PEROXYLÀMINESULPHONATES AM» BTDROX1 i. \ M I \ KTi; isr i,rilo\\\Tl<;s. ;;:; 



Determination of the Molecular Magnitude of Sodium Hydroxylamine- 

 trisulphonate. — Thia was carried out by Löwenherz's method with 

 melted sodium sulphate crystals (Zeit, physikal. Cheni.^ 1896, 18, 7<>) 

 :iik1 using hydrated sodium hydroxylaminetrisulphonate. Sodium 

 sulphate gets by dissolution in it of the hydrated hydroxylamine- 

 trisulphonate a liulc more water than corresponds to the hydrate with 

 1(1 molecules of water, but the crystalline sulphate separates the 

 anhydrous salt in abundance on fusion, and as the crystallising 

 temperature of the melted salt does not change as long as the anhydrous 

 salt remains at the bottom, this additional water is only equivalent t<> 

 the use of a slightly greater quantity of the crystallised salt. A correc- 

 i ion was, therefore, introduced bv calculating from this additional water 

 the corresponding quantity of hydrated sodium sulphate. 



Hydrated salt Anhydrous salt Glauber's salt Glauber's salt At M W. 



taken. correcte I 



Oj.NSaNa,- 211,0 



2*479^ 2-2411- 58*98o£ 59*411g 0*369° 332*2 



O O O O 



3*3417g 3*02l0g 56*946g 57*520g 0*510° 335*6 



O l0 XS ; X:,, requires 339.4 

 Molecular Magnitude of Normal Sodium Hydroxylaminedisul- 

 phonate. 



Hydratedsalt. Anhydrous salt. Glauber's salt Glauber's salt At M. W. 



taken. corrected. 



N a ON(S0 8 N a ) 2 .3H 2 



l*2200g l*0093g 36*818g 37*198g 0*39° 233*2 



2*4455g 2*0230g 36*442g 37*198g 0*74° 239*6 



O r NS 2 Na 3 requires 259*3 

 Solubility of Peroxylaminesulphonate in X/IO Solution of Potassium 

 Hydroxide. — The purified salt, previously washed on the porous tile 

 with some of the solvent, was shaken with il for from L5 to 20 

 minutes, the temperatur of the solution being 29°. After some time 

 5 c.c. of the clear solution were pipetted off. The rest of the solution, 

 aloii"- with the undissolved salt, was left for some hours in ice, when 



