48 



E. DIVERS AND T. HAGA. 



disodium, potassium, or ammoiniim oximidosulphonate remaining in 

 solution. Silver oxide thus formed acts slowly us an oxidising agent, 

 ïriammonium oximidosulphonate added in excess to copper sulphate 

 gives a chromium-green solution, which is turned bkie hy ammonia 

 and which with excess of copper sulphate behaves as usual, yielding 

 a precipitate of copper hydroxide and leaving diammonium oximido- 

 sulphonate in solution. 



However, both the two-thirds normal and the normal salts of the 

 alkalis enter into some reactions of complete double decomposition. 

 Thus, either a two-thirds normal or a normal oximidosulphonate 

 precipitates with hydroxy-lead acetate in excess or with barium 

 hydroxide ; a noruial salt precipitates also with sufficient normal lead 

 acetate or with barium chloride ; but to seciu-e precipitation of a lead 

 salt the solutions must be dilute. The barium precipitates, too, are 

 very slightly soluble in solutions of alkali oximidosulphonates. 

 Calcium compounds yield no ]jreci[)itates, but its hydroxide forms 

 salts by decomposing the ammonium oximidosulphonates. Strontium 

 compounds give with potassium oximidosulphonates clear solutions 

 for a moment which then become tilled suddenly with a voluminous 

 silky precipitate. Fremy could get no precipitate with strontium 

 salts, n(jr Claus either, strange to say. With sodium or ammonium 

 oximidosulphonates, strontium salts do not precipitate, but in a few 

 hours the solution deposits silky crystals in large hemispherical 

 groups on the sides of the vessel. , 



The precipitates of barium, strontium, and lead salts are soluble in 

 acids and in ammonium salts including ammonium oximidosulpho- 

 nates. The lead precipitates are also soluble in sodium or potassium 

 hydroxide. 



Barium sulphate is distinctly soluble to a small extent in solutions 

 of the nc^rmal alkali oximidosulphonates. Thus, barium chloride may 



