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EW YO ,IIU. S. A. I

233

FULTO ISTREET :

I'I ,. Copyright 1918, by Electro IlDportiDg Co., N. Y. Ie-------- -----8

e---~,~_II stI CONTAINING A TREATISE ON ELEMENTARY

I CI AND

I 100II EXPERI EI FOR THE

I PE EI TO BE PERFORMED WiTH

: THE E. I Co. L 80

II THEII ELECTRO -I I P RTINGI 0

PRICE· LIST OF CHEMICALS FURNISHED WITHLABORATORY AND THEIR SYMBOLS

Alum AI2(S04)a, (NH4)2 SO•.... $0.10Antimony (powdered) (Sb)...... .10Anlmonium Aqua (NH,+H20).. .15Ammonium Carbonate (NH4)2 CO•.15Ammonium Chloride (NH4CI) . . . .10Ammonium Sulphate (NH.), S04 .15Barium Chloride (BaCI,)........ .10Boric Acid (HsBOa)............. .10Brimstone (Sulphur) (S)........ .10Calcium Chloride (CaCI,)........ .15Calcium Oxide (CaO)........... .15C'alcium Sulphate (CaSO.2H20). .10Charcoal (Carbon) (C) ...••.••. .10Chloride of Zinc (ZnCI,) ...•.••• .15Copper Sulphate (CuSO.) .....•. .15Ferrous Sulphate (FeSO.)....... .10,Ferrous Sulphide (FeS)......... .15Glycerol (Glycerine) C,H.(OH). .15Hydrochloric Acid (HCI) ..•...• .20Iodine (1) ..••..•.. • . . • . • • . • • . • • .15Iron Chloride (FeCI.) ••..... . . • • .15Iron Oxide (Fe20a)............. .10

Lead Acetate Pb (C,HaO,)•..... $0.10Litmus Paper................... .03Magnesium Carbonate (MgCO.). .10Manganese Dioxide (MnO,)..... .10Mercury (Quicksilver) (Hg) .... .15Nickel Chloride (NiCI2) . . . . . . . . . .15Oxalic Acid (H2C20.) . . . . . . . . . . . .10Sodium Bicarbonate (NaHCO.).. .10Sodium Borate (N'aB02 ) •••••••• .10Sodium Carbonate (Na2CO.) .... .10Sodium Chloride (NaCI)........ .05Sodium Nitra1te (NaNOa) • • • ••••• .10Sodium Phosphate (Na2HP'O.) .. .10Sodium Sulphate (Na2S0.)...... .10Sodium Sulphite (Na2S0.) .10Stannous Chloride (SnCI,) .15Sulphate of Nickel (NiSO.) .. . .. .15Sulphate of Zinc (ZnSO.) • . • . . • • .10Sulphuric Acid (H2SO.) . . . . . . . . . .20Tin (Granulated) (Sn).......... .10Zinc (Metal) (Zn) ......•••....• .10Zinc C-arhonate (ZnCO.). •.....•• .10

PRICE. LIST OF APPARATUS FURNISHEDWITH OUTFIT

One standard washbottle ....•.••.••..•.••...••........................ $0.5.0One conical glass measure •...••.•• •.........•.................... .. .. ..15One Erlenmeyer Flask •..•••.•.••.• •.....•........................ . . . . .30One glass funnel .•..•....•......•.................................... .10One delivery tube ....•..•.....•..•. .10Six assorted test-tubes •...•.••.•..•..••....•... ~ . . . . . . . . . . . . . . . . . . . . . . .35One test-tube holder .............••.................... .30Ten sheets of filter paper. .. . . .. . . .. .05One glass dropper ......•......•..•........•.................. ~ . . . . . . . .10One spoon measure ••.•..••.••....•..................... " . . . . . . . . . . . . . .05One spirit lamp ....•.••.••..••.••.. .15Glass tubing .............•.••..........•...•...... ' '.. ~ . ~ .. . .05Instruction book •..••..•..•....•.••..........•............ ,:. . . . . . . . . . . • .25

All Chemicals have to be sent by express, as the postal authorities don'tallow any acids, etc., to be sent by mail.

When ordering, don't forget to add postage for the goods which can besent by mail. Chemicals will go by express collect.

A discount of 10% will be allowed when ordering six chemicals at thesame time.

The manufacturers regret that they cannot fill orders below SOc.

THE ELECTRO233 FULTON STREET

IMPORTING COMPANYNEW YORK CITY, N. Y.

INSTRUCTION

BOOK

Puh/iJhed hy

THE ELECTRO IMPORTING CO.233 FULTON STREET

NEW YORK CITY, N. Y.

COPYRIGHT BY E. 1. co. 1918

TABLE oj CONTE-NTS

Page

Divisions of Matter 3

Symbols and Atomic Weights for a Num-ber of -the Most CommonElements 5

Chemical Nomenclature - 6, 7, 8

Introduction-Laboratory Operations 9Glass Working 9

First Aid 9

Fire Extinguisher Hand Grenades 9

Experimenter's Aphorisms 10

Weights and Measures-Metric System 10Measures of Weight 10Measures of Volume 11Measures of Capacity 11Measures of Length-Equivalents 11English System 11Measures of Weight (Avoirdupois) 11Troy Weight 11Dry Measure 11Liquid Measure 12Comparison of United States and Metric Systems 12

Per Cent. Solutions 12

Conversion of Measure Expressed in "Parts" 13

One Hundred Chemical Experiments 14 to 29

Formulas for Cleaning Various Substances 29

Poison ~ Antidotes 30

Chemical Substances - Their Technical and Common Names 31-32

INSTRUCTION BOOKCOMPILED BY

SIDNEY GERNSBACK

TREATISE ON ELEMENTARY CHEMISTRY

DIVISIONS OF MATTER

Chemistry embraces three divisions of m,atter-masses, molecules, and atom.A mass is any portion of matter perceptible to the senses.A molecule is the smallest particle of matter into which a body can be divided;

it is the smallest particle that is capable of separate existence.An atom is the still smaller particle produced by the decomposition of a molecule

by chemical means. I t is the unit of matter of the chemist. A molecule is usually acompound of two or more atoms of different elements or perhaps the same element.I t is the uni,t of matter of the physicist.

Elemental molecules are formed of like atoms, compound molecules are formedof unlike atoms. Matter composed of elemental molecules is called simple. or ele­mentary matter; matter composed of compound molecules is called compoundmatter.

Mas is the quantity of matter which a body oontains; VO'lume, the s'Pace itoccupies and Density. its relative quantity of matter under a given volume.

There are also several other properties which belong to all matter, as gravity,inertia, and divisibility.

Chemical attraction, or chemical affinity, is that force which cau~es elementaryatoms or molecules to unite.

Cohesion is that force which binds two or more bodies together. It is thatforce which the particles of a body exert to keep each other together.

Energy is the capacity for performing work; the kinetic energy of a body is theenergy it has in virtue of being in motion; kinetic energy is sometimes called actualenergy; potential energy is energy stored up as that existing in a spring ,or a bentbow, or a body suspended at a given distance above the earth and acted upon bygravity.

Force is that which tends to produce or to destroy motion; if a body is at rest,anything which tends to put it in motion is a force; centrifugal force is that forceby which all bodies m/oving around another body in a curve, tend to fly off from theaxis of their motion; centripetal is that which draws, or im'Pels a body toward somepoint as a center.

Friction is tha't force which acts between two bodies at their surface of contactso as to resist their sliding on each other, and which depends on the force with whichthey are pressed together. .

Gravitation is a force which gives to every particle of matter a ·tendency towardevery other particle.

3

EXPERIMENTS IN CHEMISTRY

Strain is the alteration in shape of a body, as the result of stress.Tenacity is the resistance which a body ,offers to being pulled asunder, and is .

measured by the tensile strength in pounds per square inch of the cross section ofthe body.

Atomic weight is the weight of an atom as compared with hydrogen. Hydrogencom1bines with other elements in the smallest proportion, by weight, of any of theelem,ents. The weight of oxygen entering into a combination is 15.88 tit11es thecorresponding weight of hydrogen; i. e., if the atomic weight of hydrogen is 1, thatof ,oxygen is 15.88, and if the atomic weight of oxygen is 16, that of hydrogen isabout 1.008.

Valence is that property of an element by virtue of which it can hold in com­bination a certain number of other atoms. For example, 2 atolns of hydrogen, H,unite with 1 atom of oxygen, 0, to form 1 molecule of water, H20; 1 atOtTI of hy­drogen, H unites with 1 atom of chlorine, CI, to form 1 tTIolecule of hydrochloric acid,HCl. The valence of an element is the measure of its power to hold other elet11entsin con1bination, and is stated on the basis ,that the valence of hydrogen is 1. Anelement is n10no-, di-, tri, tetra-, etc.-valent according to whether its atoms hold theatoms of other elements in combination in the proportion of one, two, three, four,etc. Hydrogen is monovalent and oxygen bivalent because 1 atom of oxygen holds2 atoms of hydrogen, as represented by the symbol H 20. Son1e elet11ents, for in­stance, copper, have two or n10re different valencies because they unite in differentproportions with certain other elements to form different con1pounds. Thus thereis cuprous chloride, CuCI, and cupric chloride, CUCl2.

Affinity is the attraction that elenlents exert for sonle of the other elelnents. Themeasure of affinity is the anlount of heat or other energy developed during achemical change.

Sublimation is the change of a solid into a condition of vapor without passingthrough the liquid state. Can1phor, ice or snow may be sublin1ated or sublit11ed.

Dissociation n1eans the senaration of a chemical conlDound into its constituentparts, especially if it has bee~ necessary to subject the ~onlpound to a high tem­perature.

Buoyancy of liquids. The upper layer of a liquid not only exerts a pressure onthe lower layers, but it also exerts a pressure in an upward direction. rrhis phenOtlle­non is called the buoyancy of liquids.

Gas is a body in which the molecules are constantly vibrating to and fro and sofar apart that their dimensions may be neglected. The average mon1entum or energyof this n10tion represents the temlperature of the gas, and the force with which theyimpinge on the walls of the vessel in which they are inclosed shows the pressure ofthe gas.

Fluid is a tern1 including both gases and liquids. I t desio-nates a body whosemolecules lllay he displaced by a very slight application of force, this property beingcalled fluidity. I t is possessed in a much greater degree by gases than by liquids.

Difference Between Liquid and Gas. A liquid has no tendency to occupy anymore space, although it yields readily to change of form; a gas, on the other hand,will at once expand and occupy any vessel in which it is put, and as a natural con­sequence, is easily conlpressible.

Combustion is the rapid con1bination of a combustible material with oxygen. Tostart it, it is necessary to elevate its temperature or bring it in contact with a burn­ing body.

If it undergoes conlbustion without ignition it is a case of spontaneous com­bustion, and if it takes place without the appearance of flame or light it is calledslow con1bustion.

Saturated Vapor. A vapor is saturated when it is still in contact with some of itsliquid; vapors in this state are at their greatest density for that temperature. If asaturated vapor be compressed, without change of temperature, a proportionatean1.ount of liquefaction will be produced, but if the temperature be allowed to risecorrespondingly to the work done by compression, the vapor becomes superheated.

Wet or Moist Vapor. A vapor which holds in suspension p·articles of its liquidis called wet or moist vapor.

Difference Between a Gas and Vapor. When a substance first changes from theliquid to the gaseous state, or while the pressure, volume and temperature are nearthose corresponding to such a change, the substance is lTIOre strictly called a vapor,

4

THE ELECTRO IMPORTING CO., N. Y.

or said to be' in the vaporous condition. If the substance is in the gaseous state,but with pressure, volume and temperature C'onditions far removed from those cor­responding to the change of state, the substance is more generally called a gas:There is no sharp line of difference between a vapor and a gas.

Vaporization. A liquid exposed to the atmosphere or a vacuum will give offvapors until the space above the liquid contains vapor of the maximum density for'the temperature.

Vapor. A volatile substance above its critical temperature is called a gas, belowit, a. vapor. Gaseous bodies are generally spoken of as vapors when they are nearthe point of maximum density, and they are often still further distinguished assaturated, superheated and wet vapors.

Mixture of Gases. If br,ought together they will mix thoroughly, and the pres­sure on a vessel containing them will be the sum of the pressure of both.

Specific Heat of Gases. A gas nl.ay be heated while its volume is kept constantand also while its pressure remains constant. In the former case the pressure in·· 'creases and in the latter the volume increases. In the former case the heat added isonly use,d to increase the momentum' of the molecules, while in the latter case anadditional amount'of heat is required to do the work of expanding the gas against thepressure of the atmosph'ere.

Inflammable Bodies are those in which comtbustion starts very easily tby merelyslight contact with a flame.

Explosive Bodies are those in which a large volume of gas is suddenly evolved,and instantaneous combustion takes place throughout the entire mass.

Chemical Combination. When the molecules of one or m,ore elementary bodiesbreak up and form new molecules in a substance whose properties are entirely dif­ferent from the original substances.

How Composition of a Molecule is Shown. By the symbols of its constituents.The number of atoms is expressed by inferior figures at the right of the symtbol, andif we know the atomic weight lof each symlbol we can easily c'lJlculate the, percentageof t:he composition.

How Chemical Elements Are Expre,ssed. By sym'bols taken from the initialletters of their Latin, Greek, or English names.

ATOMICWEIGHT

200.058.714.0416.0

106.531.0

194.839.1579.228.4

107.9323.0587.632.06

127.6204.1232.5119.0184.0239.5

51.265.4

SYMBOLRIgNiNoPdpPtKSeSiAgNaSrSTeT1ThSnWUVZn

ELEMENTMercuryNickelNitrogenOxygenPalladiumPhosphorusPlatinumPotassiumSeleniumSiliconSilverSodiumStrontiumSulphur.TelluriumThalliumThoriumTinTungstenUraniumVanadiumZinc

SYMBOLS AND ATOMIC WEIGHTS FOR A NUMBER OF THE MOSTCOMMON ELEMENTS

ATOMICELEMENT SYMBOL WEIGHTAlum,inum Al 27.1Antimony Sb 120.2Arsenic As 75.0Barium Ba 137.4Bismuth Bi 208.5Boron B 11.0Bromine Br 79.96Cadmium Cd 112.4Calcium Ca 40.1Carbon C 12.0Chlorine CI 35.45Chromium Cr 52.1Cobalt Co 59.0Copper Cu 63.6Fluorine F 19.0Gold Au 197.2Hydrogen H 1.008Iodine I 126.85Iron Fe 55.9Lead Pb 206.9Lithium Li 7.03Magnesium Mg 24.36Manganese Mn 55.0

The names of non-metallic elements in the above table' are printed in black face.The atomic weights given are based on oxygen, 0 = 16.

5

EXPERIMENTS IN CHEM ST Y

CHEMICAL NOMENCLATURE*

The names which have been given to the various elementary forn1 of matterare not ba ed upon any scientific system. The names of some have their origin inmythology. Other have received names which are indicative of SOlne characteristicproperty, while those of ... everal bear reference to some speciar circumstance con­nected with their disc/overy. I t has been the custom in modern times to distinguishmetals from non-metals by applying to the former names ending with the letters um~

and consequently such metals as are 'of Imore recent discovery all ha e names withthis termination. The common metals, however, which have been knO'wni sinceearlier times, such as gold, silver, tin, and copper, keep their old names. The twoelements selenium and tellurium were at the time of their disc/overy thought to bemetals, and they consequently received names with the term1inal urn; these sub­stances strongly resemble ll1etals in many of their physical properties, but in theirchemical relations they are so closely similar to the non-metal sulphur, that theyare by general consent classed among the non-metals; they are examples of thoseelem,ents which are distinguishe·d as metalloids. On this account selenium is by somechemists termed selenion.

In naming chemical compounds, the chemist endeavours that the names em­ployed shall not only serve to identify the substances, but shall as far as possibleindicate their composition. The siimplest chemical compounds are those composedof only tw,o different elements; such as spoken of as binary compounds, and theirnames are made up of the names of the two elements composing them, thus-The compound fOl1med by the chemical union of-

Hydrogen with sulphur is called hydrogen sulphide.Sodium with chlorine is called sodium chl'oride.Copper with oxygen is called copper oxide.Calcium with fluorine is called calcium fluoride.Potassium with iodine is called potassium iodide.

It continually happens, however, that the sa'me two eleme-nts combine togetheri~ m'ore than one proportion, giving rise to as \many different compounds, in whichcase it becomes necessary to so ffi/odify the names that each of the compoundsmay be distinguished. This is accomplished by the use of certain terminal lettersor of certain prefixes; for example, the element phosphorus combines with chlorinein two proportions, fOl1ming two different compounds-in one the molecules con­tain one atom of phosphorus united to three atoms of chlorine, in the other themolecules consist of one atom; of phosphorus associated with five of chlorine.These two compounds may be distinguished in the following ways:-

1 atom of phosphorus with 3 atoms of chlorine forms phosphorous chloride.1 atom of phosphorus with 5 atoms of chlorine f.or/ms phosphoric chloride.

or-1 atom of phosphorus with 3 atoms of chlorine formis phosphorus trichloride.1 atom of phosphorus with 5 atoms of chlorine forms phosphorus pentachloride.The latter method of distinction is the more general, thus-1 a tom of sulphur with 2 atoms of oxygen forms sulphur dioxide.1 atom of sulphur with 3 atomls of oxygen f.orms sulphur trioxide.1 atom of carbon with 1 atoln of oxygen forms carbon monoxide.1 atom of carbon with 2 atoms of oxygen forms carbon dioxide.Occasionally the prefixes sub and proto are employed to denote these differences

of composition, but their use is more limited, and is becoming out of vogue. W/henm,ore than two compounds are forlned by the union of the same two elements, theadditional prefixes hypo, under, and per, over, are sometimes used.

In a considerable number of instances the systematic names of familiar com­pounds give way to the vulgar or common names by which they are known, thus-

Common Names Systematic NamesAmnlonia -. . . .. . . . . . . . .. . .. . .. Hydroa-en nitrideHydrochloric acid Hydrogen chlorideSulphuretted hydr.ogen Hydrogen sulphideWater Hydrogen monoxide

See complete list of the technical and common names of ·chemical sub tancesa t the end of this book.

* Inorganic Chemistry, N ewth.

6

THE ELECTRO IMPORTING CO., N. Y.

Binary compounds consisting of elements united with oxygen are called theoxides of those elements. Certain of these oxides are capable of reacting withwater aiving rise to substances known as acids; such oxides are disting,uished asacid-£~r°ming oxides, or acidic oxides. They are also som,etimes termed anhydrides.All the non-metallic elements, except hydrogen, form oxides of this order, and the

• acids derived from them as known as the oxy-acids or 'hydroxy-acids.

Certain other oxides also unite with water, but give rise to compounds knownas hydroxides. When such ,oxides, which are all derived from the metallic elements,are brought into contact with acids, chemical action takes place, and a c,om'poundtermed a salt is formed, together with water. Such oxides are distinguished as salt­forming or basic oxides. There are also oxides 'iYhich are neither acidic nor basic.Tlh'e names of oxy-acids are derived from the name of the particular oxide from whichthey are formed, thus-

Carbon dioxide gives cartbonic acid.Silicon dioxide gives silicic acid.

When the same element florms two acid-forming oxides, the terminals ic andous are applied to the acids to denote respectively the one "rith the greater and theless proportion of oxygen, thus- '

Sulphur trioxide gives sulphuric acid.Sulphur dioxide aives sulphurous acid.Nitrogen pentoxide gives nitric acid.Nitrogen trioxide gives nitrous acid.

When more than two such acids are known, the additional prefixes hypo or perare nlade use of. Thus persulphuric acid denotes an acid containing the highest quan­tity of oxygen, while hyponitrous acid stands for an ac.id containing less oxygenthan is present in nitrous acid.

There is a class of binary cOlnpounds formed by the comlbination of a largenumber of the elements with sulphur; these are known as sulphides. Certain of thesesulphides are also capa'ble of forming acids which are analogous in their constitutionto oxy-acids, but in which the oxygen atoms are substituted by atoms of sulphur.T'hese acids are known as thio acids (sonletimes sulpho acids), and the same systemof nomenclature is a,dopted to distinguish these: thus we have thio-arsenious acid,thio-arsenic acid, denoting respectively the acid with the smaller and the larger pro­portion of sulphur.

It was at one tim,e believed that all acids contained oxygen, that indeed thiselement was essential to an acid. The name oxygen indicates this belief, the wordsignifying "the acid-producer." This view is now seen to have been inc,orrect, f.ormany acids are known in which oxygen is not one of the constituents. Thus theelements fluorine, chlorine, bromine, and iodine, which constitute the so-calledHalogen group 'Of elements, each combines with hydroa-en, giving rise respectively tohydrofluoric, hyd~ochloric, hydrobromic, and hydriodic acids.

All known acids contain hydrogen as one of their constituents.As already stated, when chemical action takes place between' an acid and a

base, a salt i formled. The word ba~e is unfortunately' employed by different chem­ists in ,different senses, so that it is scarcely possible to give a precise definitionof it. Originally, no doubt, the term was employed simply to denote the idea offoundation, and was applied to the metal or the oxide of the metal entering into thecomposition lof a salt; which being the more tangible constituent was thus regardedas the more important one, or the basis of the salt. At the present day the wor"dbase is use,d in inorganic chemistry chiefly to denote that class of cOln'pounds knownas hydroxides, while the oxides fr'om which these hydroxides are derived are spokenof as basic oxides. Besides this class, it includes ammonia and a few other com­pounds which like ammonia are not derived from metallic oxides. The organicchemist, on the other hand, regards a'nllnonia as the true type of a base; and allorganic conlpounds which can be regarded as "derivatives" of ammonia ate calledbases. ot only so, but the term is even extended so as to include similar "deriva­t~ves" of the phosI?horus, arsenic and antimony analogues of ammonia, thus givingrise to the expressions nitrogen basels, phosphorus bases, etc. Oxy-acids in this waygive rise to oxy-salts, thio-acids to thio-salts, and halogen acids to haloid salts.

The latter salts b~ing binary compounds, their names are given according to thesystem already explained, such, for exa'mple, as calcium fluoride sodium chloridepotassium bromide, silver iodide. "

7

EXPERIMENTS IN CHEMISTRY

In the case of the· oxy-salts and thio-salts, the names are made up from thenames of the acid and of the metal contained in the base, with the addidon of certaindistinctive suffixes: thus if the acid be one whose name carries the terminal OUS,its salts will be distinguished by the suffix ite, w,hile the names of the salts derivedfrom acids whose na'mes end in ic are tern1inated by the letters ate.

Nitrous acid and potassium oxide give potassium nitrite.Su.1phurous acid and potassium oxide give potassium sulphite.,Nitric acid and potassium ,oxide give potassium nitrate.Sulphuric acid and potassium oxide give potassium sulphate.The formation of a salt by the action of an acid up,on a base is due to the

redistribution of the atoms c'omposing the 'molecules of the two compounds, insuch a manner that some or all of the hydrogen atoms in the acid molecules exchangeplaces with certain metallic atoms from the molecules of the base. Acids! which con­tain only one atom of hydrogen 5'0 capable of 'becoming exchanged f.or a metalare termed mono-basic acids; those with two, three, or four such hydrogen atomsare distinguished respectively as di-basic, tri-basic, and tetra-basic acids.

If the whole of the d,isplaceable hydrogen in an acid becomes replaced by thebase, the salt formled is known as a normal salt. On the other hand, when, o'nly aportion of the hydrogen atom\s is displaced by the base, the salt is distinguished asan acid salt. Thus sulphuric acid contains two atoms of hydrogen in its molecule(ass,ociated with one of sulphur and four of oxygen); if hoth the hydrogen atoms areexchanged for potassium, the salt obtained is normal potassium sulphate, and whenonly one is so replaced the sale is knO'wn as acid potassium sulphate. By the termacid salt, therefore, mlUst be understood not a substance having the fatnjiliar prop­erties of an acid, such as a sour taste and the power to redden litmus, but a salt inwhich one or more ,of the hydrogen atoms of the original acid are still left in thel110lect Ie. Son1e chenlists prefer to regard the acids thelllselves as the hydrogensalts; accordingly they apply to nitric acid, sulphuric acid, nitrous acid, sulphurous

. acid, etc., the nanles hydrogen nitrate, hydrogen sulphate, hydrogen nitrite, hydrogensulphite, etc., respectively. I t is quite true that s'ome of the salts of this class dop.ossess acid qualities and will redden litl11US, but this is due to what may beregarded as merely the accidental circumstances of the acidic portion of the 'mole­cule being derived frol11 a strong acid. Many substances belonging to the class ofacid salts are perfectly neutral in their 'behaviour towards litmus, while, on the otherhand, some are strongly alkaline. For exanlple, acid potastsium sulphate is acid to

, test paper, acid calcium carbonate is neutral, while .acid sodium carbonate is alkaline.A third class 'of salts is formed 'by the association of one or more molecules

of normal E?alt, with one or mlore additional molecules of the base: these are knownas basic salts. Thus, carbonic acid and the base lead hydroxide form such a saltknown a's basic lead carbonate.

----I!J~---

8

THE' ELECTRO IMPORTING CO., N. Y.

INTRODUCTION

LABORATORY OPERATIONS

When mea uring liquids, always read fro111 the 1 wer 111eniscus (graduation).If you spill any powder or liquid on the work table, wipe it up as soon as possible.

Do not let it remain on the table for any considerable length of time without wipingit up.

When mixino- Sulphuric Acid, i\LWAYS REMEMBER that the water mustEVER be added to the acid. The correct way to mix this acid is to pour the water

into a vessel, and add the acid, in small quantities, while keeping the liquid in constantmoverp.ent by stirring.

When pouring a liquid into a test tube, extend the arms as far as possible andkeep the middle of the tube on a level with your eyes. ever hold the tlllbe close toyour body, with your face over the tube, while p,ouring in a liquid.

