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. 1912 Excerpt: ...Thus Price104 found that 10 c.c. of a solution prepared from potassium hydrogen sulphate and hydrogen peroxide were equivalent to 27-8 c.c. of a thiosulphate solution on 23 May, to 27T c.c. on 15 August, and to 26-8 c.c. on 14 September. Also, a dilute solution prepared from potassium persulphate and sulphuric acid ...
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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. 1912 Excerpt: ...Thus Price104 found that 10 c.c. of a solution prepared from potassium hydrogen sulphate and hydrogen peroxide were equivalent to 27-8 c.c. of a thiosulphate solution on 23 May, to 27T c.c. on 15 August, and to 26-8 c.c. on 14 September. Also, a dilute solution prepared from potassium persulphate and sulphuric acid showed very little diminution in strength after keeping for two years, and there was no formation of hydrogen peroxide. The solution generally has a strong odour resembling that of bleaching powder %17 which is also, accompanied by that of ozone106; the impure salt obtained by Price possessed no such odour, but when dissolved the solution acquired it again after a short time. A slightly alkaline solution rapidly decomposes, but the solution is much more stable in the presence of a large excess of potassium hydroxide,106 possibly because of the formation of a dipotassium salt. Price103 noticed that in titrating the The increase in the percentage is due to the decomposition of some persulphuric acid with the formation of the permono-acid. + It should be mentioned that a dilute solution, freshly prepared from potassium persulphate and concentrated sulphuric acid, generally contains traces of hydrogen peroxide, as shown by the titanium sulphate test, but that on keeping, the hydrogen peroxide gradually disappears. % Baeyer and Villiger17 attribute this odour to the presence of a compound of the formula S.iob( = 2H2SO6-2H2O). solution with potassium hydroxide, using phenolphthalein as indicator, the colour change was not sharp, and pointed out that this was probably due to the slight acidity of the H in the-0.0H group. The concentrated solutions (92 per cent) prepared by Ahrle 101 have a strong odour of ozone and rapidly decompose at body temperature....
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Seller's Description:
This is an ex-library book and may have the usual library/used-book markings inside. This book has soft covers. In good all round condition. Please note the Image in this listing is a stock photo and may not match the covers of the actual item, 350grams, ISBN:
