Oß ART. 15— TAMEMASA HAGA. 



experiment with the potassium salt, 71*5 mol. of lead peroxide were 

 consumed per 100 mol. sodium salt. The sulphate amounted to 34 

 mol. per 100 mol. of salt used, more, that is, than in the experiments 

 with the potassium salt. The calculated quantity of sodium 

 hydroxylaminetrisulphonate was correspondingly lower, 55 mol. 

 per 100 mol. or 82*75 per cent, of the theoretically possible 

 quantity. 



Reduction of Potassium Hydroxylaminetrisulphonate by Sodium 

 Amalgam. — In the interaction between sodium amalgam and potassium 

 hydroxylaminetrisulphonate in aqueous solution, the two liquids 

 become warm and the action is soon over, if the two are well shaken 

 together. No gas is evolved, and nothing; is left in solution but the 

 two salts, sulphate and aminedisulphonate (iminosulphate). The 

 latter is easily recognisable by its separating as the very sparingly 

 soluble 2/3-normal potassium salt when the solution is nearly 

 neutralised with an acid, and also by its nearly insoluble normal 

 mercury-potassium salt (this Journ. 6, 96 ; 9, 210). But the salt was 

 also analysed quantitatively (p. 28) in order to demonstrate its nature 

 beyond question. By cautiously adding hydrochloric acid to the 

 cold solution until it has become almost neutral to methyl-orange and 

 then precipitating with barium chloride, the sulphate is partially 

 separable from the aminedisulphonate. The latter may then be estimat- 

 ed as sulphate in the filtrate after hydrolysis at 150°. In an experi- 

 ment carried out in this way upon 2*447 grams of potassium hydr- 

 oxylaminetrisulphonate, the barium sulphate was washed with cold 

 and then with hot water, ignited, and weighed. The sulphate 

 from the hydrolysed aminedisulphonate was treated as in an 

 ordinary sulphate determination. In this way determined, 34'79 per 

 cent, of the sulphur came out as sulphate and 64*88 per cent, as 

 aminedisulphonate, leaving 0*33 per cent, unaccounted foi-. In 