Always do exactly as the experiment tells you. If the experiment calls for 5grams, use 5 grams, otherwise you will not obtain the desired results.

Wash your test tubes and bottles after each experiment. Do not leave them forany length of time, as they will be much harder to clean.

Concentrated Acid means acid of the indicated specific gravity. Hydrochloricacid has a specific gravity of 1 :19; Nitric acid has a specific gravity of 1 :42, and Sul­phuric acid of 1:84. Concentrated Am'monia should have a specific gravity of 0.09.

Diluted Acids (and _ 'mmonium Hydroxide):-Dilute 1 part of Ammonium Hydroxide with 4 parts of Water.Dilute 1 pa~t of Hydrochloric Acid with 4 parts of ater.Dilute 1 part of Sulphuric Acid with 6 parts ,of Water.Dilute 1 part of Nitric Acid with 4 parts of Water.

The Metric system is the general unit of weigh ts and Ineasure in chemistry andall the experiments will call for the Metric weights. Full infonnation about theMetric system will be found on the following pages.

GLASS WORKING

Cutting Glass Plates. Lay the plate of glass on a perfectly smooth surface, andmeasure off the required distance from the edge of the plate. N ow place a ruler on 'the plate in a line with the part to be cut, and with the left hand hold it in place. Takethe glass cutter in the right hand and draw it over the glass (guided by the ruler),using a little pressure, and until you hear a ,distinct scratching noise. N ow pick upthe glass and with the side having the scratch away from you, press gently outwardwith the thumbs and inward with the fingers. This should leave a fairly smooth edge.

Breaking Glass Tubing. Make a sharp scratch on the desired part of the tubewith a triangular file. Make ONE SCRATCIH, do not saw back and forth.

Fire Polishing. After you break a piece of ,glass tubing hold it in the flame of aBunsen Burner until the ends of the glass jus1t begin to soften.

Bending Glass Tubing. Use a Hfish-tail" burner, which gives a broad flat flame.Hold the tube lengthwise in the flame so that the full heat of the burner will becentered on about two inches of the tube. Roll the tube between the fingers, so thatthe heat will be evenly distributed, but do not bend it or a:Uow it to bend, while it is inthe flame. The first indications that the tube is softening will appear when theflame turns to a yellow color. As soon as the heated portion of the tube is softTAKE IT FROM THE FLAME and bend it at the angle which you desire. Do notput it on anything except the asbestos pad while it is hot. i\l1 {bends should have thesame diameter at the bend as at any other part of the tube.

In fitting a glass tube to a rubber stopper, L WAYS run some water in the holeand wet the tube before inserting, otherwise the tube might break and cause seriousresults. A little oommon sense and care are prime requisites to good results.

FIRST AID

Soothing Burns from Acids

Moisten well a rag or sponge with dilute aqua ammonia and apply to the affectedparts. Then grease the parts with olive oil.

9

EXPERIMENTS IN CHEMISTRY

FIRE EXTINGUISHERHAND GREN,ADES

It often happens in a laboratory that some inflammable acid is accidentally spilledor some chemicals which do not agree be mixed. A very 'bad explosion ,or fire isusually the outcome of such mistakes.

A sanitary and safe device can be made by the experimenter at the cost. of afew cen ts which will end chemical fires as quickly as they begin.

I t consists of a mixture of chloride of calcium, twenty parts; sodium chloride(common salt), five parts, and water, eighty-five parts. Several smaJ1 thin bot~les arepurchased, filled with this mixture and corked. .

When a fire occurs. one of these grenades should be thrown in such a way that itwill break in or near the fire which will quickly be extinguished.

EXPERIMENTER'S APHORISMSIn the following, we wish to give. to the Experimenter some hints as to the use

of the different ingredient and how to work then1: .1. Always hear in m,ind that the exact w.orkin,g of a form'ula requires

ACCURACY, CLEA LI ESS, PATlE ,CE AND SKILL. .2. Know whClJt you are about before you start to experiment.3. THE HISTORY OF FAILURES IS THE HISTORY OF SUCCESS

goes an old adage, and it applies well to the experimenter.4. Many tim,es impure, wrong, or deteriorated raw materialls, spe.I1 FAILURE

instead of SUCCESS.5. A great many of the chemicals and ingredients required, cannot be ohtained

from drug stores; 'buy them at a reputable supply house.6. BEFORE CO DEMNI G A FORMULA, be sure the fault does not lie

with the 'manner of handling it, or the purity of the ingredients.7. Be sure to mix the materials comprising a certain formula in the proper

sequence.8. When starting to prepare a mixture especially one containing liquids, ask

yourself: "IS THE SPECIFIC GRAVITY C RRECT, AS INDTCATED BY AHYDROMETER? IS TIHE TEMPERATURE RIGHT? IS THE QUANTITYOR WEIGHT RIGHT?

9. Acids and water, when mixed should be manipulated in the proper manner,i. e., THE ACID SHOULD BE PIOURED I -TO THE WATER, and not vice versa,as the solution is liable to be forcibly ejected from the containing vessel and intothe mixer's face.

10. For any kind of SYSTEMATIC WORK, a floatino- THERMOMETER andHYDROMETER, as weN as measurino- o-lasses and scales, should always be pro­vided as GUESSWORK is EXPENSIVE and SOMETIMES FATAL.

11. Put la,bels ,on ALL bottles, boxes and packages with FULL INSCRIP­TI 0 N as to their canten ts; it will avoid troubles and mistakes.

WEIGHTS AND MEASURESMETRIC SYSTEM

In place of the com'plicated English system of weights and measures, chem.istsnow use the very simple and convenient metric system. This system is based onthe meter, which has a length of a,bout 39.37 in. There are three principal uni,ts: themeter, the liter, and the gram-the units of lenoth, capacity, and weight, respectively.Multiples of these units are obtained by prefixing to he names of the principal unitsthe Greek words deka (10), hekto (100), and kilo (1,000); the subm,u'ltiples, or sub­divisions, are obtained by prefixing the Latin words deci (1/10), centi (1/100), andmilli (1/1,000). These prefixes form the key to the entire system.

In the following tables, the abbreviations of the principle units of these sub­multiples ,begin with a smlall letter, while those of the multiples begin with a capitalletter. Chemists commonly use c.c. for cubic centimeter. The equivalents in thecommon units in use in the United States are o-iven in connection with these tables.

10

THE ELECTRO IMPORTING CO., N. Y.

MEASURES OF WEIGHT

10 milligrams , == centigram (cg)10 ceJ:?tigrams == 1 decigram (dg)10 decigrams == 1 gram (g)10 grams == 1 dekagram (Dg)10 dekagratns == 1 hektogram (Hg)10 hektograms == 1 kilogram (Kg)

1 000 kilograms == 1 ton (T)

1 gram == 15.432 grains Troy or .03527 oz. avoirdupois.1 KNogram == 2.2046 lb. avoirdupois or 2.6792 lb. Troy1 Metric Ton == 1.1023 Ton of 2,000 lbs.

The gram is the weight of 1 cubic centitneter (c.c.) of pure di tilled water at atemperature -of 4° C.; the kilogram is the weight of 1 liter (1.) of water; the metricton is the weight of 1 cubic n1eter (CU.111.) of water at 4° C.

MEASURES OF VOLUME

1,000 cubic mjllimeters ==1,000 cubic centimeters ==1,000 cubic decimeters ==

cubic centi111eter (c.c.)cubic decimleter (cu.dm.)cubic meter (cu.m.)

1 C.c. == .061023 cu. inch1 CU.111. == 35.314 cu. ft. or 1.3079 cu. yd.

MEASURES OF CAPACITY

10 tnilliliters == centiliter (cl)10 centiliters == deciliter (dl)10 deciliter . . . . . . . . . . . . . . . . liter (1)10 liters : == dekaliter (DI)10 dekaliters == hektoliter (HI)10 hektoliters == 1 kiloliter (KI)

1 liter == 61.023 cu. in. or 1.0567 liquid qt.- or .9078 dry qt.The liter i equal in volu111e to 1 cu. dm.

EQUIVALENTSMEASURES OF LENGTH

Metric U. S. Measuremetre 39.3704 inchesdecimetre 3.9370 inchescentimetre 0.3937 inchesmillimetre 0.0393 inches

U. S. Metricyard (3 feet or 36 inches) 0.9143 metresfoot (12 inches) . 30.40 centin1etres

ENGLISH SYSTEM

One United States gallon has a volume of 231 cu. in., and contains 4 qt., or 8 pt.The English Imperial gallon contains 277.46 cu. in., hence the English gaUon isequivalent to 1.20032 U. S. gal.

A gallon of pure water at 62° F. weighs 133.37 oz. Or 58,350 gr.; hence, 1 pt. ofpure water at 62° F. weighs 16% oz., or a little over 1 lb. The measure termed afluid ounce is a measure of volume, and not of weight, and is equal to 1/16 part ofa pint or approximately the volume of 1 oz. of pure water.

11

EXPERIMENTS IN CHEMISTRY

FIRE EXTINGUISHERHAND GREN,ADES

It often happens in a laboratory that some inflammable acid is accidentally spilledor some chemicals which do no't agree be mixed. A very 'bad explosion lor fire isusually the ou tcome of such mistakes.

A sanitary and safe device can be made by the experimenter at the cost. of afew cents which will end chemical fires as quickly as they begin.

It consists of a mixture of chloride of calcium, twenty parts; sodium chloride(common salt), five parts, and water, eighty-five parts. Several smaU thin bottles arepurchased, filled with this mixture and corked. .

When a fire occurs. one of these grenades should be thrown in such a way that itwill .break in or near the fire which will quir.kly be extinguished.

EXPERIMENTER'S APHORISMSIn the following, we wish to g·ive. to the Experin1enter some hints as to the use

of the different ingredients and how to work them:1. Always hear in m.ind that th e exar.t w,orkin.g of a formula requires

ACCURACY, CLEA LI ESS, PATIE ICE AND SKILL. .2. Know whaJt you are about before you start to experiment.3. THE HISTORY OF FAILURES IS THE HISTORY OF SUCCESS

goes an old adage, and it applies well to the experimenter.4. Many timles impure, wrong, or deteriorated raw materia/Is, spell FAILURE

instead of SUCCESS.5. A great many of the chemicals and ingredients required, cannot be ohtained

from drug stores; 'buy them at a reputable supply house.6. BEFORE CONDEMNING A FORMULA, be sure the fault does not lie

with the 'manner of handling it, or the purity of the ingredients.7. Be sure to mix the materials comprising a certain formula in the proper

sequence.8. When starting to prepare a mixture especially one containing liquids, ask

yourself: HIS THE SPECIFIC GRAVITY C RRECT, AS INDJ.CATED BY AHYDROMETER? IS T'HE TEMPERATURE RIGHT? IS THE QUANTITYOR WEIGHT RIGHT?

9. Acids and water, when mixed should be manipula'ted in the proper manner,i. e., THE ACID SHOULD BE PIOURED INTO THE WATER, and not vice versa,as the solution is liable to be forcibly ejected from the containing vessel and intothe mixer's face.

10. For any kind of SYSTEMATIC WORK, a floating THERMOMETER andHYDROMETER, as weIll as measuring glasses and scales, should always be pro­vided as GUESSWORK is EXPENSIVE and SOMETIMES FATAL.

11. Put IClJbels ·on ALL bottles, boxes and packages with FULL INSCRIP­.TI 0 N as to their contents; it will avoid troubles and mistakes.

WEIGHTS AND MEASURESMETRIC SYSTEM

In place of the complicated English system of weights and measures, chem.istsnow use the very simple and convenient metric system. This system is based onthe meter, which has a length of a'bout 39.37 in. There are three principal units: themeter, the liter, and the gr.am-the units of length, capacity, and weight,' respectively.Multiples of these units are obtained by prefixing to t:he names of the principal unitsthe Greek w,ords deka (10), hekto (100), and kilo (1,000); the suhmu!ltiples, or sub­divisions, are obtained by prefixing the Latin words deci (1/10), centi (1/100), andmilli (1/1,000). These prefixes form the key to the entire system.

In the following tables, the abbreviations of the principle units of these sub­multi'ples ,begin with a sm,all letter, whiile those of the multiples begin wit1h a capitalletter. Chemists commonly use C.c. for cubic centimeter. The equivalents in thecom'mon units in use in the United States are given in connection with these tables.

10

THE ELECTRO IMPORTING CO., N. Y.

MEASURES OF WEIGHT

10 n1.illigrams J == 1 centigram (cg)10 cef?tigrams == 1 decigram Cdg)10 decigrams == 1 gram (g)10 grams == 1 dekagram (Dg)10 dekagrams == 1 hektogram (Hg)10 hektograms == 1 kilogram (Kg)

1 GOO kilograms == 1 ton (T)

1 gram == 15.432 grains Troy or .03527 oz. avoirdupois.1 KNogram == 2.2046 lIb. avoirdupois or 2.6792 lb. Troy1 Metric Ton == 1.1023 Ton of 2,000 lbs.

