no On Oxdtic Add. 



But f^r practical purposes, it is more cohvenient to con- 

 sider the acid as a constant quantity. The following table 

 js constructed upon that plan : 



Oxalate of Ammonia 



Magnesia 



• Soda 



Lime 



Potash 



' Strontian 



— Barvles 



Acid. 



100 

 J 00 

 ]00 

 100 

 ]00 

 )00 

 100 



Base. 



34-12 

 35-71 

 57-14 

 60 00 



12-2-S6 

 J51-51 

 14^-SS 



Weifjlit of 

 Salt. 



134-12 

 135-71 

 157-14 

 ICOOO 

 22iJ-86 

 251-51 

 242-86 



9. Tn the preceding utafemenf, no account has been 

 taken of the water of crystallization which might still re- 

 main attached to the salts, notwithstanding the heat to which 

 they were exposed. There i» reason to believe, however, 

 that in most of them this water must be so small, that it 

 tnay be overlooked without any great error. Oxalates of 

 soda and of ammonia, I have reason to beHeve, lose all their 

 water of cr^'stallization at a n)oderate heat. This is the case 

 also with oxalates of lime and barytes, and I presume that 

 the oxalates of strontian and magnesia are not exceptions ; 

 but oxalate of potash retains its water much more obstinate- 

 ly. I believe that in that salt the weight of acid and of base 

 is nearly equal, and that v/hen dried in the temperature of 

 212^, it still retains nearly ten per cent, of water; but I 

 have not been able to establish this opinion by direct ex- 

 periment. 



The composition of oxalate of strontian in the preceding 

 table, was so different from what T expected, that I repeated 

 the experiment ; but the result was the same. This induced 

 nie to combine strontian and oxalic acid in the following 

 manner: lop grains of a solution containing 7 grains of real 

 oxalic acid were neutralized by ammonia, and the oxalic 

 acid preci|)itatcd by means of muriate of strontian. The 

 salt obtained weighed 1"3'3 grains; of course it was com- 

 zi\ of 



Acid 



poser 



