APPENDIX I. OUTLINES OF SUGGESTED EXPERIMENTS ON PART I. I. GIVEN two elements. Find what elements they are; then prepare a compound of each of these elements and prove experimentally that the bodies you have prepared are compounds. (Ferrum redactum; Sulphur.) II. Of the two bodies A and B, one is an element and the other is a compound. Examine quantitatively the action of heat on A and B, and also the action of dilute sulphuric acid on A. From the results of your experiments determine as far as you can which is the element and which is the compound. (A=Ferrum redactum; B=Potassium chlorate.) III. Given three oxides A, B, and C. Determine experimentally which is a basic oxide, which is an acidic oxide, and which is a peroxide. Manganese dioxide; B = Chromic oxide, Cr2O3; C = Chromic (A anhydride.) IV. Given two elements. From the properties of their oxides classify the elements as metals or non-metals. (Zinc powder; Flowers of sulphur.) V. Given four elements. Prepare an oxide of each, and examine the interaction of water with each oxide, determining whether an acid or an alkali is formed, or whether no change Then act on each element with dilute sulphuric acid and determine whether gas is evolved; in cases of gas-evolution occurs. M. P. C. 13 find what particular gas is given off. In those cases where an action occurs and the element dissolves, boil down the liquids, and find whether salts have been formed. From the results obtained classify the four elements as metals and non-metals. What other properties would you expect to belong to those which are metals, and what other properties to those which are non-metals? (Ferrum redactum; Flowers of sulphur; Powdered magnesium; and Powdered charcoal.) VI. Prove that the given oxide is not acidic, but that it reacts with an acid to form a salt. (Chromic oxide, Cr2O3.) VII. Given four salts, A, B, C, and D. Sulphuric acid reacts normally with two of these salts, A and B: the products of the interaction of this acid with C and D are not such as would result from a normal reaction between an acid and a salt. Prove these statements experimentally. (A=Potassium chloride; B = Lead acetate; C= Potassium iodide ; D=Mercuric chloride.) VIII. Given red lead. From it prepare two other oxides of lead. Prove one to be a basic oxide and the other a peroxide. Determine experimentally whether the peroxide does or does not react under any conditions as an acidic oxide. IX. Given a salt A. Find its qualitative composition; then prove that the gas evolved when A interacts with concentrated sulphuric acid is soluble in water and that this solution reacts as an acid. By neutralising this acid solution, obtain the original salt in a solid form. Perform similar experiments with the salt B, and compare the results obtained in this case with those obtained in the case of A. (A=Potassium chloride; B=Potassium nitrate.) X. Given an aqueous solution of an acid, a metallic oxide, a metallic carbonate, and a metal. Determine qualitatively the change that occurs when (1) the oxide, (2) the carbonate, and (3) the metal, reacts with the acid. (Zinc; Magnetic oxide of iron; Sodium carbonate; Hydrochloric acid.) XI. Compare the reactions of the given metal with each of the acids given; determining, as far as can be done by qualitative examination, (1) what gas (or gases) is evolved in each case, (2) what are the compositions of the non-gaseous products of the reactions. (Zinc; Hydrochloric acid; Nitric acid.) XII. From the metal A prepare two salts each composed of the metal and the same acid radicle, establishing by experiments that the salts you have prepared are different in their properties. Find out as much as you can by qualitative experiments regarding the differences between the compositions of the two salts. Determine experimentally whether the metal B forms two salts with the same acid radicle or only one. (A=Iron; B=Zinc.) XIII. From the given salt, prepare that oxide of the metal of the salt which contains the metal and oxygen united in the proportion of three atoms of metal to four atoms of oxygen. [You are not required to prove the composition of the oxide analytically, but merely to identify your preparation with the oxide M.O from knowing the properties of that oxide.] 4 Determine by experiment what salts are formed by the interaction of hydrochloric acid with the oxide you have prepared. Contrast this reaction with that between the same acid and the oxide M2O, of the same metal, which oxide you must prepare. 2 3 (Ferrous sulphate crystals.) XIV. Given a salt A and an oxide B. What changes occur when each is heated? Compare the results obtained with the action of heat on the oxide C. From an aqueous solution of A prepare the same body as results from the action of heat on A. (A=Potassium chlorate; B = Mercuric oxide; C=Litharge.) XV. Given potassium dichromate. Prepare from it, (1) a solution containing a salt of chromium; (2) a specimen of pure chromic hydrate; Prepare potassium dichromate from a portion of the chromic hydrate made in (2). XVI. Given manganese sulphate. Prepare therefrom a solution of potassium manganate ; transform this solution into one of potassium permanganate, and from this solution pass back again to manganese sulphate. Prove that an acidulated solution of potassium permanganate oxidises ferrous to ferric salts, and oxalic acid to carbon dioxide. XVII. Given two oxides, A and B, of the same metal. Prove distinctly and conclusively, (1) that A is an acidic oxide but that B is not acidic; (2) that A reacts with hydrochloric acid to form a salt; (3) that B also reacts with the same acid to form a salt. Determine by experiment what body is produced during the reaction of A with hydrochloric acid that is not produced when B reacts with the same acid. From A prepare B; and from B prepare the potassium salt of the acid corresponding to A. (A = Chromic anhydride; B = Chromic oxide, Cr,2O3.) XVIII. Given an acid in aqueous solution. Prove experimentally that it is monobasic. [At a red heat this acid is completely volatilised but its potassium salt is unchanged.] XIX. (Hydrochloric acid.) Given solutions of sulphuric acid and barium chloride of stated strengths. Prove that the equation BaCl ̧Aq + H2SO1Aq = BaSO4 + 2HClAq accurately represents the mutual reaction of these two bodies. and XX. Given phosphorus pentoxide. From it make (1) a solution of metaphosphoric acid; (2) a solution of orthophosphoric acid; recognising each acid by the usual tests. From the orthophosphoric acid obtained prepare the salt disodic orthophosphate, and from this prepare a solution of pyrophosphoric acid. XXI. Prepare oxygen, nitrous oxide, and nitric oxide; and distinguish these three gases by as many tests as possible. XXII. From copper sulphate prep are the two oxides of copper. Prepare also the two chlorides of copper, corresponding in composition to the two oxides. APPENDIX II. OUTLINES OF SUGGESTED EXPERIMENTS ON PART I. (more difficult than those in Appendix I.). I. A and B are aqueous solutions of salts which readily give up oxygen. Find the oxidising power of A; that of B being unity. (A=Solution of potassium dichromate; B=Solution of potassium permanganate.) II. You are given solutions of barium chloride and ammonium oxalate of stated strengths. Determine the influence which variation of temperature exerts on the amount of chemical change which takes place in five minutes, when the solutions are so mixed that molecular proportions of the two salts interact. III. Determine the equivalents of the three metals A, B, and C, by finding the mass of hydrogen produced by the reaction between a weighed mass of each of the elements and excess of hydrochloric acid. (Magnesium; Aluminium; Zinc.) IV. Determine the number of c.c. of each of the three aqueous solutions of acids given which contain masses of the acids that are equivalent as regards their reactions with an alkali. (Sulphuric acid; Nitric acid; Phosphoric acid.) V. Prove by at least three roughly quantitative experiments that iron is an element and not a compound. Prove that copper oxide is a compound. |