The gram is the weight of 1 cubic centirneter (c.c.) of pure di tilled water at atemperature ,of 4° C.; the kilogram is the weight of 1 liter (1.) of water; the metricton is the weight of 1 cubic n1eter (cu.nl.) of water at 4° C.

MEASURES OF VOLUME

1,000 cubic mlillimeters ==1,000 cubic centimeters ==1,000 cubic decimeters ==

cubic centimeter (c.c.)cubic decimleter (cu.dm.)cubic meter (cu.m.)

1 C.c. == .061023 cu. inch1 CU.ill. == 35.314 cu. ft. or 1.3079 cu. yd.

MEASURES OF CAPACITY

lOInilliIi te r s '. . . == cen til it er (cI)10 centiliters == deciliter (dl)10 deciliters == liter (1)10 liters == dekaliter (DI)10 dekaliters == hektoliter (HI)10 hektoliters == 1 kiloliter (KI)

1 liter == 61.023 cu. in. or 1.0567 liquid qt., or .9078 dry qt.The liter i equal in volun1e to 1 cu. dm.

EQUIVALENTSMEASURES OF LENGTH

Metric U. S. Measuremetre 39.3704 inchesdecimetre 3.9370 inchescentimetre 0.3937 inchesmillimetre 0.0393 inches

U. S. Metricyard (3 feet or 36 inches) 0.9143 metresfoot (12 inches) . 30.40 centin1etres

ENGLISH SYSTEM

One United States gallon has a volume of 231 cu. in., and contains 4 qt., or 8 pteThe English Imperial gallon contains 277.46 cu. in., hence the English gaB'on isequivalent to 1.20032 U. S. gal.

A gallon of pure water at 62° F. weighs 133.37 oz. Or 58,350 gr.; hence, 1 pt. ofpure Wiater at 62° F. weighs 16% oz., or a little over 1 lb. The measure termed afluid ounce is a measure of volume, and not of weight, and is equal -to 1/16 part ofa pint or approximately the volume of 1 oz. of pure water.

11

EXPERIMENTS IN. CHEMISTRY

One fluid ounce is equivalent to 29.57 C.c. and contains 455.86 gr. of water at62° F. One gram is equivalent to 15.43 gr., and 1 oz. avoirdup-ois is equivalent to28.34 gr.

The unit of dry measure is the bushel which contains 2,150.4 cu. in.

The avoirdupois pound contains 7,000 gr.

MEASURES OF WEIGHT (AVOIRDUPOIS)

437.5 grains (gr.) == 1 ounce (oz.)16 ounces == 1 pound (lb.)

100 pounds == 1 hundredweight (cwt.)20 cwt., or 2,000 lb == 1 ton (T)

T. cwt. lb. oz. gr.== 20 or 2,000 or 32,000 or 14,000,000

TROY WEIGHT

24 grains (gr.) 1 pennyweight (pwt.)20 pennyweights == 1 ounce (oz.)12 ounces == 1 pound (lb.)

1 1b. == lL, uL.. or L40 pwt. or 5.760 gr.

DRY MEASURE

2 pints (pt.) 1 quart (qt.)8 quarts == 1 peck (pk.)4 pecks == 1 bushel (bu.)

1 bu. == 4 pk. or 32 qt. or 64 p·t.

LIQUID MEASURE

4 gills 1 pint (pt.)2 pints == 1 quart (qt.)4 quarts == 1 gallon (gal.)

31.5 gallons == 1 barrel (bbI.)2 barrels, o.r 63 gallons == 1 hogshead (hhd.)

hhd. bbl. gal. qt. pt. gills1 == 2 or 0.3 or 252 or 504 or 2,016

1 cubic foot of water at its maximum density 4° C., weighs 62.425 lb. and 1 gal.weighs 8.345 lb.

LONG-TON TABLE16 ounces '== 1 pound (lb.)

112 pounds == 1 hundredweight (cwt.)20 cwt., or 2,240 Ibs == 1 ton (L.T.)

COMPARISON OF UNITED STATES AND METRIC SYSTEMS

1 C.c. X .0338 == 1 fluid oz.1 c.C. X .608 == 1 cu. in.1 cU.m. X 35.315 == 1 cu. ft.t g. X .0353 == 1 oz.1 gal. X 3.785 == 1 liter1 gr. (Troy) X .0648 == 1 gram1 kg. X 2.2046 == 1 lb.1 pk. X 9.08 == 1 liter

1 liter X 1.0567 == 1 qt. (liquid)1 liter X .264 == 1 gal.1 liter X .908 == 1 qt. (dry)1 liter X .0353 == 1 cu. in.1 m. X 39.37 == 1 inch1 oz. (Troy) X 31.104 == 1 gram1 oz. (avoirdupois) X 28.35 == 1 gram1 qt. (liquid) X .946 == 1 liter

12

Grams,or c.C.

12345

10205060

100250­500-

1,000'2,500'5000-

10;OQOt

THE ELECTRO IMPORTING CO., N. Y.

PER CENT. SOLUTIONS

A table glVl~g the weight in grains (avoirdupois) of any chemical substancerequired to make a per cent. solution from 1 per cent. to 50 1?er ce~t. based on t~eweight 'Of one gallon of water at 40° F. == 8.33888 llbs. (avOIrdupoIs) or one flUIdounce of water weighing 456.03 grains (avoirdupois).

For each fluid ounce of water takeFor a 1 per cent. solution.................... 4.66 Grains

2"" I' 9.38 "3 " 14.104 u .•..•••••.•......... 19.005 " 24.006 " 29.107 u 34.308 " 39.609 " 45.09

10 I' .••••••••.••.•.•.••• 50.6715 " 80.4820 " 114.0025 u 152.0030 " 195.4435 " 245.5640 " 304.0245 " 373.1050 " " 456.03

It should be noted that the above table applies to 'water; percentage solutions f.orother liquids would necessarily have to be figured on the weight of the particularliquid.

Percentage solutions are also sometimes made up from a saturated base.This method is incorrect unless it is so designated in giving the formula, that is, bystating in the formula saturated solution base. ~uch percentages are made byplacing in the liquid used, more of the chemical than the liquid will carry in solution;this resulting solution is filtered to remove the excess chemical and then used as abase. For example, to make a 10 per cent. solution, 10 per cent. of the base is usedand 90 per cent. of the pure liquid or in other words, 1 ounce of the saturated solu­tion to 9 ounces of the liquid.

CONVERSION OF MEASURE EXPRESSED IN "PARTS"Sometimes a formula in an experiment is expressed in "parts"; for example, a

formula may read: Use 1 'Part of nitric acid, 2 parts of potassium bichromate and 5parts 'of water. All that is necessary would be to designate the exact quantity thatthe part represents; then, if one grain for solids and one minim for liquids shouldbe used, the above formula would work out as follows: Nitric acid, 1 minim; potas­sium bichromate, 2 grains, and water,S minims. Of course, this can be multipliedto any p1"oportion.

F,or further reference the following table will also be found very useful:No. of ~ . .parts Grains Minims

1 1 12 2 23 3 34 4 455510 10 1020 1 scr. 2050 50 5060 1 ,dr. 1 dr.

100 dr. 2 scr. 1 dr. 40 min.250 112 oz. 32 grs. 3112 dr. 40 min.500 1 oz. 62 grs. lh oz. 10 min.

1,000 214 ,oz. 16 grs. 2 oz. 40 min.2,500 5lh ,oz. 94 grs. 5 oz. 1 dr. 40 min.5,000 11~ oz. 79 grs. 10 oz. 3 dr. 20 min.

10,000 1 lb. 6%: oz. 49 grs. 20 oz. 6 dr. 40 m.in.

13

EXPERIMENTS IN CHEMISTRY

ONE HUNDRED CHEMICAL EXPERIMENTS

The experiments contained in this book were arranged with one idea in mind,namely, that of enabling one to learn more, while seemingly at play. Chemistry andits allied arts are of the greatest use in every industry of today. To be conversant inchemistry is to thoroughly understand the whys and wherefores of Nature's won­derful series ,of chemical reactions shown in plants, minerals, animals and humanbeings. All of these can be classed as large complex chemical engines. Chemistryis a very spectacular and interesting science and many chemical phenomena are moststartling and mystifying to the layman. Chemistry is very often looked upon as adangerous profession. But this is. far from being the case. Contrary to an oldbelief, a chemical experiment does not neces,saliily result in an explosion. All thatis necessary is a small amount of precaution and cleanliness of all apparatus usedin the various experiments. C'hemistry also plays an important part in the changesthrough which the earth, the air and the water continually pa,ss. Now that we haveallowed our minds to dwell upon the proper aspect of chemistry, we will start toperform the experiments as they fo11o\\r in consecutive order and gain a fundamentaland basic knowledge of all things chemical.

EXPERIMENT NO.1

A Test for AcidsThe easiest test for acidity is accomplished ,by using the tblue Litmus Paper and

-placing it one-half way into the solution to be te,sted. The presence of acid isshown by the Litmus Paper turning red.

EXPERIMENT NO.2

A Test for AlkaliesProceed the same as in Experiment No.1 with the exception that for this test,

we use the red Litmus Paper, and if it turns blue, the solution can be 'Pronounced asbeing alkali.

EXPERIMENT NO.3

To Test for the Presence of LimePlace one-half measure of Sodium Carbonate (Na2COa) in the large test tube

one-half full of water. Shake ,this mixture well until it is thoroughly dis,solved. Allowthe solution to stand. After a few minutes if it shows a 'white turpidity, there isa considerable amount of lime contained in the water.

EXPERIMENT NO.4

Showing How Steel May Be Easily MeltedProcure a small steel rod and ,heat 'it until i,t becomes a cherry red, and touch it.

with some Brimstone (Sulphur) (S). You will discover that it im'mediately meltsas though it 'were wax.

EXPERIMENT NO.5

Liquids Which Do Not MixUse a small test tube, wherein place a small quantity of Mercury (Mg), then a

small amount of Alcohol, and finally add Kerosene. A dis,tinct line will be noticeablebetween each of the l,iquids. They do not comlbine with eac·h other.

EXPERIMENT NO. 6

To Show the Necessity of the Presence of Oxygen to Produce CombustionApparatus. A small dish pan, a candle, a match and a clear glass milk bottle.Directions. Light the ,match and hold underneath the 'bottom of the candle,

heating same slightly and when wax softens, place candle in the absolute center ofdish pan. Hold it there for a few seconds un til the wax at base of candle harcfens

14

THE ELECTRO IMPORTING CO., N. Y.

and holds it in place. FiU the basin slowly Wlith water to a height of two inches,measuring by the candle. Hold the milk bottle in your left hand and light ,the candle

. with your right. C'over the lighted candle very quickly, being careful not to createa breeze that will blow it out. If you have been successful lin .placing the bottle overthe lit candle without extinguishing it, you will find that in a very short while theflame will gradually ,become dim, and finally go out entirely.

Observation. The flame,after having consumed all ofthe Oxygen in the invertedbottle. went out. It will alsobe not-ed that the water levelon the inside of the bottleis higher than the level of thewater in the basin.

Conclusion. The waterrose higher in the milk bot­tle due to the vacuum thatwas created when the Oxy­gen (0) was consumed. Car­bon Dioxide was formed bythe combustion and dissolvedin the water. The flamedied out due to lack of Oxy­gen. Oxygen must bepresent to have a proper andthorough combustion.

Note. Carbon Dioxideis soluble in about one-halfits volume in water.

EXPERIMENT NO.7

Production of Oxygen by ElectrolysisApparatus. Electric batteries of not less than three volt output, a ba·sin of wate~,

two test tubes, two pieces bare copper wire and Sulphuric Acid (H2S04). l

Directions. Connect battery as shown in diagram, fill test tubes with acidulate~

water, and invert with the free ends of copper wire within the tubes, placing themin the basin of water containing a 20% solution of Sulphuric Acid (i.e., twenty partsof Sulphuric Aoid (H2S04) to each one hundred parts of water). Close the circuitand allow the current to travel through the electrodes in the two tubes.

Observation. I t will be noted that the test tube containing the positive electrodeexpels one-half as much water in a given time as the negative electrode in test tubeNo.2. The positive pole or the one with the least water expelled contains Oxygen (0).

EXPERIMENT NO. 8

Production of Hydrogen by ElectrolysisFollowing the same di­

rections as in the precedingexperiment, No.7, take thetest tube that has the greateramount of air expelled andcontaining the negative elec­trode, and you will find thatthis contains Hydrogen (H)Gas. When taking thesetubes out of the water, leavethem inverted; that is, withmouth downward so as tominiulize the chance of thegases escaping. Take the

8t7.5liloradClt//aleti 11'(1ler ~~~e (cf~c~ndo~~~k i\h~~l?;piece of white chalk· that has.

15

EXPER MENTS IN CHEMISTRY

been moistened, "No.1," likewise mark the tube containing Hydrogen (H) "No.2."Still holding the test tubes inverted, light a match and allow the flame to burn fora while. Blowout the flame and plunge the glowing ember into the Oxygen (No. 1)tube. It will again burst into flame. Take tube No.2 (containing the Hydrogen),hold- a 'match to its mouth, and you will immediately have an explosion.

