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Part II 

 (Answer five questions from Part II. Extra questions will receive no credit.) 



6. a) Give directions for making a normal solution of sulphuric acid and one of 



sodium hydroxide. 



b) Ten cubic centimeters of a normal solution of sulphuric acid requires 

 2.5 cc. of a solution of sodium hydroxide for complete neutralization. 

 Find the concentration of the solution of sodium hydroxide in grams 

 per hter. (S 32, Na 23, O 16, H 1.) 



7. The water solutions of certain substances give the following tests: What may 



be the dissolved substance in each case ? 



a) The solution turns blue litmus red and forms with silver nitrate solution 



a white precipitate insoluble in nitric acid. 



b) The solution gives a deep-red color with ammonium or potassium thio- 



cyanate (NH4CNS or KCNS), and with barium chloride solution a white 

 precipitate insoluble in hydrochloric acid. 



c) The solution gives a blue coloration with iodine. 



d) The solution colors the Bunsen flame violet and forms a brown ring when 



it is mixed with concentrated sulphuric acid and ferrous sulphate solu- 

 tion is added. 



e) The solution colors the Bunsen flame yellow and turns red Utmus blue, 



8. Calculate the molecular weight of carbon-dioxide gas from the following data, 



showing clearly every step of the calculation: 



Weight of flask filled with CO2, dry = 102 . 38 grams 



Weight of flask filled with air, dry = 101 .56 grams 



Temperature of measured gases = 0° C. 



Pressure of measured gases =770 mm. 



Volume of flask =1200cc. 



Note. — One liter of air at 0° C. and 760 mm. weighs 1 .29 grams. 



9. Outline one practical method for the preparation of each of the following 



substances: (a) nitrogen from the air, (6) carbon mono.xide, (c) calciiun 

 oxide, {d) glucose. Mention one industrial use for each of the above- 

 mentioned substances. 



10. a) What do the following terminations indicate, -ite, -ic, -ide, -ate, -oiis? 



b) What relation does the combining weight of an element bear to its atomic 

 weight ? 



11. a) Describe the laboratory preparation of ammonia and mention its most 



important properties. 



b) How can ammonia be made conmiercially from the elements ? 



c) In what way can ammonia be used in the manufacture of explosives ? 



(TfflS EXAMINATION IS CONTINUED ON PAGE 3) 



