Prepare a solution of 4 measures of Sodium Perrocyanide (No. 
 6) in a test tube half full of water. Cut a small piece of absorbent 
 cloth about 1 inch or % inch square and place it in the bottom of a 
 clean tumbler. Now pour the solution of sodium ferrocyanide into 
 the tumbler and saturate the cloth thoroughly with the solution. 
 Remove the cloth and while it is drying, prepare the following solu- 
 tion: 2 measures of Ferrous Ammonium Sulphate (No. 17) in a test 
 tube half full of water. When the cloth has dried place it in the 
 bottom of a clean tumbler and pour this solution over it. Stir it 
 around well so that the solution wets every part of it. Now remove 
 the cloth from this solution and you will find that it is dyed a light 
 blue color due to the precipitate which was formed in the fabric. 
 
 Experiment 80 — Dyeing Fabrics Dark Blue. 
 
 Prepare a solution of 4 measures of Sodium Ferrocyanide (No. 
 6) in a test tube half full of water. Place a small square of cloth 
 in a tumbler and moisten it with this solution as in the perceding 
 experiment. After the cloth is dried moisten it again with a solu- 
 tion of 2 measures of Ferric Ammonium Sulphate (No. 21) in a 
 test tube half full of water. This time the cloth will be dyed dark 
 blue, due to the formation of soluble Prussian blue in the fabric. 
 
 Experiment 81 — Dyeing Fabrics Red. 
 
 Dissolve 2 measures of Sodium Sulphocyanate (No. 26) in a 
 test tube half full of water and moisten a small square of cloth 
 with the solution as in Experiment 79. Now prepare a solution of 
 2 measures of Ferric Ammonium Sulphate (No. 21) in a test tube 
 half full of water, and when the cloth is dry moisten it with this 
 solution. In this case the cloth will be dyed red. 
 
 Experiment 82 — Dyeing Fabrics Black. 
 
 Prepare a solution of 2 measures of Tannic Acid (No. 15) In a 
 test tube half full of water and moisten a small square of cloth with 
 the solution as in the preceding experiment. When the cloth be- 
 comes thoroughly dried moisten it again with a solution of 2 mea- 
 sures of Ferric Ammonium Sulphate (No. 21) in a test tube half 
 full of water. This time the cloth will be dyed black. 
 
 Experiment 83 — Dyeing Fabrics Brown. 
 
 Prepare a solution of 2 measures of Sodium Carbonate (No. 4) 
 in a test tube half full of water and moisten a small square of 
 cloth with the solution as in the preceding experiment. 
 
 W!hen the cloth becomes thoroughly dry moisten it again with 
 a solution of 2 measures of Ferric Ammonium Sulphate (No. 21) 
 in a test tube half full of water. The cloth will be dyed brown. 
 
 Experiment 84 — Dyeing with a Mordant. 
 
 Put 4 measures of Logwood (No. 29) in a glass and pour in 
 one test tube full of hot water. Let the solution stand for half an 
 hour to extract the color. 
 
 Cut a small slip of white cloth about 2 inches square and wet 
 one corner of it with a solution of 2 measures of Aluminum Sul- 
 
40 THE CHEMCRAPT BOOK 
 
 phate (No. 12) in half a test tube of water. Put this where it will 
 dry. 
 
 After the logwood solution has stood for half an hour add 3 
 measures of Sodium Carbonate (No. 4) to it and stir well. Now 
 put the piece of cloth, which must be dry, into this solution and 
 let it soak for about 10 minutes. 
 
 When the cloth has been taken out and dried you will see that 
 it has been dyed two colors, the part which was treated with a solu- 
 tion of aluminum sulphate being darker than the rest of the cloth. 
 
 Formerly most of our dye-stuffs were imported from 
 Germany, and on the outbreak of the European war this 
 source of supply was cut off and for a time there was a 
 great scarcity of dyes in this country. At the present 
 time, however, the United States has a large and flourish- 
 ing dye manufacturing industry. Before the develop- 
 ment of the artificial dye industry coloring matters were 
 used. 
 
 Experiment 85 — Some Naturally Occurring American 
 Dye-stuffs. 
 
 Place a few chips of the bark of the horse-chestnut or buckeye 
 tree in a test tube filled with water to which a small quantity of 
 household ammonia has been added. In a few minutes streamers of 
 blue fluorescent dye will descend from the chips of bark. 
 
 The wood of the Osage Orange tree contains a valuable yellow 
 dye. If you can obtain a few chips of this wood boil them with a 
 little water to extract the color. 
 
 Logwood is taken from the heart of a tropical tree which grows 
 in Central America. The wood is cut into chips and the coloring 
 matter which it contains is extracted with water as in the preceding 
 experiment. This coloring matter forms many different colored 
 dyes when treated with the proper chemicals. It is used frequently 
 in dyeing cloth. 
 
 Experiment 86 — The Effect of Acids and Alkalies on 
 Logwood. 
 
 Put 2 measures of Logwood (No. 29) in a test tube and fill the 
 tube % full of water. Boil for a few minutes to extract the color. 
 In another test tube H full of water dissolve 1 measure of Sodium 
 Bisulphate (No. 7). 
 
 Pour the red logwood solution into the sodium bisulphate solu- 
 tion and a very pretty yellow color results. 
 
 Now add 2 measures of Sodium Carbonate (No. 4). The solu- 
 tion boils violently and gradually changes to a dark purple color. 
 Experiment 87 — Logwood Black. 
 
 Boil 2 measures of Logwood (No. 29) in a test tube % full of 
 water as in the preceding experiment. In another test tube 14 full 
 of water dissolve 1 measure of Ferric Ammonium Sulphate (No. 21). 
 
 Pour the logwood solution into the ferric ammonium sulphate 
 solution and a very intense black color results. 
 
THE CHEMCRAFT BOOK 41 
 
 Experiment 88 — Dark Red Logwood Color. 
 
 Boil 2 measures of Logwood (No. 29) in a test tube % full of 
 water as before. Prepare a solution of 1 measure of Cobalt Chloride 
 (No. 27) in a test tube % full of water and pour the red logwood 
 solution into this. This time a very pretty dark red color is formed. 
 