Conclusion for Experiments Nos. 7 and S. There are two parts of Hydrogen~enerated to everyone part of Oxygen, which is the formula of water (H20). Waterqan be disassociated by the action of electricity into its two component parts.i1 Observation. Hydrogen (H) is a violent explosive. Oxygen (0), is a sustainer~f combustion. Sulphuric Acid (H2S04) is placed in the water in order to make it~n electrolyte, thereby creating a better conductor of electricity than if water alonewere used.

EXPERIMENT NO.9

Making Hydrogen Chemically

Apparatus: One Ibottle, zinc filing, basin, glass t-ube, test ·tube, funnel or thistletube, cork and Sulphuric Acid (H2S04).

Pour st/lplJur/c .Clc/d here ....

/)e!lY~r!l

It/be

I.

Woterftlled lest

tube ....

I/ydroge/JgQScomes otllbere:

~~~=~3~

./ !Yo!er

zinc"pieces

Directions: Place a smallquantity of zinc in a pintmilk bottle and cover thezinc 'iVith water. Arrangeapparatus as in diagram.Add sufficient Sulphuric Acid(H2S04) to cause bubbles toform on zinc. Collect theHydrogen Gas (H) fromtube under water as shownin sketch.

Conclusion: Hydrogenis an invisible, inodorous andtasteless gas.

.J

EXPERIMENT NO. 10

Proving Some Other Properties of Hydrogen

Apparatus: A small rubber toy balloon, a sufficient quantity of Hydrogen Gas(H) to fill it; generate the gas as in Experiment No.9.

Directions: Inflate the toy balloon with the 'Hydrogen Gas.

Observation: A tendency for the balloon to rise is noted, and it will float in air.

Conclusion: Hydrogen is the lightest gas known. It lis lighter than the air,'herefore, it made the balloon rise.

16

THE ELECTRO IMPORTING CO., N. Y.

EXPERIMENT NO. 11

The Production of Chlorine Gas

Apparatus: Two meas­ures of Manganese Dioxide(Mn02), a small test tubethree-fourths filled with Hy­drochloric Acid (H Cl), glasstube, 2 connections.

Directions: Shake con­ten ts. Connect glass de­livery tube from the smalltest tube to a larger tubecontaining one ounce ofwater as shown in diagram.Heat the tube over an alco­hol flame very gently.

Observation: Bubblesare noted going into the largetube. These bubbles areChlorine Gas for!ming withthe water to make a satura tedsolution of C'hloric Gas.

EXPERIMENT NO. 12

Hydrochloric Acid

Apparatus: Two testtubes (one containing Chlor­ine Gas, the other HydrogenGas), a spirit lamp or openflame.

Directions: CombineHydrogen Gas and ChlorineGas by placing the mouths ofboth test tubes together(see diagram), the mouthsbeing kept together by en­circling with the fingers.Allow the gases to mix. Themouths of the tubes are thenquickly brought, in succes­sion, over an open flame.

Conclusion: A slight ex­plosion occurs and fumes ofa compound of HydrochloricAcid are formed with themoisture of the air.

17

.....C/J/orj,ne 90S

Ll7cir c/e mou!1;)-----~ of!Jot!? lubes )fif!J ..;~~~.:;;"'h.h.;.:~fingers

~.../ hydrogen gas

EXPERIMENTS IN CHEMISTRY

EXPERIMENT NO. 13Spontaneous Combustion

A piece of paper moistened with Aqua Ammonia ancL placed into a test tube-containing Chlorine Gals, will ignite spontaneously (without the add of an openflame).

EXPERIMENT NO. 14Another Spontaneous Ignition

In a spoon, melt a small quantity -of Sulphur (S) and while it is in the liquidstate, put a spoon in the tube containing Chlorine Gas. It will burn rapidly.

EXPERIMENT NO. 15Generating Chlorine Smoke

Take a sheet of filter paper and soak in com,mon Turpentine, then fold. \\Thenthis is put in the test tube containing Chlorine Gas, it will burn ilmmediately, pro­ducing much smoke. This is another form of spontaneous combustion.

EXPERIMENT NO. 16Chloride of Mercury

Wit'h the Chlorine Gas as made in Experiment No. 11, fill a test tube. Now heat adrop of Mercury (Mg) in the measure and when it is hot, pour it into the ChlorineGas. I t will burn with a reddish flame, producing Chlonide of Mercury (HgCI2)'Thi s chemical is poisonous.

EXPERIMENT NO. 17Bleaching Cloth

Put some differently colored cloths in ,SOlne Imoistened Chlorine Gas (Chloric Gas,see Exp. No. 11), and in a few moments the color wiU have faded, leaving the ma­terial white. The dye has been "bleac1he,d out" by the chemical action of the ChlorineGas.

EXPERIMENT NO. 18A Test for th'e Presence of Carbon Dioxide Gas

Repeat Experiment No.6, and just as the candle goes out, take the bottle whichnow c.ontains Carbon Dioxide and pour Lime Water (see Exp. No. 25) into the bottle,shaking the contents well. Exan1ine the solution and you will note that it containswhite particles, and that it is turbid. The white particles are Calcium Carbonate(CaCOa) and are insoluble in water, hence ,here we have a good test for the 'presenceof Carbon Dioxide Gas.

EXPERIMENT NO. 19Preparing Sodium Hydroxide (Caustic Soda) (NaOH)

This is used in the manufacture of soap, bleaching solutions, etc. In a largetest tUlbe one-quarter full of Water (H20), .place one-quarter of a Imeasure -ofCalcium Oxide (CaO) and an equal amount of Sodium C'aflbonate (Na2Coa). Nowboil this solution for five 'minutes and then allow it to cool. Upon cooling, therewill be found a sediment of solid matter, while the clear -soluti,on, -when felt, has a"soapy feeling." It is well to filter this solution and put aside for future experin1ents,labeling it "Sodium Hydroxide" ( aOH).

EXPERIMENT NO. 20Production of Nitrogen Gas (N)

In a test tube place one-fourth measure of Ammonium Sulphate (NH4)2 SO",and one-half measure of Sodium Nitrate ( aNOa) and moisten with about six orseven drops of Water (H20), -whereupon Nitrogen Gas (N) will be produced.

EXPERIMENT NO. 21Production of Ammonium Chloride (NH 4CL)

Put five to ten drop,s of Aqua A'mmonia in a test tube and cover same with apiece of stiff paper. Do likewise with a similar am,ount of Hydrochloric Acid (HCI),invert and place the test tubes on top of each other. Pull the papers out. Whitevapor will appear, the particles of which are Amlmoniun1 Chloride or Sal Ammoniac(NH"Cl).

18

THE ELECTRO

EXPERIMENT NO. 23Boric Acid (HaBOa)

This acid is produced ,by filling the large test tube one-sixth full of water towhich is added twelve drops of Sulphuric Acid (H2S04) and three measures otSodium Borate ( aB02). This rmixture should now be boiled for a few momentsand then allowed to cool. Upon cooling there will be found some flat and glossycrystals of Boric Acid. Label liquid for future use, "Sulphate of Soda," and retainB,oric Acid crystals.

EXPERIMENT NO. 22Making Sulphuric Acid (H2S04 )

Take one-third measure of -Sulphur (S) and one measure of Manganese Dioxide(Mn02) in a large test tube. Heat this mixture and by means of a delivery tube, thefree end is 'placed in -a saucer or cup containing one ounce of water. (See diagram,Ex. No.9). After cooling, the resultant liquid will be a solution of Sulphuric Acid(H2S04). Lalbel and :hold.

EXPERIMENT NO. 24Testing Boric Acid (HaBOa)

Fill a small test tube ,one-half full of water and dissolve one-half measure ofBoric Acid in this water. Now put a few drops of alcohol and a few ,drops of "thesolution just mia-de (Sulphate of Soda) (Na2S04) into the measure and light it bymeans 'of a match. The fact that a green flame results, indicates that it isB10racic Acid (HaBOa).

EXPERIMENT NO. 25Making Lime Water

Here Calcium Chloride (CaCI2) is used. Three measures are placed in a halfglass of water and the resulting solution stirred. I t should then be allowed to standunti~ the ,powder settles. N ow pour off the resulting clear solution and mark it"Lime Water." (Prove by use of te,st for presence of lime; see Ex. No.4.)

EXPERIMENT NO. 26Violet Iodine Vapor

Put a small quantity of iodine crystals in a test tube and apply very gentle heat,whereupon it will be noted that a wonderful and mlost beautiful violet gas is given off.

EXPERIMENT NO. 27Explosive, Using an Iodine Base

. Put a very small quantity of Iodine Crystals in a dish and cover them with afew drops of (aqua) Ammonia, and allow saJme to evaporate. In a short while crystalswill form, and they should be broken up into small pieces, while wet; and then al­lowed to dry on blotting paper.. Touching this with a stick at the end of which is abit of cotton will cause it to expl10de violently. We advise handling very carefully.

EXPERIMENT NO. 28Another Way of Producing Hydrochloric Acid

Put two measures of Sodium Chloride ( aCl) in a test tube. Cover it well with~ 40% solution ,of Sulphuric Acid (H2S04) and a.I1ow to heat gradually. Hydro­chloric acid gas will be given off and should be connected by means of a delivery tubeand 'another test tube one-half full \of water. A saturated solution is the result.

EXPERIMENT NO. 29Calcium (Ca)

Take three teaspoonfuls of Calcium ulphate (CaS04) and add just enoughwater so that a pasty cream results. An impression can be made from this bypressing a 'penny into it, or any figure m'ay be moulded and when it- hardens itretains the imparted shape.

EXPERIMENT NO. 30Precipitating Barium Sulphate (BaS0 4 )

Take 10 drops of Water and add two drops of Sulphuric Acid. Now add a fewdrops of Barium Chloride (BaCI2) and you will have a white precipitate of BariumSulphate.

19

EXPERIMENTS IN CHEMISTRY

EXPERIMENT NO. 31Formation of Zinc Oxide (ZnO)

Heat one-half ,measure of Zinc Carbonate (ZnCog) and see that a supply of fres,hair is constantly passing over the chemlical. Zinc oxide will form in a few minutes.

EXPERIMENT NO. 32Green Paint

Take one-third measure of Nickel Chloride (N'iCI2) and pour a few drops ofAmmonia on same. A beautiful light green paint is the result.

EXPERIMENT NO. 33Iron Chloride (FeCI~)

Heat an iron wire until it is red hot and allow sa'me to pass over a te/st tubefrom which some hydrochloric acid gas is escaping. Light green crystals of ironchloride form.

EXPERIMENT NO. 34Copper Chloride (CuCI2 )

Into two ounces of distilled \TVater place three measures of Copper Sulphate(CUS04). In one ounce of distilled Water make a saturated solution of Carbonateof Soda (Na2COg). N ow, add the latter to fhe former, until the solution is distinctlyalkaline (test wit1h red lit,mus paper). The blue precipitate should be allowed tosettle, and a,s 111uch of the clear liqui,d should be poured off as is possible. SufficientHydrochloric Acid (HCI) -should now ·be a1dded so as to just dissolve the prec:ipitate;which it does readily, with effervescence. Upon allowing the liquid to evaporate,green crystals of Cupric Chloride will be for111ed. T1his should be labeled andheld for future use.

EXPERIMENT NO. 35Nickel Nitrate Ni(NOa)2

The Chloride or Sulphate of Nickel should be· treated as in the above experi­ment with Sodium Car/bonate. The precipitate ,sh'Ould be dissolved in diluted NitricAcid. Green Nickel Nitrate is thus 'produced and may be crystallized and reta'inedfor other experiments.

EXPERIMENT NO. 36Hydrogen Sulphide (H2S)

Hydrogen Sulphide is known as "Chemists' Food;" however, it is not to be eaten.It is prepared by putting one measure of Iron Sulphide (FeS) in a test tube and cov­ening same with I%: inches Water. Sulphuri,c Acid should now be poured down thetube until the gas begins to form. Attach a delivery tube and collect the gas underwater. When the action has stopped, a little more acid should be put in. (Five partsWater to one part Acid.)

EXPERIMENT NO. 37Crystallization of Sulphur (S)

Heat some Sul,phur in an eva'porating dish nnt'il it melts, care being taken tosee that the temperature does not become too high. Then allow it. to cool. It willbe noted that as the sl1lpJhur cools, small crystals ,shoot out continually.

EXPERIMENT NO. 38Effects of Sulphur Gas

H'eat some Sulphur in a test tube, and note the following: A copper tube willcatch fire when placed in this tube. Nickel powder will burn spontaneously. Anymetal heated a little before 'it is placed in this gas will melt rea'dily.

EXP'ERIMENT NO. 39Mercury of Tin

Take a small amount of granulated T·in and put a drop of Mercury over it. Itwill be found that at once the Tin dissolves and apparently co'mbines with theMercury.

EXPERIMENT NO. 40Carbon (C)

Procure some corn or cane syrup and allow a few drops of Sulphuric A,cid tofall on same. \Vithin a few seconds steam will be given off and Carbon (C) formed.

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THE ELECTRO IMPORTING CO., N. Y.

EXPERIMENT NO. 41Charcoal

Into a small test tube put a few pieces of wood and heat the test tube. In a.short time the pieces wiU turn to charcoal and the gases (combustible carbon gases)given off can be lighted.

. EXPERIMENT NO. 42Chlorine Smoke

