OXlMlDOîsULl'HONA'J'E« UK .SL'LPHAZUTaTES. 49 



l)e addrd in very «nuill (juaiitity fo a .solution, not too dilute, of a 

 normal alkali oximidosulphonate containing- sulphate without oceasion- 

 ing any permanent precipitate even on standing. But when the 

 alkalim'ty of the solution is ahout neutralised with hydrochloric acid, 

 the solution becomes turbid from the separation of barium sulphate. 



The purified barium or lead oximidosulphonates can be decom- 

 posed by sulphates and very completely l)y carbonates, and thus be used 

 to furnish other oximidosulphonates. The ammonium salts which can 

 be formed in this way serve in tm-n for the [)reparation of salts of 

 metals which do not unite with ammonia by evaporating their 

 solution with the oxide or hydroxide of the metal. However, the 

 oximidosulphonates obtained in this way are the more unstable ot 

 these salts and we have not pursued their examination. 



Oximidosulphonates comlnne readily with each other and with 

 other salts, a fact which will be made fully evident in the brief descrip- 

 tions which follow of the salts we have prepared. 



Sodium oximiclosul'phonates. 



Xornial sudiuiii salt, Xa3NS207,3H20. — This salt forms rhombic 

 prisms often a centimetre in length. It is strongly alkaline, soluble 

 in 1'3 parts of water at 20°, and tends to form supersaturated solutions. 

 It is only partly precipitated b}' alcohol but without decomposition, 

 and is less soluble in sodium-hydroxide solution than in water. Its 

 analysis gave — 



Calc. Found. 



Sodium 22-05 21'94 



Sulphur 20-45 20-38 



Oximide residue 9*58 9-32 



Water 17-28 17-86 



This and other oximidosulphonates were decomposed for the es- 