 ORGANIC CHEMISTRY 
 
 General chemistry was at first divided into two 
 parts, inorganic and organic. Those compounds belong- 
 ing to the mineral kingdom were classed as inorganic sub- 
 stances while those found in plant and animal matter 
 were considered under the head of organic chemistry. 
 
 Every animal and vegetable substance contains car- 
 bon in combination with hydrogen and also in most cases 
 oxygen and nitrogen. It was at one time supposed that 
 the artificial production of these^substances was impos- 
 sible, and that their preparation required the interven- 
 tion of life. In 1828, however, Woehler, a German chem- 
 ist, succeeded in preparing one of these compounds arti- 
 ficially. Since that time a great many organic compounds 
 have been prepared in laboratories by artificial means, 
 and thousands of other organic substances unknown to 
 animal or vegetable life, including many valuable drugs 
 and dyes, have been added to the catalogue of chemical 
 compounds. 
 
 The term organic chemistry is now understood to 
 mean "The Chemistry of the Compounds of Carbon." 
 Several hundred thousand of these compounds are now 
 known to the chemxist. 
 
 A series of organic coloring materials may be pre- 
 pared by heating certain organic substances with sulphur 
 in the presence of an alkali. These colors are chiefly used 
 in dyeing cotton fabrics. 
 
 Experiment 89 — The Manufacture of Sulphur Co!ors. 
 
 In a dry test tube put 1 measure of Tannic Acid (No. 15), 1 
 measure of Sodium Carbonate (No. 4) and 1 measure of Sulphur 
 (No. 1). Shake the tube gently to thoroughly mix the powder and 
 then heat over a flame for three or four minutes or until sulphur 
 vapor is no longer given off. Set the tube aside to cool. 
 
 W^hen the tube is cool, fill it three-quarters full of water, close 
 the mouth with your thumb and shake well. Pour the dark solution 
 obtained into a glass, add fresh water to the tube and shake again 
 to dissolve any remaining dye. Dilute the dye solution with clear 
 water and notice the intense coloring power. 
 
42 THE CHEMCRAFT BOOK 
 
 A great many organic compounds are composed of 
 hydrogen, oxygen and carbon. Some of these compounds 
 may be broken up on heating, into water and carbon. 
 
 Experiment 90 — The Decomposition of Sugar. 
 
 Place 3 or 4 measures of ordinary granulated sugar in a spoon 
 and heat over a flame for a few minutes. The sugar first melts and 
 then turns brown, caramel. W^ter is given off in the form of steam 
 and finally there remains only a black porous mass which consists 
 almost entirely of carbon. Notice that this black residue has none 
 of the properties of sugar. Sugar is a compound of hydrogen, oxy- 
 gen and carbon. Wlien heated the hydrogen and oxygen are driven 
 off in the form of water and the carbon remains. 
 Test the vapor which is driven off with moisture test papers to 
 prove that it is water (see Experiment 23). 
 
 Experiment 91 — The Perparation of Casein. 
 
 Obtain a small quantity of skimmed milk and dilute it with 
 from 3 to 4 parts of water. Now dissolve 4 measures of Sodium 
 Bisulphate (No. 7) in a test tube half full of water and add this 
 solution to some of the skimmed milk contained in another test 
 tube. Shake the milk every time a little of the sodium bisulphate 
 solution is added. 
 
 You will notice that a precipitate is formed in the milk and 
 upon allowing it to stand for awhile the precipitate becomes 
 heavier. It consists principally of casein. When milk sours, lactic 
 acid is formed; this precipitates the casein and the milk is then 
 "curdled." Casein is the principal ingredient of cheese. 
 
 Experiment 92 — The Chemistry of Tanning. 
 
 Dissolve a few drops of the white of an egg in half a test tube 
 of cold water. In another test tube dissolve 1 measure of Tannic 
 Acid (No. 15) in half a test tube of water. 
 
 Add the solution of tannic acid, a few drops at a time, to the 
 solution of the white of egg and notice the precipitate which is 
 formed. 
 
 Skins of animals contain a large amount of albuminous sub- 
 stance, and when they are exposed to a solution containing tannic 
 acid, this substance is changed to a tough, pliable mass. If hides 
 and skins were not tanned they could not be used for the purposes 
 for which leather is used. 
 
 THE CHEMISTRY OF FOODS 
 
 Foods consist chiefly of compounds or mixtures of 
 compounds containing the elements carbon, hydrogen, 
 oxygen and nitrogen. There are three principal classes 
 of foods, carbohydrates, fats and proteids. Carbohy- 
 drates include sugars and starches and are found chiefly 
 in vegetable foods, while fats and proteids are found 
 mainly in animal foods. 
 
THE CHEMCRAFT BOOK 
 
 43 
 
 Starch in foods may be recognized by the chemical 
 test with iodine. 
 
 Experiment 93 — A Test for Starch. 
 
 Put % measure of Ferric Ammonium Sulpliate (No. 21) and 
 % measure of Sodium Bisulphate (No. 7) in a test tube and fill the 
 tube three-quarters full of water; shake well. Add to this solution 
 about 10 drops of Sodium Iodide Solution (No. 23) and shake the 
 tube well. Ferric ammonium sulphate in the presence of an acid 
 liberates iodine from sodium iodide so you now have a solution 
 ccntaining free iodine. Free iodine gives a blue color with starch. 
 
 This starch test solution, directions for making which have just 
 been given, should be put in a small bottle and saved for use in fol- 
 lowing experiments. 
 
 Now take a bit of potato or bread about the size of a pea, boil 
 in a test tube about one-third full of water for a minute or two and 
 let cool. The solution must be perfectly cold, otherwise the test for 
 starch will not work. Now add 2 or 3 drops of the starch test solu- 
 tion. A blue color will be formed, showing the presence of starch. 
 
 Instead of potato or bread a few grains of rice or a little starch 
 may be used in this experiment. 
 
 Proteids are distinguished by containing nitrogen, 
 and by chemical treatment this element can be driven off 
 in the form of ammonia. 
 
 Experiment 94 — Testing for Proteids. 
 