Put two measures of Ammonium Chloride (NH4Cl) in a test tube, and heatgently for a minnte. A large quantity of smoke will ·be given off, until theAmmonium Chloride is volatilized.

EXPERIMENT NO. 43Does Your Mouth Contain Acid?

Place a piece of Iblue Litmus Paper in your Imouth, and if it turns red it ·is asure indication that you have an acid n10uth, and it is probably due to decayed teethor to a sour stomach.

EXPERIMENT NO. 44Testing Soil

Dig up some soil and put a piece of blue Litmus Paper three-fourths of itslength in the soil and aUow it to stand for half an hour. If at the end of this time ithas turned partly red, it is an indication that the soil is acid and needs liming.

EXPERIMENT NO. 45Reduction of Water in Volume

F·ill a test tube one-half full of Water, marking the level of same in tube; thenpour in an equal quantity of Alcohol. I t will be noticed that the resulting heightwill be less than 'previously, due to the chemical affiliation existent between Alcoholand Water.

EXPERIMENT NO. 46Another Way of Boiling Water

Put a few drops of Sulphuric Acid in a test tube and then pour a few drops ofwater over this. The water w'ill boil immediately.

Caution: Do not expose any part of your body to mouth of test tube as acidis spattered out when the water is poured upon it.

EXPERIMENT NO. 47Discoloration of Flowers by Chemicals

A few dr·ops of Water should be added to some Chlorine Gas. Any flower putin this mixture will lose its color. The action is one of bleaching. .

EXP'ERIMENT NO. 48Disappearing Writing

A letter written with the ordinary ink and imm,ersed in a bottle containingChlorine Gas, will cause the writing to fade away. This is a :bleaching action.

EXPERIMENT NO. 49Invisible Ink No.1

Take a lemon and squeeze all the juice out, and write with an ordinary pen.Upon being heated the writing will become visi'ble.

EXPERIMENT NO. 50Invisible Ink No.2

Dissolve equal parts of Copper Sulphate (CUS04) and Ammonium Chloride(NH4Cl) in water until it becomes light green. F'ollow procedure in ExperimentNo. 49. When heated the writing will turn yellow and become legible.

Some other Ink Recipes are given in the formulas below:

MAGIC INK RECIPESRed Ink.-One drachm Potassium T'hiocyanate to one-half ounce of Water. Re­

agent-One-'half ounce 10f Ferric Chloride to one ounce of Water. Apply with a mopor brush and writing will appear red.

21

EXPERIMENTS IN CHEMISTRY

Blue Ink.-One drachtTI Potassium Ferrocyanide to one ounce of Water. Re­agent-Fifty per cent. solution of Ferric Chloride or other ferri.c salts.

Blue Ink.-One drachm Potassium Ferricyanide, otherwise called Red Prussiateof Potash (note, not Ferrocyanide, which is Yellow Prussiate of Potash), to oneounce of Water. Reagent-Strong solution of Ferrous Sulphate.

Black Ink.-Tannine (strong solution) for the writing solution. Reagent-Verystrong solution of Ferrous Sulphate.

Glycerine gives the ink more "body."

EXPERIMENT NO. 51Erasure Ink

Take ordinary starch and dissolve -it in water and then add some iodine (I), andshake well. Use this as regular ink. I t can be erased when dry and will leave notrace, by simply rubbing a c.loth over it.

EXPERIMENT NO. 52Preservation of Flowers

Dissolve t~o large measures of Ammonium Chloride (NH4Cl) in a glass ofwater (H 20). If the flowers are 'put in a ·case containing this solution, they 'may bekept for quite a while.

EXPERIMENT NO. 53Discoloring Vegetables Chemically

To deprive all vegeta:bles of their colors, use a solution of Chloride of Lime.They will lose all vestige of ever having had color.

EXPERIMENT NO. 54Oxalic Acid

For cleaning a straw hat:In a tumbler of Water place two spoonfuls of Oxalic Acid and use as a cleanser

on your straw hat. It may be used for renovating rust stains, cleaning copper andbrass, etc.

Caution: This is a poison. Care must be exerted.

EXPERIMENT NO. 55Tin Plating by Chemical Action

Take two measures of Tartaric Acid (H 2 C4H 4 Ca) and allow same to be dissolvedin two ounces of Water (H20). ,ow throw in some Tin (Sn) and a new penny(C) and boil all the water off, whereupon you will find a silver coated penny.

EXPERIMENT NO. 56Copper Plating

In a small test tube put two measures of Copper Sulphate (CUS04) and fill halffut.1 of water. ow put a clean piece of Carbon (C) or Steel (Fe) in the tube andafter a few moment,s it will be copper coated.

EXPERIMENT NO. 57Electroplating with Battery

In the graduate place a strip of Copper and the article to be plated. Now fillwith the solution as used in Experilment o. 56 and connect to a -battery of threevolts. I t is in1portant to see that the strips of Copper are connected to the positive orcarbon pole of the battery.

The article to be plated is connected to the negative or zinc of the battery. Thisprocess is much faster than the preceding one.

EXPERIMENT NO. 58Fireproof Mixture

Make the following mixture:Ammonium Carbonate, 1/6 mea,sure.Boracic Acid, 1/5 measure.Ammonium Sulphate, lh Imeasure.Sodium Borate, 1/10 measure.and Corn Starch, to make a pasty substance.Dissolve in a large test tube half full of Water. All articles soaked in this mix­

ture will become fireproof. T'his solution is used extensively to dip the filmy gauzedresses of 'ballet dancer and the scenery used in theatres.

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THE ELECTRO IMPORTING" CO., N. Y.

EXPERIMENT NO. 59Fireproofing Any Kind of Fabric

A very good formula for this purpose is as follows:Boric Acid, 3 measures.B,orax, 4 (measures.Water, 2 ounces.Paint or soak fa:brics in the solution; then either hCl:ng up to dry or press fabric

with a hot iron.

EXPERIMENT NO. 60Preparing Explosive Paper

Dissolve some Iodine crystals in aqua Ammonia; the amount makes no differ­ence and for best results the crystals should not "be entirely dissolved. Then pourthe solution in a filter paper to filter. The pre,cipitate should then be put on differentpieces of pa/per and left to dry. When dry the paper will explode if touched;the thicker the precipitate has been put on the paper the louder the report. A jokecan be played on anyone by placing it, when almost dry, vl'here they will touch itwhen it is dry. Don't handle when dry because it will explode very easily. Theexplosions will take place very easily. The explosions are harmless to anyone butthey cause heat and for this rea,son care should be taken where they ignite. Thecorrect proportion can best be found by experi'ment, since it differs with the material.One part <of Iodine to 5 parts of Ammonia gives good results.

EXPERIMENT NO. 61Producing Fireworks (Yellow Stars)

A small qauntity of ntin10ny should be thrown into a long tube filled withChlorine Gas and held mouth upward, whereupon it will produce a shower of burn­ing yellow stars. This is similar to the method employed in making the 4th ofJuly Roman Candles.

EXPERIMENT NO. 62Parchment Paper

Obtain some unsized paper and "make a solution of 1 part Water and two partsSulphuric (H2S04 ) Acid. ow dip the paper into this solution for less than onesecond and thoroughly wash the pa'per in clean running water. Allow it t,o dry andthen proceed to write w:hat you wi h upon it. It will withstand much more of astrain than the -ordinary paper.

EXPERIMENT NO. 63Fresh Egg Test

One may determine the freshness of an egg Iby floating the egg in a solutionof sodium chloride (comlmon table salt)-if the egg readily floats it has a low specificgravity and that is a sign that it is stale while if the egg sinks rapidly it is fresh.

EXPERIMENT NO. 64Testing Flour for Bleaching Substances

Obtain one measure of flour as used for 'baking and put in a test tube. Nowpour enough gasoline to fill the tube one-quarter full and after shaking for afew minutes and the Imixture having been allowed to settle, a yellow solution willindicate unadulterated flour. If the flour i,s bleached, the solution will be nearlycolorless.

EXPERIMENT NO. 65Invisible Pictures Made Visible

Use some of the Hydrogen Sulphide Gas (H2S) as generated previously in thefollowing manner. Paint a picture Imade up· with a solution of one-half measure ofLead Acetate Pb(C2H 30 2)2 in one ounce of Water and allow it to dry. By passingthe 'Picture tJhrough the gas it immediately becomes visible in a dark brown tone.

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EXPERIMENTS IN CHEMISTRY

EXPERIMENT NO. 66The Trick of the Changing Colors

Get a picture or photograph of a girl and paint her hands and cheeks withPhenolphthalein Solution (bought at any drug store). Having thus prepared the pic­tures you are ready for your trick. Put in a glass some Aqua Amlmonia (whichlooks like water) and with a 'brush wash the picture 'back and forth with this liquid.The parts painted with Phenolphthalein will appear red to the amazement of youraudience.

EXPERIMENT NO. 67Pink Color

Put two ounces of clear Water in a large test tube (a'bout one-half full) and dis­s'olve one-half measure of sodium carbonate. By a,dding a few drops 'of fresh Phen­ol'phthalein, the solution will turn pink.

EXPERIMENT NO. 68Blu'e Dye

Into a test tube half filled wit'h Water place ten to twenty drops of mmoniaand then put in a few pieces of ·bark obtained from the horse chestnut or birch tree.As a result of the chemical action a blue dye 'will be formed.

EXPERIMENT NO. 69Chemical Growths Resembling Foliage

A 10% solution of Sodium Sili'cate (water glass) is put into a glass or beaker,and crystals of any or all of the following salts are dropped in; Copper Sulfate,Ferrous Sulfate, Nickel Sulfate, CO'balt Nitrate, which can be purchased at any drugstore. Many other salts will give similar results 'but the various sulfates appear tobe the best.

Shortly after the crystals are placed in the solution they will begin to grow infantastic shapes, each of the salts giving a different growth of different color. The,segrowths look 5'0 much like undersea foliage that they have often been called "Sub­marine Gardens.'"

The rate of growth depends on the strength of the silicate solution; as thecrystaLs are due to a formation of the silicate of the particular salt used. A solutionof the strength mentioned above allows the crystals to grow in a more even man­ner at a rate which can be watched. The growths, however, will not keep unlessthe solution is very weak, and then they grow too slowly.

EXPERIMENT NO. 70Making a Solid from Two Liquids

Make up a transparent solu/tion of Zinc Sulphate (ZnS04). Fill a glass half fullof Zinc Sulphate solution and another with half glass of strong Ammonia (NHs).

Pour them together and if the proportion be properly maintained a solid will result.

EXPERIMENT NO. 71To Make Solids from Liquids

Pour a concentrated solution of Water Glass (sodium silicate) into a glass andadd enough Hydrochloric Acid (HCI) to make the solution aci'd. The solution willturn into a solid resembling an opal and if the dish is inverted it will not fall out.

Dissolve a lump of alum in water and add enough Ammonia Water so t:hat thesolution smells strongly of it. Shake the mixture and it will turn to a thick trans­parent jelly.

EXPERIMENT NO. 72Saturn's Trees

Put one measure of Lead _Acetate into a test tube one-quarter full of Water. Thissolution sh'ould be heated gently, and a strip of zinc should be allowed to hang onthe inside for about ten hours, after which period, fern-like formations will befound.

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THE ELECTRO IMPORTING CO., N. Y.

EXPERIMENT NO. 73All from One Bottle

Fill a one-pint green bottle with a solution made up of Sulphate of Iron (FeS04),one teaspoonful into a pint of warm Water, and upon dissolving) add seven drops of.Sulphuric Acid (H2S04). Then procure four wine glasses. In the first glass, put onemeasure of Calcium Chloride (C'aCI2) and allow it to dissolve in a few drops ofWater. Leave the second empty. In the third put 1/6 measure of Potassium Per­m'ancranate (KMn04) which can be obtained from any drug house. The fourthshould contain one measure of Sodium Bicarbonate (NaHCOa) mixe'd with a fewdrops of Water (H20). ow as some of the liquid is poured in the first glass, therewill appear to be milk; in the second, water; in the third, wine; and in the fourth,champagne.

EXPERIMENT NO. 74Freezing Solution

Fill a test tube half full of water and place in an ordinary glass. N ow put someIce and Sodium Chloride (NaCI) in the outer glass jar. It will be found that upontaking temperature readings of the water in the test tube that they fall below zeroo C.,or below 32° F. It is important that the water be kept still.

