OXIMIDOSULPHONATES OR SULPHAZOTATES. QJ 



the very concentrated solution be quickly evaporated cold over sul- 

 ])])nric ncirl, it is possible to o-et the (lianntinuiinii salt in good prismatic 

 crystals, very soluble in water. If instead, the solution is mixed with 

 concentrated ammonin-watei* and evaporated in an ammoniacal atmos- 

 phere over solid potassium hydroxide, crystals of another very sohible 

 salt are obtained, having- an unconquerable tendency to climb the 

 sides of the vessel and there exfoliate. These crvstals slowly effloresce 

 in the desiccator, and (^crui- in masses of overlapping flat prisms. 

 They are believed to be the ßre-sixfh s normal ammonium oximido.wîpho- 

 natr. corresponding to Fremy's basic potassium sulphazotate. 



We have no analyses to bring forward. The dinmmonium salt 

 has hydrolysed before it could he freed îvo\\\ its motlier-liquor. The 

 alkaline salt has also not been obtained in (piantity in such definite 

 form as to promise results of value from its c|uantitative analysis. 

 Heated, this salt decomposes like other oximidosulphonates suddenly, 

 and le;ives a residue of ammonium acid sulphate. 



On evaporating a solution of normal ammonium oximidosul- 

 phonate with ammonium acetate over a water- bath, ammonia escaped 

 as usual and the concentrated solution on cooling yielded a magma 

 of lustrous needles. This magma slowly drained itself dry on 

 the tile and for àr^y^ evolved strong acetic-acid vajiour without the 

 oximidosulphonate hydrolysing or the compact dry mass losing its 

 silky lustre. In the course of weeks, however, hydrolysis occurred 

 and the mass became loose opaque crystals of ammonium hydrogen 

 sulphate. It thus seems that diammonium oximidosulphonate like 

 the potassium salt combines with other salts such as ammonium acetate. 



Barium oximidosulphonates. 



Barium chloride does not precipitate a solution of dipotassium or 

 disodium oximidosuljjhonate, but the mixed solutions are very 