 Place in a test tube a small bit of lean meat or some white of 
 an egg, together with 2 measures of Calcium Oxide (No. 20) and 
 two or three drops of water. Heat gently and test for ammonia by 
 placing In the upper part of the test tube a piece of moistened red 
 litmus paper (see Experiment 42). 
 
 Adulteration of foods was at one time very general 
 and is still sometimes met with, although the pure food 
 laws have largely 
 done away with 
 the more harm- 
 ful forms. The 
 National Govern- 
 ment and the va- 
 rious health 
 boards maintain 
 chemical labora- 
 tories in most of 
 the larger cities 
 for the purpose 
 
44 THE CHEMCRAFT BOOK 
 
 of testing foods, and the following experiments are given 
 as examples of the methods used in this work. 
 
 Experiment 95 — Testing Baking Powder. 
 
 Baking powder consists of sodium bicarbonate mixed with 
 either cream of tartar, alum, or calcium acid phosphate. Starch is 
 frequently added as a harmless though inert filler. 
 
 Put 2 measures of any baking powder in a test tube, fill half 
 full of water and when the liquid has stopped foaming, heat it to 
 boiling. A clear solution shows a pure cream of tatar baking pow- 
 der. Let cool and test for starch by adding a little of the starch 
 test solution as in Experiment 93. 
 
 Experiment 96 — Testing Flour. 
 
 Flour is practically never adulterated in this country, but it 
 is sometimes artificially bleached by a chemical process. Artifi- 
 cially bleached flour may be detected as follows: 
 
 Place 2 heaping teaspoonfuls of flour in a glass, fill half full 
 of gasoline (not included in outfit), stir for several minutes and 
 allow to settle. If the flour is unbleached the gasoline will be dis- 
 tinctly yellow, while if bleached it will remain nearly colorless. 
 
 Experiment 97 — Testing Butter. 
 
 Oleomargarine is an artiflcial butter made from cotton seed oil 
 and other materials. It is not necessarily interior to real butter. 
 Renovated or process butter is prepared from rancid or spoiled but- 
 ter by a chemical process. 
 
 Place a small lump of butter in the spoon and heat over the 
 candle flame. If it is fresh butter, it will boil over, producing a 
 large amount of foam. If it is either oleomargarine or process but- 
 ter it will sputter and crack like a green stick in a flre. 
 
 Fill a tumbler 14 full of sweet milk, set it in a pan of water 
 and heat to boiling. When thoroughly heated add a teaspoonful of 
 the butter to be tested and stir until it is melted. Now remove the 
 tumbler, set it in a pan of cold water (preferably ice water) and 
 continue stirring until the butter solidifies. If the sample Is either 
 fresh butter or renovated butter it will be solidified in a granular 
 condition and distributed through the milk in small particles. If it 
 is oleomargarine it solidifies in one cake and may be lifted from the 
 milk with the stirring rod or spoon. 
 
 Experiment 98 — Testing Canned Goods for Copper. 
 
 This test may be tried on articles such as canned peas, beans, 
 spinach, pickles, etc. Mash a small portion of the sample with a 
 spoon and place a spoonful of the pulp in a teacup with 3 spoonfuls 
 of water and 2 measures of Sodium Bisulphate (No. 7). 
 
 Heat the cup in a saucepan containing boiling water and place 
 the saucepan on the stove. Now drop a bright wire nail into the 
 cup and keep the water in the pan boiling for 20 minutes, stirring 
 the contents of the cup frequently with a splinter of wood. Ex- 
 
THE CHBMCRAPT BOOK 45 
 
 amine the nail and if it appears reddish in color due to a plating of 
 copper having been formed on it the sample which you tested was 
 colored with copper compounds, probably copper sulphate. 
 
 Experiment 99 — The Manufacture of Baking Powder. 
 
 Mix together thoroughly five measures of Tartaric Acid (No. 
 14) and 4 measures of Sodium Bicarbonate (No. 25). Place this 
 mixture in a test tube and fill the tube half full of water; notice 
 that an action takes place and that a gas is given off. This gas is 
 carbon dioxide. 
 
 When baking powder is mixed with dough and moistened, car- 
 bon dioxide is set free and causes the dough to become porous or 
 light. In addition to carbon dioxide other products are formed 
 when baking powder is moistened, depending on the materials used 
 in the baking powder. In the case of calcium monophosphate and 
 baking soda the other products are calcium phosphate and sodium 
 phosphate, both of which materials remain in the food. They are, 
 however, quite harmless. Other acid substances besides calcium 
 monophosphate are frequently mixed with baking soda in the manu- 
 facture of baking powder. Those most commonly used are tartaric 
 acid, potassium acid tartrate and alum. An inert substance such as 
 flour or starch is also sometimes added to baking powder. Thi» 
 substance is added to prevent the reaction from taking place too 
 soon in case the baking powder is exposed to moist air. 
 
 Experiment 100 — A Test for Acid Mouth. 
 
 Cut a small piece of Blue Litmus Paper (No. 18) and place it in 
 your mouth for a moment. If when you remove the paper it is 
 turned red, you have "acid mouth." 
 
 Decayed teeth or an up-set stomach are generally the cause of 
 "acid mouth." Perhaps you have seen advertisements of tooth 
 paste which offers test paper for "acid mouth." These test papers 
 are blue litmus paper. 
 
 TESTING SOILS 
 
 The chemical constituents of soil vary greatly in 
 different localities, depending on the composition of the 
 rock from which the soil was derived. 
 
 All soils contain silicon and aluminum, but in addi- 
 tion to these the elements, nitrogen, phosphorus and po- 
 tassium are essential to plant growth. Most soils con- 
 tain an abundant supply of these elements, but they are 
 frequently combined in such a way as not to be readily 
 absorbed by the plants. These conditions are especially 
 apt to exist in an acid or sour soil. By treating such soil 
 with an alkali, such as lime (calcium oxide or calcium 
 hydroxide) the acidity is neutrahzed and a portion of the 
 unavailable elements necessary to the growth of plants 
 are converted into readily available forms. 
 
46 
 
 THE CHBMCRAFT BOOK 
 
 Experiment 101 — A Test for Acid Soil. 
 