EXPERIMENT NO. 75Blue Liquid from Two Colorless Liquids

Take one-quarter measure of Copper ulphate (CUS04) and dissolve same ina few drops of Water. ow dilute it until it appears colorless. Put a few drops of

qua Ammonia into this solution and it will turn blue.

EXPERIMENT NO. 76Green Paint

Take one-half measure of Sodium Carbonate ( a2COa) and dissolve it in a smalltest tube one-quarter full .of Water. N ow put an equal amount of Copper Sulphate(ICUS04) in an equal amount of ater and boil thi solution. The Sodium Car­bonate solution should now !be mixed with the Copper Sulphate solution, whereupona beautiful green paint will be had.

EXPERIMENT NO. 77Transparent Soap

Procure one measure of White Soap, and take about thirty drops of Glycerol.Put this in a smal.1 tin tray and heat over the flame of a iBunsen burner or analcohol lamp for five or ten minutes until all of the Soap has melted and mixed withthe Glycerol. N,ow wait until it cools and it will be found that upon solidificationthat the resulting Soap is transparent.

EXPERIMENT NO. 78Electrolytic Rectifier (to Change A.C. to D.C. Current)

In a small test tube putan Aluminum electrode anda Lead electrode. Fill thistube with a saturated solu­tion of Sodium Phosphate.Connect as per diagram withA. C. supply of curren t anda D. C. current will be ob­tained. As this outfit is sosmall it is advisable to con­nect a 10 W. lamp in seriesas shown.

D.C.

DC.

25

A.C.

/o/Yoll IJU/.6

A.C.

EXPERIMENTS IN CHEMISTRY

EXPERIMENT NO. 79Making Sm'elling Salts

Take one measure ,of Calcium Oxi'de (CaO) and one measure of AmmoniumChloride (NH4CI). Now heat the m'ixture over a flame for five minutes. It willbe noticed that a gas is generated which has the property of reviving one who hasfainted. This is Ammonium Gas.

EXPERIMENT NO. 80Making a Weather Barometer

In a small test tube put one-half ounce of Alcohol and then one measure ofAIUlm. With the approach 'Of bad weather the Alum will cal1se the mixture to appe'arturbid, and on clear weather will turn clear.

EXPERIMENT NO. 81Plaster of Paris

Take two measures of Calcium Chloride (CaCI2) and allow it to dissolve in oneoz. of Water, in a small test tube. Stir constantly with a glass rod so as to insure agood mixture. N ow add Sulphuric Acid until the solution solidifies. Thus we havePlaster of Paris.

EXPERIMENT NO. 82A Good Test for Copper

First take the solution supposed to contain Copper and put it in a shallowvessel. When the solution is ready, im'merse a pie.ce of Iron or Steel that has beencleaned of all rust. If the solution contains C,opper the Iron or Steel will be coatedwith MetaHic Copper. Should Copper not show in this test pour into the solution alittle Ammonia; if Copper is present a light blue precipitate will form and thesolution will take on a blue col'or.

EXPERIMENT NO. 83Chemical Colors

An infusion of Logwood Chips and Water will change color when other chemi­cals are adde,d.

Take three glasses, Nos. 1, 2, and 3, and prepare the'm as follows :-Rinse No. 1with strong Vinegar; dust No.2 with Powdered Alum; rinse o. 3 with a solutionof Copper Sulfate. The next step is t,o pour the Logwood into each. If the glasseshave been prepared correctly the Logwood in 1TO. 1 will fade to a pale yellow.That in No. 2 will become almost black and that in o. 3 will change to a palepurple. This is the principal set of changes, but foI.1owing is a list of changes usingnot only Logwood but other chemicals also. Som1e of them can Ibe used as stateda;bove but in the case of Ammonia, for instance, the odor would give it away.

Color changes that are due to chemit;;:al action.1. Logwood mmonia and Copper ulfate give a brown.2. Logwood, Vinegar and Ammonia give a purple.3. Logwood, Alum and Ammonia cause a red precipitate.4. Logwood, Vinegar and Copper Sulfate give a brown.5. Logwood, Amlmonia and Common Salt give a light brown.6. Logwood, Copper Sulfate, Clom'm/on Salt and Alum, mixed, give a pink.7. Phenolphthalein and Ammonia give a bright red (test for free Am.monia).8. Copper Sulfate and Amm'onia o-ive a bright blue (test for Copper Sulfate).9. Logwood and Hydr,ogen Peroxid o-ive a pale yellow.10. Logwood and Copper Sulfate and Caustic Soda give a pale blue precipitate.

EXPERIMENT NO. 84Making a Crystal Basket

Water 'will, espe,cially when boiling, dissolve large quantities of various sub-stances, which when the ater has cooled, are left behind in the form 'Of most

.beautiful crystals, the shapes of which may vary with the substance employed. Onemay take advantage of this fact to nlake very handsome ornaments. It is also knownthat boiling Water will take up a much larger quantity of Alum than cold Water.If we dissolve as much Alum as possible in the former, as the liquid co'Ols, crystals.of Alum will be ,deposited on any obje,ct p'laced in the fluid. A piece of Coke orCinder allowed to stand in a boilino- solution of Alum will become coated with nu­mer,ous glistening crystals as the liquid cools. It will have the appearance of anaturally formed mineralogical pecitmen.

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THE ELECTRO IMPORTING CO., N. Y.

Ornamenta1 baskets, etc., may be formed in this way by covering wire or willowbaskets. The baskets covered wi th wire and then cotton are the most successfulas the surface to !be coated with crystals must be somewhat rough. Take twice asmuch Water as will be sufficient to cover the 'basket, boil it in a saucepan and addas much Alum as will dissolve in the water. A quart of Water will require about 18ounces of Alum. Strain this through muslin or blotting paper into a large jar apdhang the basket in the boiling liquid. Stand the jar on one side to cool and keep freefrom dust. In a few hours the basket will be com,pletely covered with white crystalsof Alum. Should it be desired to color the crystals, add the requisite dye-stuffto the Alum solution before straining it. A few drops of cheap dye will serve thepurpose \Nell.

EXPERIMENT NO. 85Cold Soft Solder

Precipitate some Copper from a Copper Solution, such as Copper Sulfate orCopper Nitrate by means of Zinc or Iron filings. Into a mortar pour some Mercuryand the Copper Precipitate. Add a few drops of dilute Sulfuric Acid and o-rinduntil the Copper has united with the Nlercury. Wash the Amalgam with Water tillbright and clean. Put into a cloth to dry and by means of a twisting motion, likegrapes are strained, squeeze out the exces's of Mercury until the Copper Amalga,mis just workable~by the fingers. Rub well into the surfaces to be joined and presstogether over night. Some of the 1\1 ercury penetrates the surface and some of theCopoer Crystalizes out, and the compound becomes very hard. Strange t.o say thiscompound is silver white. By using more Mercury a pliable metal is obtained thathardens slowly. If the solder is too hard, grind up with more Mercury. Keep Goldand Silver]ewelry. etc., out of the way, as Mercury destroys them.

EXPERIMENT NO. 86Undercooled Water

Obtain a tumblerful of crushed Ice and mix in two or three spoonfuls of ordinaryTable Salt. N ow place a clean test tube about one-!quarter full of pure Water inthis mixture. Do not allow any of the Salt or Ice to get into the test tube. If keptperfectly quiet, the water in the test tube may be cooled to minus 4 or 5 degrees Cen­tigrade (25 ,degrees) Fa'hrenheit) even as low as minus 10 degrees Centigrade (15degrees Fahrenheit), without solidifying. If this water in the undercooled state isstirred, ·or if a tiny crystal of ice is -added, it immediately freezes and its te,mpera­ture rises to zero degrees Centigrade or (32 degrees Fahrenheit) the freezing point.

EXPERIMENT NO. 87An Explanation of Solution

Dissolve a spoonful of common Table Salt (Sodium Chloride) in a half glass ofWater.

N ow pour this solution into a small pan or sim/ilar cooking utensil and heaton the stove until the water is all driven off. Taste what you find remaining inthe 'Pan and satisfy yourself that it is the same Salt that you -originally started with.Unless the pan is heated very gently and when the salt is nearly dry you wiU findthere will be some violent popping due to the expansion of steam in the crystalsof Salt.

EXPERIMENT NO. 88Softening Hard Water

If the water in your hOtne is hard, add a spoonful of household atnm\onia to abasinful of this water before washing in it. Note the ease with whic'h a lather canbe raised with the soap.

EXPERIMENT NO. 89Making Water from Fire

Take a cold dry glass and invert it over a lighted candle, holding the mouthjust above the flame for a few seconds. Remove glass and examine the inside ofsame. You 'will observe that a film of m\oisture has been deposited on the inside ofthe cold glass. .

T'he water was liberated from the flaJme in the f.orm of steam and in order tom'ake it visilble it was necessary to condense it on some' cold object:

27

EXPERIMENTS IN CHEMISTRY

EXPERIMENT NO. 90Making Ammonia in Your Hand

Put one measure of Calcium Oxide and one measure of Am1monium Chloride inthe palm of your right hand and mix with the index finger of your left hand. Smellthe mixture occasionally and notice that Ammonia gas is being generated.

EXPERIMENT NO. 91Another Way of Making Ammonia

Place two measures of Ammonium Chloride in a test tu'be and add two measuresof Sodium Car1bonate (Na2C03). Heat the mixture gently and notice the smell ofammonia at the mouth of the test tube.

EXPERIMENT NO. 92A Study of the Prop'erties of Sulphur

Place two measures of Sulphur into a dry test tube and heat gently over a flame.1. N ate that it first melts to a dark liquid and then is converted into vapor. The

vapor recondenses in the cool upper part of the test tube.2. N ow put two measures of Sulphur in a spoon and heat this over the flame.

While the Sulphur is burning smell it cautiously. In o. 1 the Sulphur in the testtube did not burn because there was an insufficient supply of air. In No.2 the Sul­phur did burn, due to the fact that it united with the Oxygen (0) of the air formingthe o-as, Sulphur Dioxide (S02).

Sulphur is odorless; try it by sme1ling. What is usually termed the odor ofSulphur or Brimstone is the smell of Sulphur Dioxide.

EXPERIMENT NO. 93Flame Color Test for Zinc

Place a small quantity of Granulated Zinc in the bottom of your measure ~nd

shake small quantities of it into the flame of the alcohol lamp. Note the str'onggreenish tinged flame which ensues. This flame is characteristic of Zinc and itscompounds.

EXPERIMENT NO. 94Coins

Heat a copper cent in a gas flame or on a coal fire until it becomes red hot.Let a few drops of Water fall on the coin and when it cools, take note of the forma­tion of Black Copper Oxide which covers it. Try the above experiment with a silverten cent piece and observe that a somewhat lighter coat of Black Oxide is obtainedin this case. Pure silver will not oxidize in air even when heated. The blackcoating is Copper Oxide (CuO) and the presence of same proves that the coin is notpure silver.

EXPERIMENT NO. 95The Decomposition of Sugar

Sugar is a compound of Hydrogen, Oxygen and Carbon. When heated theHydrogen and Oxygen are given off in the form of Water and the Carbon remains.

Place 4 measures of granulated sugar in a spoon and heat it over an alcohollaJmp flame for a few moments. The sugar finally melts and turns brown. Water(H20) is given off in the form of steam and there finally remains a black porous mass,almost entirely Carbon.

EXPERIMENT NO. 96To Make Coal-Gas

Heat some coal-dust in a small flask made of hard glass and pr'ovided with a corkand delivery tube. In a short time a mixture of various vapors will begin to pass offtogether with a certain a1mount of smoke. Some of these vapors wi'll condense onthe upper part of the flask and in the delivery tube. These vapors should then becollected over Water when many of the impurities will be separated, and clear gaswill be obtained. Apply a match cautiou ly and the gas will burn with a bright flamejust as the gas supplied to our homes.

28

THE ELECTRO IMPORTING COo, N. Y.

EXPERIMENT NO. 97

Burning IronTake a fine iron wire and dip one end into Flowers of Sulphur. A little of the

Sulphur will probably adhere; if not, it may be made to do 5'0 by first heating theend of the wire. Now io-nite the Sulphur, and while it is burning pass it quicklyintd a jar of Oxygen. The burning Sulphur heats the Iron wire to redness, andthen the Iron itself c'ommences to burn brilliantly, continuing to do so until eitherthe metal or the Oxygen is consumed. Upon examining the jar there 'will be foundnumerous small particles of a black substance. This is Black Oxide of Iron.

