PEROXYLÀMINESULPHONATES AND HYDROXYLAMINETRI3ULPHONATE8. 25 



trisulphonate was only imperfectly carried out, 136*33 grams of the 

 disulphonate gave 84*33 grams of the crystalline product thai is, 

 LOO mol. gave 45*56 mol., or 68*33 per cent, of the theoretical 

 quantity. But, since the quantity of sulphate, almosl ifnol actually 

 the only other sulphur compound produced, amounted to only L9 

 mol. per 100 of disulphonate, the actual yield of trisulphonnte 

 can have been little short of 60*33 mol. per 100. The nitrite, as 

 determined by the urea method, was 28*4 mol. per 100 of disulpho- 

 nate taken. But the lead peroxide consumed was in this case 

 determined, and made out to be 71*5 mol. per 100 mol. disulphonate, 

 and this indicates the production of 31*8 mol. nitrite. Accepting 

 the mean of these numbers for the nitrite, it results that about 90 

 per cent, of the hydroxylaminedisulphonate was converted into 

 trisulphonate and nitrite, and the rest into sulphate and nitrous 

 oxide. 



In an experiment with 35 grams of potassium hydroxylamine- 

 disulphonate, in which the crystals of hydroxy laminetrisulphonate 

 were not weighed, 100 mol. yielded 13 mol. of sulphate and 2ti mol. 

 of nitrite. Calculating from these quantities, 78 per cent, of the 

 salt was oxidised into trisulphonate and nitrite, 15*5 into trisulpho- 

 nate and nitrous oxide, and 6*5 into sulphate and nitrous oxide. 

 The trisulphonate produced will therefore have been about 93*5 per 

 cent, of the calculated quantity, or 62*33 mol. per 100 mol. 

 disulphonate. 



Another experiment was made on the normal sodium hydroxyl- 

 aminedisulphonate (this Journ. 7, 49) in dilute solution, 11*33 

 grams being; taken without adding sodium hydroxide, because the 

 alkalinity of the salt was sufficient to protect it. But in this 

 experiment, only the quantities of lead peroxide consumed and of 

 sulphate formed were estimated. Exactly as happened in the 