 Obtain a sample of soil and mix with it sufficient clear water to 
 make a thin mortar or paste. Imbed a strip of Blue Litmus Paper 
 (No. 18) in the mixture and allow It to remain for half an hour. 
 Withdraw carefully and rinse in clear water. If the paper has 
 turned pink the soil is acid. 
 
 This test may also be carried out by making a mud ball, press- 
 ing a piece of blue litmus paper against it, and allowing it to stand 
 half an hour. 
 
 Sorrel and moss thrive in acid soils. Clover, alfalfa, peas and 
 beans will not grow, and wheat, corn and most crops do poorly in 
 acid soil. 
 
 PART II 
 
 CHEMICAL MAGIC 
 
 This section contains many new experiments which 
 are especially adapted for exhibition as magic. Certain 
 experiments given in Part I which are of particularly 
 spectacular or mystifying nature, are referred to from 
 4ime to time. 
 
 MAGIC INKS AND PAPERS 
 
 In addition to the new experiments listed under this 
 head, Experiment 9 Fire Ink, and Experiment 24 Sym- 
 pathetic Ink, are especially appropriate. 
 
 Prepare some drawings or writings beforehand, fol- 
 lowing directions given in Experiment 9. Tell your au- 
 dience that you have trained fire to be your servant, and 
 that it will burn out a design or word as you direct. 
 
 There are great possibilities in Experiment 24 for 
 making Chemical Magic. You can draw pictures with 
 the ink prepared in this experiment and it will be per- 
 fectly invisible, but when 
 you hold the blank paper 
 near a stove or over a lamp 
 the drawing or writing sud- 
 denly appears. The eifect is 
 startling. This ink and also 
 a number of those described 
 in the following experi- 
 ments are frequently used 
 by spies in transmitting 
 secret dispatches. We have 
 many instances during the 
 past years where important 
 military secrets have been 
 
THE CHBMCRAPT BOOK 47 
 
 written with some of these inks and have been sent to 
 
 an enemy's country. 
 
 Experiment 102 — Magic Writing. 
 
 Make up three solutions as follows: 
 
 First, 1 measure of Sodium Ferrocyanide (No, 6) in a test tube 
 half full of water. 
 
 Second, 1 measure of Sodium Sulphocyanate (No. 26) in half a 
 test tube of water. 
 
 Third, 1 measure of Tannic Acid (No. 15) in half a test tube 
 of water. 
 
 Using a soft brush, coat a piece of white writing paper with so- 
 lution number 1, a second piece with solution number 2, and a third 
 piece with solution number 3. Be sure to clean your brush well 
 each time you use it for a fresh solution. 
 
 Set the three pieces of treated paper aside to dry and prepare a 
 solution of 2 measures of Ferric Ammonium Sulphate (No. 21) in 
 half a test tube of water. 
 
 Now when the sheets of paper are thoroughly dry, write on each 
 one with the solution of ferric ammonium sulphate, using a clean 
 pen. The same liquid writes a different color on each sheet of paper. 
 
 An interesting variation to this experiment can be worked by 
 painting the three solutions first prepared, in streaks on the same 
 piece of paper. Now when lines are made on the paper with ferric 
 ammonium sulphate solution they will change color every time they 
 are drawn over a new streak. 
 
 Experiment 103 — Magic Inks. 
 
 Set 3 glasses in a row and number them 1, 2 and 3. Put 4 tea- 
 spoonfuls of water in each glass. 
 
 In the first glass dissolve 1 measure of Tannic Acid (No. 15). 
 
 In the second glass dissolve 1 measure of Ferric Ammoinum 
 Sulphate (No. 21). 
 
 In the third glass dissolve 1 measure of Sodium Ferrocyanide 
 (No. 6). 
 
 Number three pieces of writing paper, 1, 2 and 3. Using a clean 
 pen, write on each piece of paper with the solution in the glass of 
 the same number, thus paper number 1, would be written on with 
 the solution in glass number 1. Be sure to wipe your pen carefully 
 each time you use it for a fresh solution. , 
 
 When the writing on the papers has dried wet paper number 1 
 with solution number 2, using a small soft brush or sponge to apply 
 the solution (be sure to wash the brush or sponge thoroughly when 
 changing it from one solution to another) . Wet part of paper num- 
 ber 2 with solution number 1, and part of it with solution number 
 3, wet paper number 3 with solution number 2. 
 
 The many colors in which the writing appears miakes this a 
 very mystifying experiment to ■show to your friends. 
 Experiment 104 — Magic Writing Paper. 
 
 Lay a sheet of ordinary writing pafief on a smooth flat surface, 
 put 1/2 measure of Tannic Acid (No. 15) and % measure of Ferric 
 Ammonium Sulphate (No. 21) on it and mix them together. Now 
 rub this mixture all over the sheet using a small piece of paper to 
 
48 THE CHEMCRAFT BOOK 
 
 rub with. Your hands and also the paper must be perfectly dry, as 
 the slightest trace of moisture will cause black smudges. When 
 the mixture has been rubbed all over the paper shake off the re- 
 maining powder and write on the prepared surface with water. The 
 written characters will be black just as if you had used ink. 
 
 Prepare another sheet of paper in the same way, using % mea- 
 sure of Sodium Ferrocyanide (No. 6) and Vz measure of Ferric 
 Ammonium Sulphate (No. 21). Characters written with water on 
 this sheet are blue. 
 
 Some people will not believe that you can write with plain water, 
 but just fix up some sheets of paper in this way and let them try it. 
 
 MAGIC CHANGES 
 
 Under this section Experiment 12, Bleaching with 
 Sulphur Dioxide (Changing Colored Flowers White) may 
 be used to good advantage. This is a very mysterious 
 trick to those who do not understand the chemistry of it. 
 The colored flowers upon being hung in the glass are 
 changed to white before the eyes of your audience. 
 
 Experiment 105 — Changing Red, White and Blue to Blue. 
 
