v^2 DIVERS A^'D HAGA. 



calculatioii for BaAmN(S03)2 requires 41'64 7o- ^^^^t it may, not 

 improbably from what follow«, have l^een a hydrou« salt with less 

 ammonia. 



The experiment repeated with diammoniiim imidosulphonate 

 gave ns a precipitate at first gelatinous but becoming granular on 

 standinf^". Under the microscoj'C it was seen to consist of granular 

 crystals intermixed with a very few slender needles of the tribarium 

 imidosulphonate insignificant in amount. Its alkalinity determined 

 bv decinormal acid and methyl orange showed it to be a normal salt, 

 the alkalinity being eqiT^l to one ntmn of univnlent base to two atoms 

 of sul])hur present. After hydrolysis the totnJ îimmonia, as well as 

 the sulphuric acid, was estimated. The results agree well with the 

 calculation for Ba5Am2N4(S03)8(OH2)a, a five-sixths barium salt, cor- 

 respoiidiiig, therefore, to tlie sodium amuKniium salt : — 



Calc. Found. 



Barium 43-88 43-84 



Sulphur 16-40 16-53 



Nitrogen 5-38 5-27 



It is here assumed that the observed presence of a very little 

 tribarium salt could be disregarded. The assumptiori that the pre- 

 paration was a mixture Bn3N2(SO.,)4, (OHo), + 2[I^»aAm¥(S03)2, (0E,'),_,] 

 could not possibly be admitted as in accordnuce with the microscopic 

 a]>penrnnre of the preparation. 



Jncquelain ol)l;nned, by adding diammonium imidosulphonnte to 

 a slight excess of baryta water, a precij)itate which he very fully 

 analysed, and found to be composed in accordance with the empirical 

 formula, (NH3)2(BaO)2(S03)3. Instead of this impossible formula we 

 venture to write Ba4AmN3(S03)6, (0112)3, the formula of an eight-ninths 

 bnrium nmmoniuin imidosulphonate, since the calculated numbers 

 agree still better witli his auiilysis than tliose for his formuhi 



