OXIMIDOSULPHONATES OR SULPH AZOTATES. g]^ 



3H2O. — Hemihvdroxv or still more ba.sic lead acetate in u'ood excess 

 of the calculated (jiiantity yields this salt in the pure state when 

 normal sodium oximidosulphonate is poured into it with stirriuir. 

 When the lead sohitiijn is poiu'ed ^-radiinlly into tlic S(xlium salt the 

 precipitate conhdns generally a little lead hydroxide, free or C(jnd)ined. 

 The salt is (^uite stahle and may he freely washed wiLli water hot ov 

 cold. It is a very vohmiinoiis tlocculent precipitate, not in the least 

 slimy or gelatinous, evidently crystalline under the microscope. The 

 reaction hy w^hich it is formed is expressed by the equati(jn — 



A^asNS.O, + 3( PbÜH)OÄc = (HO Pb)3X6,0, + 3NaO ÄI-. 



The salt can also Ije prepared, when sufticient care is taken, 1)V addin«-»- 

 to good excess of tri basic lead acetate a solution of the disodium salt. 

 The reaction then is — 



Na3NS,U, + rb3(0H)/0Ä:^),-(HüPb)3XS,0, + i>Xa0i^+lL,0. 



This lead salt decomposes when heated, as already described 

 (p. 4:'J) into sulphite and nitrite. It is soluble in acetic and other 

 acids, in sodium hydroxide, in ammonium chloride and otlier 

 ammonium salts, including ammonium oximidosulphonate. It is 

 easily and fidly decomposed in the cold b\' sodium, potassiiun. or 

 ammonium hydrogen carbonate. The last named salt gives as an 

 intermediate product a soluble lead anmionium salt (7). The results 

 of analysis agree well with calculation : — 



Calc. Found. 



Lead 67-70 67-57 



Sulphur (y[)l} CrSD 



(o) l'iro-tltiras noniial hijdwxij-lcad oxi)nidosuli>]ioi[alc, (HOPb)., 

 HNS2O;, 1I.,0. — Idemihydroxy-lead acetate added to a solution of 

 dipotassium oximidosulphonate, the latter in small excess, ^ives a 