 Arrange three glasses in a row. In the first put % measure of 
 Sodium Ferrocyanide (No. 6), 3 or 4 drops of Phenolphthalein Solu- 
 tion (No. 22) and Vz measure of Calcium Oxide (No. 20). In the 
 second put Vz measure of Sodium Ferrocyanide (No. 6), 3 measures 
 of Aluminum Sulphate (No. 12) and 3 measures of Strontium Nit- 
 rate (No. 10). In the third put Vz measure of Sodium Ferrocyanide 
 (No. 6) and Vz measure of Ferrous Ammonium Sulphate (No. 17). 
 Fill each of the glasses two-thirds full of water and stir each one. 
 The first glass will contain a red, the second white, and the third 
 a blue liquid. 
 
 In the fourth glass put 2 measures of Ferric Ammonium Sul- 
 phate (No. 21) and 2 measures of Tartaric Acid (No. 14). Fill the 
 glass full of water and stir for a minute. 
 
 Now pour the liquid in the fourth glass into the other three 
 glasses, filling each one. Instead of red, white and blue liquids, 
 three blue solutions re^main. 
 
 Experiment 106 — Changing Water to Wine and Wine to 
 Water. 
 
 (a) — Pouring Water and Wine out of the, same Pitcher. 
 
 Pour a glass of water into a pitcher or similar container and add 
 2 or 3 drops of Phenolphthalein Solution (No. 22). 
 
 In one glass put 1-3 measure of Sodium Carbonate (No. 4) and 
 in another 1 measure of Tartaric Acid (No. 14). If you wish, a few 
 drops of water may be added, thus dissolving the solid so that to 
 anyone watching the experiment the glasses will appear to be only 
 a little wet inside. 
 
 JSTpw pour from your pitcher into the first glass and a rich red! 
 
THE CHBMCRAPT BOOK 49 
 
 liquid will result. Fill the glass about half full. Pour into the 
 second glass and it remains plain water. If you wish you may then 
 pour the contents of the second glass into the first and the red color 
 will disappear. 
 
 (b) Changing Water to Wine and Wine to Water. 
 
 Fill two tumblers half full of water and add to each 1 or 2 drops 
 of Phenolphthalein Solution (No. 22). To the first one add also 
 1-3 measure of Sodium Carbonate (No. i). 
 
 Now one glass contains a red liquid (wine) and the second glass 
 apparently plain water. To the first or red liquid add 1 measure of 
 Tartaric Acid (No, 14) or a little vinegar, and to the second or col- 
 orless liquid add 1-3 measure of Sodium Carbonate (No. 4). Now 
 the colors have become reversed, the red liquid being in the second 
 glass and the colorless liquid in the first. 
 
 To change them hack again add to the first glass 3 measures of 
 Sodium Carbonate (No. 4) and to the second 2 measures of Tartaric 
 Acid (No. 14) or some vinegar. 
 
 Experiment 107 — -Changing Water to Milk. 
 
 Fill 2 glasses each half full of water and dissolve in one 2 mea- 
 sures of Manganese Sulphate (No.24). In another dissolve 2 mea- 
 sures of Sodium Carbonate (No. 4). 
 
 Now pour the contents of one glass into the other and a thick 
 white precipitate will he formed, making it seem as though the 
 glasses were full of milk. 
 
 Experiment 108 — Changing Water to Blood and Blood to 
 Stone. 
 
 Put one Inch of Water Glass (No. 19) in a test tube and add 
 water until the tube is 1-3 full. In another test tube put 2 or 3 drops 
 of Phenolphthalein Solution (No. 22) and fill 1-3 full of water. In 
 another test tube 1-3 full of water put 5 measures of Aluminum 
 Sulphate (No. 12) and shake until dissolved. 
 
 Now hold the tubes in your hand and pour their contents all 
 at once into a clean glass. The three colorless liquids coming to 
 gether immediately form a red blood-like liquid, which in a few 
 minutes will turn into a red, solid mass. 
 
 MAGIC COLORS 
 
 The experiments listed under this head are very 
 pretty as well as mystifying, and lend themselves espe- 
 cially well to exhibition. 
 
 Experiment 109— Pouring Many Colors from the Same 
 
 Vessel. 
 
 Arrange nine dry, clean glasses in a row. In the first glass put 
 1 measure of Ferric Ammonium Sulphate (No. 21) and 1 measure 
 nf Tannic Acid (No. 15). "•- ^ ^ »- 
 
50 THE CHEMCRAFT BOOK 
 
 In the second put 3 measures o£ Strontium Nitrate (No. 10) 
 and 3 measures of Sodium Carbonate (No. 4). 
 
 In the third put 1 measure of Sodium Sulphocyanate (No. 26) 
 and 1 measure of Ferric Ammonium Sulphate (No. 21). 
 
 In the fourth put 3 measures of Cobalt Chloride (No. 27) and 
 2 measures of Sodium Carbonate (No. 4). 
 
 In the fifth put 1 measure of Calcium Oxide (No. 20) and 1 or 
 2 drops of Phenolphthalein Solution (No. 22). 
 
 In the sixth put 3 measures of Sodium Ferrocyanide (No. 6) 
 and 3 measures of Nickel Ammonium Sulphate (No. 13). 
 
 In the seventh put 1 measure of Ferric Ammonium Sulphate 
 (No. 21) and 4 measures of Sodium Carbonate (No. 4). 
 
 In the eighth put 1-3 measure of Sodium Ferrocyanide (No. 6) 
 and 1-3 measure of Ferric Ammonium Sulphate (No. 21). 
 
 In the ninth put 2 measures of Cobalt Chloride (No. 27) and 1 
 measure of Sodium Ferrocyanide (No. 6). 
 
 Now get a large pitcher of water and fill the glasses, stirring 
 each one slightly after you have filled them all. The water will 
 turn a different color as it goes into each glas^. The effect is start- 
 ling as well as beautiful. 
 
 Experiment 110 — Pouring Ink and Milk from the Same 
 
 Vessel. 
 
 In one glass place 1 measure of Tannic Acid (No. 15) and in a 
 second glass place 2 measures of Strontium Nitrate (No. 10). Add 
 about a teaspoonful of water to each glass and stir until the chemi- 
 cals are dissolved. 
 
 Now in a small pitcher or other vessel dissolve 5 measures of 
 Ferric Ammonium Sulphate (No. 21) in about a glass of water. 
 
 When ready to exhibit pour half of this liquid into each of the 
 first two glasses. The liquid in the first one will become intensely 
 black like ink, and that in the second will become milky white. 
 
 Experiment 111 — Pouring Red, White and Blue from the 
 Same Vessel — Patriotic Colors. 
 
 Fill 3 glasses 2-3 full of water. In the firs^' ,1 e 1 measure 
 
 of Sodium Sulphocyanate (No. 26). In the f gsolve 3 mea- 
 
 sures of Strontium Nitrate (No. 10) and irf •'A dissolve % 
 
 measure of Sodium Ferrocyanide (No. 6). ii; - aj, 
 
 In another glass 1-3 full of water dissolve 5'nleasures of Ferric 
 Ammonium Sulphate (No. 21). Pour some of this solution into 
 each of the other 3 glasses and stir. 
 
 The liquid in the first glass will turn red, in the second white, 
 and in the third blue. 
 
 Experiment 112 — Pouring Wine and Water Into the Same 
 
 Glass. 
 
 Put 3 measures of Sodium Bisulphate (No. 7) in a glass full of 
 water and add 2 or 3 drops of Phenolphthalien Solution (No. 22). 
 In another glass put 1 measure of Sodium Carbonate (No. 4) and 
 
THE CHEMCRAFT BOOK 51 
 
 add just enough water to dissolve the solid. 
 
 Now pour from the first glass into the second. At first a red 
 color will result, but as you add more of the solution from. the first 
 glass the red color will mysteriously disappear and apparently only 
 water is in the glass. 
 
 Experiment 113 — Pouring White and Red Into the Same 
 Glass. 
 
 Dissolve 3 measures of Sodium Carbonate (No. 4) in a glass full 
 of water and add 2 or 3 drops of Phenolphthalein Solution (No. 22). 
 In another glass dissolve 2 measures of Sodium Bisulphate (No. 7) 
 in 3 or 4 drops of water. Now pour the red solution in the first glass 
 into the second. At first the red liquid will turn white, but as you 
 add more it will change to red again. 
 
 CHEMICAL SORCERY 
 
 Experiment 114 — Chemical Ice. 
 
 Pour % inch of Water Glass (No. 19) in a test tube and add 
 3 or 4 drops of water. Shake to mix the liquids. 
 
 In another test tube put 4 measures of Sodium Bisulphate (No. 
 7) and fill Vi full of water. Shake until the solid is dissolved. 
 
 Pour the liquid in the first tube into the second. The mixture 
 will gradually freeze into a transparent solid, becoming hard first 
 at the surface and gradually solidifying through the entire mass. 
 In a minute or two the test tube can be inverted as there will be 
 no liquid to spill. 
 
 Experiment 115 — Chemical Soda Water. 
 
 Put 4 measures of Nickel Ammonium Sulphate (No. 13) in a 
 test tube % full of water, and boil for 2 or 3 minutes to dissolve 
 all of the solid. 
 
 Add to the hot solution 1 measure of Sodium Carbonate (No. 4). 
 When the action has stopped add to the solution 2 measures of 
 Sodium Bisulphate (No. 7). 
 
 The soda water is now finished, but it will not do for drinking 
 purposes. 
 
 Exj,- ^hemical Plants. 
 
 Put 1 ' of Water Glass (No. 19) and 4 teaspoonfuls 
 
 of water in a u.^an glass. Stir slightly to thoroughly mix the 
 liquids. Now take 1 measure of Aluminum Sulphate (No. 12), 1 
 measure of Nickel Ammonium Sulphate (No. 13), 1 measure of Fer- 
 rous Ammonium Sulphate (No. 17), 1 measure of Ferric Ammonium 
 Sulphate (No. 21) and 1 measure of Cobalt Chloride (No. 27) antt 
 drop them all into tue water glass solution. 
 
 Watch! In a few minutes trees, grass and all manner of chemi- 
 cal vegetation will begin to sprout and grow. In a short time the 
 liquid will be filled with variously colored chemical plants and 
 trees The thickness of the jungle may be varied by the amount 
 of salts put in. The glass should be set in a place where it will 
 not be shaken. 
 
52 THE CHEMCRAFT BOOK 
 
 Experiment 117 — Chemical Snow. 
 
 Dissolve 2 measures of Strotium Nitrate (No. KU in a test tube 
 nearly full of water. 
 
 In a second test tube put 2 measures of Sodium Carbonate (No. 
 4) and add % inch, of water. Heat until tbe sodium carbonate Is 
 dissolved. 
 
 Carefully pour the contents of the second test tube into the 
 first. A thick white precipitate will form at the top of the tube and 
 as the particles slowly settle to the bottom the effect is very much 
 like a miniature snow storm. 
 
 Sodium carbonate and strontium nitrate react, forming sodium 
 nitrate and strontium carbonate. The latter is not soluble in water 
 and hence separates out of the solution in solid particles. 
 
 Experiment 118 — A Chemical Clock. 
 
 Prepare in several glasses a series of solutions of Sodium 
 Thiosulphate (No. 16) of decreasing strengths; for example, place 
 in the first glass 10 measures of sodium thiosulphate. In the second 
 6 measures, in the third 3 measures, and in the fourth 1 measure. 
 Fill each glass half full of water and stir until the solid is dissolved. 
 
 Prepare a solution of 6 measures of Sodium Bisulphate (No. 7) 
 in a test tube of water, and add an equal portion of this to each 
 glass. A white precipitate of sulphur will appear after a few 
 minutes, but it will form in the different glasses in different lengths 
 of time according to the concentration of the thiosulphate solution. 
 A little experimenting makes it possible to cause the appearance 
 of the precipitate within any specified time. 
 
 CHEMICAL COLORS 
 
 Colors of every shade and variety may be produced 
 by mixing various chemicals. The following experiments 
 give a few examples. 
 
 Experiment 119 — Clots of Color. 
 
 Put a. spoonful of Water Glass (No. 19) in a glass and add two 
 spoonfuls of water. Mix well. 
 
 Fill a test tube half full of water and add 3 measures of Stron- 
 tium Nitrate (No. 10). Shake well. 
 
