This historic book may have numerous typos and missing text. Purchasers can download a free scanned copy of the original book (without typos) from the publisher. Not indexed. Not illustrated. 1921 Excerpt: ... in a pure state. From the chlorates, chloric acid itself can be prepared. The most convenient method consists in adding sulfuric acid to an aqueous solution of barium chlorate: Ba(C108)2 + H2S04---BaS04 + 2 HCIO8 The barium sulfate, being insoluble, separates as a white precipitate, which is removed by filtration, ...
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This historic book may have numerous typos and missing text. Purchasers can download a free scanned copy of the original book (without typos) from the publisher. Not indexed. Not illustrated. 1921 Excerpt: ... in a pure state. From the chlorates, chloric acid itself can be prepared. The most convenient method consists in adding sulfuric acid to an aqueous solution of barium chlorate: Ba(C108)2 + H2S04---BaS04 + 2 HCIO8 The barium sulfate, being insoluble, separates as a white precipitate, which is removed by filtration, leaving a solution of chloric acid. This may be concentrated until it contains 40 per cent of acid. Further concentration leads to the decomposition of the acid, forming perchloric acid, water, and chlorine dioxide. The concentrated aqueous solution of the acid is a colorless liquid and has powerful oxidizing properties. The chlorates can readily be obtained in the pure state. They are all soluble in water and ionize as follows: Potassium chlorate is perhaps the most important of these salts, being used in the preparation of oxygen and as an oxidizing agent. Preparation of hypochlorites and chlorates by electrolytic methods. It will be recalled that the electrolysis of a solution of potassium chloride or of sodium chloride results in the formation of chlorine, together with the corresponding hydroxide of the metal. It is possible to so regulate this process that the chlorine, instead of being evolved, is retained in the solution, together with the hydroxide, with which it interacts to form hypochlorite or chlorate, according to the equations given above. This method is now coming into general use for the preparation of these salts. It is possible to obtain either the hypochlorite or the chlorate by properly choosing the conditions of the electrolysis. Perchloric acid and the perchlorates. When potassium chlorate is heated, a portion of the compound changes into the perchlorate: 4 KC108--y 3 KC104 + KC1 This reaction serves as a convenient method ...
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Seller's Description:
Good. No Jacket. Hardcover. 8vo-over 7¾"-9¾" tall. Former owners name is on the first page in ink, some writing on the inside cover and on the first page, but minimal throughout the book, pretty good copy!
