PEB< »XTLAMINESULPH« »NATES AND BTDR< »X V I, AM 1 NKTlilsr I, I'll« »XATK.3. 1:1 



of the salt, and ai 29 only 6.6 parts (p. 33). It info-acts in solution 

 with normal potassium sulphite and then produces hydroxylaminetri- 

 sulphonate and hydroxylaminedisulphonate, evidently in molecular 

 proportions (p. 34), this change being a fact of great theoretical import- 

 ance. Its chemical activity is manifested in oxidising certain easily 

 oxidisable substances and being thereby reduced to its parent salt, 

 hydroxylaminedisulphonate. Although it liberates iodine from hydr- 

 iodic acid, it fails to oxidise hydrochloric acid. When the latter acid in 

 concentrated solution is poured upon the solid salt, it sets up the same 

 decomposition as that which occurs spontaneously (p.15). But here, 

 as the rise of temperature is moderated, definite although minute 

 quantities of aminemonosulphonate and of hydroxylamine (not its 

 sulphonate) can be found. The salt has practically no action on 

 alcohol ; nitrous and sulphurous acids rapidly reduce it, so also does 

 sodium amalgam, first to hydroxylaminedisulphonate (as already 

 observed by Schatzman), and then this salt passes slowly but completely 

 into aminedisulphonate (iminosulphate). Clean granulated zinc slowly 

 reduces the salt, but copper does not. The spontaneous decomposition 

 of the salt may, however, easily be mistaken for its slow reduction by a 

 reducing agent, since in this case also, as will be presently described 

 (p. 16), hydroxylaminedisulphonate is produced. The difference is 

 readily detected by testing for nitrite, which is produced only in the 

 spontaneous decomposition of the salt. Manganese dioxide very slowly 

 decomposes it, causing a minute effervescence ; lead peroxide is in- 

 active. Potassium permanganate is reduced to green manganate. Clean 

 filter- pa per, unlike the paper in use in Fremy's time, does not affect it. 



Part of the instability of peroxylaminesulphonates must be 

 attributed to the presence of oxidisable impurities. Thus, Fremy 

 noticed the decomposing action of atmospheric dust; whilst nitrite, 

 another impurity liable to be found in the salt, also greatly increas- 