 Now pour a few drops of the solution in the test tube into the 
 glass containing the water glass. Beautiful white clots of precipi- 
 tate will form. 
 
 Add 1 or 2 drops of Phenolphthalein Solution (No. 22) to the 
 remaining strontium nitrate solution. Now pour a few more drops 
 from the test tube into the glass. This time red clots of precipi- 
 tate will form among the white ones. 
 
 Experiment 120 — A Potpourrie of Colors. 
 
 Put V2 inch of W^ater Glass (No. 19) in a test tube and add 
 water until the tube is 1-3 full. 
 
 In a second test tube make a solution of 2 measures of Cobalt 
 
THE CHEMCRAPT BOOK 53 
 
 Chloride (No. 27) in % inch of water. Heat the solution for a 
 minute to completely dissolve the solid. 
 
 Now pour a very few drops of the water glass solution from 
 test tube number 1 into a third clean test tube and add an equal 
 amount of cobalt chloride solution from test tube number 2. The 
 two liquids together should not equal more than Vz inch in the 
 test tube. A blue precipitate will form. 
 
 You are now through with the cobalt chloride solution con- 
 tained in test tub'e number 2, so that tube may be cleaned and used 
 for making up the next solution. 
 
 A few drops of a solution of a measure of Strontium Nitrate 
 (No. 10) in % inch of water should now be added to the blue pre- 
 cipitate and an equal amount of water glass from the solution in 
 test tube number 1. This will form a white color on top of the 
 blue. 
 
 To make a green color dissolve 1 measure of Nickel Ammonium 
 Sulphate (No. 13) in % inch of water. This solution must be boiled 
 for a few minutes to dissolve the solid. Add a few drops to the 
 color test tube and a few drops of the water glass solution as before. 
 
 To add a brown color make a solution of 1 measure of Ferric 
 Ammonium Sulphate (No. 21) in % inch of water. Heat the solu- 
 tion and add a few drops to the color test tube and a few drops of 
 water glass solution. 
 
 To add a red color dissolve 1 measure of Strontium Nitrate 
 (No. 10) in % inch of water and add 1 or 2 drops of Phenolphtha- 
 lein Solution (No. 22). Add a few drops of this and some water 
 glass solution. 
 
 Your test tube should now be full of a mixture of colors. Blue 
 — white — green — brown and red. This is not an easy experiment 
 to do, but it is very pretty and by following the directions closely 
 and working carefully good results can be obtained. 
 
 Experiment 121 — Green Alcohol. 
 
 Dissolve 2 measures of Boric Acid (No. 2) in a test tube 1-3 
 full of alcohol. Pour a few drops on a large spoon and light it. 
 You will find the flame will be bright green in color. 
 
 Any alcohol lamp or stove can be made to burn with a green 
 flame by adding boric acid to the alcohol used in the proportion 
 of six measures of boric acid to each test tube full of alcohol. 
 
 Experiment 122— A Color Chase. 
 
 Arrange 5 dry glasses in a row. Put in the first Vz measure of 
 Ferric Ammonium Sulphate (No. 21), in the second V2 measure of 
 Sodium Sulphocyanate (No. 26), in the third % measure of Sodium 
 Ferrocyanide (No 6) , in the fourth a spoonful of Water Glass (No. 
 19), and in the fifth 2 or 3 drops of Phenolphthalein Solution (No. 
 
 22) 
 
 ' Pill the first glass with water and stir to dissolve the solid. Now 
 nour the contents of the first glass into the second, the second into 
 the third, etc. Stir well each time a change is made to bring out 
 the color. 
 
54 THE CHEMCRAFT BOOK 
 
 Experiment 123 — Changeable Colors. 
 
 Fill two glasses each half full of water. In the first glass put 
 2 or 3 drops of Phenolphthalein Solution (No. 22). In the second 
 1-3 measure of Ferric Ammonium Sulphate (No. 21), and 1-3 mea- 
 sure of Sodium Ferrocyanlde (No. 6) ; stir the contents of each 
 glass slightly. 
 
 In the third glass put a spoonful of Water Glass (No. 19) and 
 2 spoonfuls of water; stir slightly to mix. 
 
 Now take the first glass containing the colorless liquid in one 
 hand and the second glass containing the blue liquid in the other 
 hand; pour them both at once into the water glass solution. A 
 glass full of bright red liquid will result. 
 
 Experiment 124 — A Fugitive Color. 
 
 Mix a small amount of starch about the size of a pea (or 1 mea- 
 sure of powdered starch), with a few drops of water, pour the mix- 
 ture into a test tube half full of hot water, and boll for a minute. 
 If the solution obtained becomes stiff on cooling add water until it 
 is fairly fluid. 
 
 WJien the solution is perfectly cold add to it a few drops of the 
 starch test solution prepared in Experiment 93. A deep blue coloi 
 will be obtained. Now heat this blue solution to boiling and the 
 color will entirely disappear, leaving a clear solution. On cooling 
 the blue color will again appear. The change may be repeated as 
 often as desired. 
 
 Experiment 125 — A Magic Pitcher of Ink. 
 
 This experiment and the two following are especially good to 
 entertain your friends. 
 
 Obtain a good sized pitcher; a glass pitcher will not do for this 
 experiment, as you need one which is not transparent. Place the 
 pitcher on a tray or a table, fill it with water and arrange five clear, 
 glasses around it. In one glass place 5 measures of Tannic Acid 
 (No. 15). In another 4 measures of Ferric Ammonium Sulphate 
 (No. 21) and in the third 10 measures of Sodium Bisulphate (No. 
 7). The remaining glasses are used only to make the experiment 
 seem more complicated to the audience, and need not be used unless 
 you wish. Add a few drops of water to each glass to dissolve the 
 chemicals. Be sure to remember which glass contains the sodium, 
 bisulphate. 
 
 Now you can show the pitcher to the audience and let thero 
 see that it contains only water. Fill each of the glasses with water 
 from the pitcher and then pour the contents of each glass back into 
 the pitcher except the sodium bisulphate solution. Now you can do 
 some magic talk, etc., over the pitcher, and then pour the contents 
 into the empty glasses. The liquid will be black. 
 