EXPERIMENT NO. 98

Removing Tarnish from Silver by ElectricityTo remove tarnish from Silver electrically, make a dilute acid solution, 1 part

chemically pure Sulphuric Acid to 10 parts of Water, and use a Carbon electrode.Immerse the articles to be cleaned. The tarnish will disappear in a few minuteswithout injury to the silver.

In the absence of a battery, suspend the silverware in the solution and bring apiece of Aluminum in contact with it. This will restore the lustre.

EXPERIMENT NO. 99

Whitening Old and Discolored MarbleTo whiten old and discolored marble mantels, hearthstones, vestiibule floors,

basins, table tops and the like, treat in the following manner:Take some Muriatic Acid, a paint brush and a pair of old gloves. After wiping the

dust off with a wet cloth and allowing the Imarble to thoroughly dry, don your glovesto protect your hands from possible c'ontact with the acid and pro-ceed to brush theacid over the marble as you would a paint. You will be obliged to turn your headand take a breath between strokes so as to avoid inhaling the fumes which arise asyou apply the acid. The marble 'will show astonishing results.

EXPERIMENT NO. 100

Cementing Glass Receptacles, Tubing, etc..Take about half a pound of finely pulverized Stone and Glass (in equal propor­

tion, i. e., a quarter pound of each), and after thoroughly mixing it with four ouncesof Sulphur subject the compound to a moderate heat until the Sulphur melts. At thispoint stir well until the whole is homogeneous, and then pour into a mould untilrequired for use.

When needed, it should be reheated to 248 degrees F., at which temperature itmelts freely. This cement is a:bsolutely impervious to water, it resists acids and allatmospheric action, is not affected by boiling water and even at a temperature of 230degrees it holds firmly and remains hard.

----~----

29

EXPERIMENTS IN CHEMISTRY

PoisonsPOISON - ANrrIDOTES

Antidotes(a) Acids

Oxalic Chalk, whiting, or magnesia in water.Nitric Bicarthonate of soda, or carbonate of magnesia,Hydr·ochloric chalk; in emergency, plaster of the room beatenSulphuric up in water.Carbolic White of egg well ,beaten up with water. A tea-Muriatic spoonful of mustard flour in a cup of hot water.Nitro-Muriatic Very thick lime water.Acetic Soap and water, lime, magnesia, milk, oil, thick

gruel. ,Carbonic Fresh air, artificial respiration, friction.Tartaric Lime 'water, castor oil.Chromic White of egg in water. Mustard flour.Prussic Continuous and heavy douches of ice cold water

over head and back. Mustard plasters onstomach and soles of feet. Prevent sleep.

(b) Metallic SaltsAcetate of Lead Sulphate of soda or magnesia.Bichromate -of Potash Magnesia and chalk. Emetics.Nitrate of Silver Common salt in water, followed immediately by

emetic.Preparations or compounds of White of egg in water. Teaspoonful of mustard

Chromium, Antimony, Cop- flour in cup -hot water.per, Mercury, Zinc .

(c) Caustic AlkalinesAmmonia Vinegar in water. Lem'on JUlce. Oil. Demul-Potash cent drinks. Large doses of milk.Soda .

(d) Vegetable PoisonsIvy Saline laxatives.

Apply weak lead water and laudanum, or limewater and sweet oil; or bathe freely with spiritsof nitre.

Alcohol Strong coffee. Douche. Stomach pump.Belladonna Stomach pump. Emetics. Coffee. Artificial res-

piration.Digitalis Stomach pump. Emetics. Tannic acid. Stimu-

lants.Mushrooms Stomach pump or emetics. Ca,stor oil. Warmth.

Stimulants.Opium, Morphine tomach pumps or emetics, inhale ammonia.

Douche. Artificial respiration.Nic-otine tomach pump or emetics; stimulants, tannic acid.

Hot applications to skin; keep patient lyingdown.

(e) MiscellaneousEther, Petroleum, Benzine, Fruit Plenty of mustard flour in large quantity of hot

Essence water. Cold water douches. Fresh air. Pre­vent absolutely sleep.

Arsenic and all compounds Stomach pump. Teaspoonful mustard flour inhot water. Teaspoonful dialyzed iron mixedwith same quantity of calcined magnesia everyfive minutes for one hour. Then plenty of oil,or milk.

Chloroform Stomach pump or en1etic. Solution of carbonateof soda. Mustard to the heart.

Coal Gas Mustard to the heart. Artificial respiration. Stim-ulants.

Iodine Stomach pump or emetic. Starch.Phosphorus (matches) Emetic. French oil of turpentine. Copper Sul-

phate. Purgatives.Snake Bite Cauterization and ligature. Stimulants. Perman-

ganate, liquor potassae, artificial respiration.Ammonia injection.

30

THE ELECTRO IMPORTING CO., N. Y.

CHEMICAL SUBSTANCES-THEIR TECHNICAL ANDCO'MMON NAMES

Nearly all the chemicals in common use today have more than one name, andthe purpose of this list is to classify some of the most common ·ones in use for thebene'fit of the a,mateurs who sometimes bec'ome confused in the different names.Chemicals in the two lists opposite eac·h other are the same.

Common Name

Aqua FortisAqua RegiaBlue Vitriol, Qr Blue StoneCalomelChalkCreanl of 'fartarSalt of TartarCaustic Potassa (Potash)ChloroformCommon SaltCopperas, or Green VitriolCorrosive SublimateDry AlumEpsom SaltsEthiop's MineralGalenaGlauber's SaltsIr,on PyritesJewelers PuttyKings YellowLaug,hing GasLimeLunar CausticMuriate of LimeNiter of SaltpeterOil of Vitriol .RealgarRed LeadRust of IronSal-Amm·oniacSlacked LimeSodaSpirits of HartshornSpirits of SaltStucco 'or Plaster of PariSugar of LeadVerdigrisVermilionVinegarVolatile AlkaliWaterWhite VitriolBoraxBrimstone

Chemical Name

itric Aciditric and Hydrochloric Acid

Su'lfate of C,opperSub-Chloride of MercuryCalcium Cat1bonateTartarate of PotassiumCarbonate of PotassiumHydrate PotassiumChloride of FormyleChloride of SodiumSulfate of IronBi-Chloride of MercurySulfate AIU'm~num and PotassiumSulfate of MagnesiumBlack Sulfide of MercurySulfi'de of LeadSulfate of SodiumBi-Sulfide of IronOxide of TinThe Sulfide of ArsenicProtoxide of itrogenOxide of Calcium

itrate of SilverChloride of CalciumNitrate of Potash or Potassium NitrateSulfuric AcidBi- ulfide of ArsenicLead OxideIron OxideMuriate of AnlmoniaHydrate CalciumOxide of SodiumSes.quicarbonate of AmmoniunlHydrochloric or Muriatic AcidSulfate of Lime

cetate of LeadAcetate of CopperSulfide of MercuryJ. cetic Acid (dilute).i\.mmoniaSub-Oxide ,of HydrogenSulfate of ZincSodium BorateSulphur

31

EXPERIMENTS IN CHEMISTRY

Common NameButter of AntimonyFowler's SolutionGypsumHorn SilverHartshornHypoLime WaterLithargeMagnesiaMeerschaumMosaic GoldNiterNiter CakePrussian BluePrussic AcidPyr,oQuicksilverRochelle Sa;ltsSal SodaWater GlassWhite Lead

Chemical Namentimonous Chloride

Potassium ArseniteCalcium SulphateSilver Chloridei\mm'onia WaterSodium HyposulphiteCalcium HydrateLead OxideMagnesium OxideMagnesium SilicateTin BisulphideSodium itrateSodium BisulphateFerric-<FerrocyanideHydrocyanic AcidPyrogallic AcidMercuryPotassium and Sodium TartrateSodium Carbonate (crysta'l)Sodium SilicateLead Carbonate

FORMULASFOR CLEANING VARIOUS SUBSTANCES

Alabaster. Use strong soap and water.Black Silk. Brush and wipe it thoroughly; lay on a table with side intended to

show, up; sponge with hot coffee strained through m,usIin; when partly ·dry, iron.To Remove Stains or Grease from Oil Paint. Use Bisulfid of Carbon, Spirits of

Turpentine, or if dry and old, use Chloroform", These and tar spots can be softenedwith Olive Oil and Lard.

Stains, Iron Rust, or Ink from Vellum or Parchment. Moisten the spot with asolution of Oxalic Acid. A'bsorb same quickly by blotting paper or cloth.

Rust from Steel. Take half ounce of emery powder with one ,ounce of soap and .rub well.

Fruit Spots from Cotton. Apply cold soap, then touch the spot with a hairpencil ·or feather dipped in Chlorate of Soda, then dip imn1ediately in cold water.

Grease from Silks. Take a lump of Magnesia, rub it wet on the spot, let it dry,then brush the powder -off.

Iron Rust may be removed from white goods lby sour milk.Scorch Stains from White Linen. Lay in bright sun.Mildew. Moisten the spot with clean Water, rub on it a thick coating of Castile

Soap mixed with Chalk Scrapings, rub with end of finger, then wash off.Oil Marks on Wall Paper. Apply paste of cold water and pipe clay, leave it on

all night and brush off in the :morning.Paint Spots from Clothing. Saturate with equal parts of Turpentine and Spirits

of Amm-onia.. To Cleanse House Paper. Rub with a flannel cloth dipped in oatmeal.

Black Cloth. Mix one 'part of Spirits of Ammonia with three parts of warmwater, rub with sponge or -dark cloth, clean with Water, rub with the nap.

Furniture, for Finger Marks. Rub with a soft rag and sweet oil.Chromos. Go over ligh tly with a damp linen cloth.Zinc. Rub with a piece of cotton cloth dipped in kerosene; afterward with

a dry cloth.Hands from Vegetable Stains. Rub with a slice of raw potato or lemon.Window Glass. Paint can be removed by a strong solution ·of soda.To Clean Tinware. Comm,on soda applied with a moistened newspaper and pol­

ished with a dry piece will make it look like new.

32

Keep. you Posted on the Latest Scientific Doings

ELECTRICAL EXPERIMENTERScience and Invention

Edited by H. GERNSBACK

Devoted solely to the interests of the experimenter. Is clean, up-to':'date and original. The magazine you must have.

Contains new articles on Electricity, Chemistry and Wireless inevery issue; also the following departments: "The Constructor," "Wire­less Department," "How to Make It," "Latest Patents," "Phoney Pat­ents," "Among the Amateurs," "Question Box," "Patent Advice," "Ex­perimental Chemistry," "Marvels of Physics," "Popular Astronomy,"etc., etc. Every article by an authority.

Each issue contains at least 80 big ~ x 12 inch pages (~ as large asSaturday Evening Post) and 150 to 200 original illustrations that areonly possible on so large a page.

PU:~~:l: PRICE· $2.00 YEA SIND POSTAL fOR ASAMPlf COPY

As a special offer we will give you free, for a limited time only,EITHER a complete copy of the 160 page, 20 lesson "WirelessCOURSE" or a cloth bound copy of the "EXPERIMENTALELECTRICITY COURSE" with a year's SUbscription (12 num­bers) of the Electrical Experimenter at $2.00. Either of thesebooks is worth more than the subscription price, yet you willget 12 big numbers of this wonderful magazine and either bigboo~ FREE for only $2.00. '.

EXPE IMENTER PUBLISH G CO., Inc.233 FULTON STREET, NEW YORK CITY, N. Y.

EX E IME ,•

NAME .•••.•..•..•.•...•..•.....•.••.•.•.••.•......•..•.••••••••••••

'ADDRESS •.........................•.••.•..........•....•....••.••••

STA'I:~, .

. ELECTRO IMPORTING COMPANY!33 Fultoll St., New York City

I enclose herewith 6 cents in stamps or coin for whieh pIe.lesend me your lateBt Cyclopedia Catalog. .

"THE BOY'S ELECTRIJ:C TOYS" contains enough material TOMAKE AND COMP'LETE OVER TWENTY-FIVE DIFFER­ENT IDLillCTRJICAL APPARATUS without any other tools,

except a screw-driver furnished with the outfit. Thebox contains the following complete instruments'l.nd apparatus which are already assembled:

Student's chromic plunge battery, com­pass-galvanometer, solenoid, tele­phone receiver, electric lamp.

Enough various parts, wire,etc., are f u r­nished to makethe following ap­paratus:

Electromagnet,electric cannon,mag net i epic­tures, dan c i n g8 P ira I, electrichammer, galvan­o met e r, v 0 I t­meter, hook for

telephone receiver, con·denser, ensitive micro­phone, short distancewireless telephone, teststorage battery, shock­ing coil, complete tele­graph set, electric riv­eting machine, electricbuzzer, dancing fishel,singing telephone, mys­terious danci ng man,electric Jumping Jack,magnetic geometric fig­ures, rheostat, erraticpendulum, electric but­terfly, thermo electricmota , visual telegraph,etc., etc. .

This does not by anymeans exhaust the list, buta great many more ap­paratus can be built actu­ally and effectually.

With the Instructionbook which e furnish.one hundred experimentsthat can be made with thisoutfi t are listed. ~

The outfit contains'11'4 separate pieces of

· material and 24 piecesof finished art I c I e 8ready to use at once.

Among the finishedmaterial the followingparts are included: Chro­mic salts for battery,lamp socket, bottle of mer­cury, core wire (two dif­feren t lengths), a bottle ofiron filings, three spoolsof wire, carbons, a quan­tity of machine screws,flexible cord, two woodbases, glass plate, paraffinepaper, binding posts,screw-driver, etc., etc.

The size over all of theoutfit is 14 x 9 x 2~.Shipping weight, 8 lbs.No. EX2002 "The BoysElectric Toys," out- $5 00fit as described .. •IMMEDIATE SHIPMENTS