 Now empty all of the glasses into. the pitcher again, this time 
 Including the sodium bisulphate solution, then after you have cast 
 your magic spell over the pitcher, pour the contents into the glasses 
 again and it will be clear water once more. 
 
THE CHEMCRAFT BOOK 55 
 
 MISCELLANEOUS 
 Experiment 126 — Chameleon Paper. 
 
 Hold the Chameleon Paper (No. 28) over a heater, near a stove 
 or in any warm place and notice the color change which takes 
 place. Do not hold the paper over a flame or too close to a very 
 hot surface, as this will harm it. 
 
 Some substances undergo a change when heated and on being 
 cooled return to their original form. In this case the change effects 
 the color of the substance and the paper may be made to change 
 color whenever desired, as long as it is not heated too hot. 
 
 Experiment 127 — Chameleon Liquid. 
 
 Place 1 measure of Cobalt Chloride (No. 27) in a test tube and 
 add 2 drops of water. A pink solution will be formed. Heat the 
 tube gently over a flame and the solution will turn deep blue in 
 color; on cooling the color again changes to pink. 
 
 This change can be repeated as often as you wish, although it 
 may be necessary to add another drop of water occasionally 
 
 Experiment 128 — Rainbow Streamers. 
 
 Fill a large glass pitcher, milk bottle or similar vessel of clear 
 glass with water. Allow it to stand for ten minutes where it will 
 not be shaken so that the water will become perfectly quiet. 
 
 Now drop 1 or 2 measures of Mixed Dyes (No. 30) on the sur- 
 face of the water. Watch closely the beautiful action which follows. 
 
 Experiment 129 — Changing Rainbow Streamers into 
 Moss. 
 
 Dissolve 2 measures of Sodium Carbonate (No. 4) in a glass of 
 water. Allow the glass to stand until the water becomes perfectly 
 quiet and then add 1 or 2 measures of Mixed Dyes (No. 30). Wait 
 until the streamers of color from the dyes have reached the bottom 
 of the glass, then add 2 measures of Aluminum Sulphate (No. 12) 
 without stirring. As the aluminum sulphate dissolves it forms a 
 precipitate with the sodium carbonate. This precipitate absorbs a 
 large amount of the color from the streamers and carries it to the 
 surface of the water. The changing colors and the motion in this 
 experiment make it very beautiful and interesting to watch. 
 
 Experiment 130— The Magic Handkerchief. 
 
 Prepare a solution of 2 measures of Cobalt Chloride (No. 27) 
 in a test tube %, full of water. Now obtain a small handkerchief 
 and put it in the test tube so that it soaks up the cobalt chloride 
 
 solution. , ^ ^ , 
 
 Remove and dry handkerchief on a heater or over a stove, and 
 
 you will find it blue when it is thoroughly dry and warm. Here's 
 
 where you have some fun. u--, -^ , ■,-■, j *i. 
 
 Show the handkerchief to someone while it is blue, and then 
 crush it between your hands and blow through it for a few minutes. 
 It will become colorless. You can repeat this as often as you wish, 
 turning the handkerchief blue by warming it. 
 
56 THE CHEMCRAFT BOOK 
 
 INSTRUCTIONS FOR OBTAINING ADDITIONAL SUPPLIES 
 OF CHEMICALS AND APPARATUS 
 
 Additional supplies of any chemical or extra appara- 
 tus can be obtained by sending direct to The Porter 
 Chemical Co., Hagerstown, Md. 
 
 All prices include postage paid. Refill Chemicals are 
 packed in the same style containers as in the original 
 outfits and the price includes new containers. In ordering 
 refills, state the number of your outfit and the edition of 
 your Chemcraft book. 
 
 Coins sent by mail should be very carefully wrapped 
 and unless letter is registered, are at the sender's risk. 
 Canadian or foreign coins or stamps will not be accepted. 
 The best way to send money is by postal or express 
 money order. 
 
 Please write order on a separate sheet of paper and 
 sign your name and address, in fact, use a separate sheet 
 for letters, questions, experiments, orders, etc. Be sure 
 to sign your name and address on each sheet. 
 
CHEMCRAFT 
 
 LIST OF CHEMICALS— PRICE OF REFILLS 
 Number 
 
 1— Sulphur $ .10 
 
 2— Boric Acid 10 
 
 3 — Powdered Charcoal .10 
 
 4 — Sodium Carbonate 10 
 
 5 — Sodium Bisulphite 10 
 
 6 — Sodium Ferrocyanide • 15 
 
 7 — Sodium Bisulphate 15 
 
 8 — Potassium Nitrate 15 
 
 9 — Ammonium Chloride ...» 10 
 
 10 — Strontium Nitrate 15 
 
 11— Powdered Zinc Metal 10 
 
 12 — Aluminum Sulphate 10 
 
 13 — Nickel Ammonium Sulphate 10 
 
 14 — Tartaric Acid ■ 15 
 
 15— Tannic Acid 10 
 
 16— Sodium Thiosulphate 10 
 
 17— Ferrous Ammonium Sulphate 10 
 
 18— Litmus Paper 10 
 
 19— Sodium Silicate Solution (Water Glass) ■ 15 
 
 20— Calcium Oxide 15 
 
 21— Ferric Ammonium Sulphafe . 10 
 
 22 — ^Phenolphthalein Solution 15 
 
 23— Sodium Iodide Solution 10 
 
 24 — Manganese Sulphate 10 
 
 25 — Sodium Bicarbonate 10 
 
 26 — Sodium Sulphocyanate 10 
 
 27— Cobalt Chloride 10 
 
 28— Chameleon Paper 10 
 
 29-.Logwood 10 
 
 30— Mixed Dyes ■ 10 
 
 31— Sulphide Test Paper • 10 
 
 Stirring Rod 05 
 
 Glass Tube 05 
 
 Gas Delivery Tube and Stopper 10 
 
 Spoon 10 
 
 Measure ■ "^ 
 
 The Chemcraft Book— Outfit Number 2 25 
 
 Test Tubes — 5c each. 
 
 3 for 10c. 30c per dozen. 
 
! ;