368 Report of the Department or Chemistry of the 



phate and the following results were obtained on analysis: C = 14.98; 

 H = 2.46; P = 11.89; Ba = 31.64 per ct. 



The substance was quite soluble in cold water. It was therefore 

 rubbed up in a mortar with a small quantity of water in which the 

 greater portion dissolved. After standing over night the insoluble 

 portion was filtered off, washed in water, alcohol and ether and dried 

 in vacuum over sulphuric acid. The water-soluble portion was 

 precipitated with alcohol, filtered, washed in dilute alcohol, alcohol 

 and ether and dried in vacuum over sulphuric acid. 



After drying at 105° in vacuum over phosphorus pentoxide the 

 following results were obtained on analysis: 



The water-insoluble substance gave: C = 12.58; H = 2.02; P = 10.06; 

 Ba = 40.62 per ct. 



The water-soluble substance gave: C = 15.54; H = 2.95; P = 12.30; 

 Ba = 30.24 per ct. 



examination of the crystalline barium oxalate obtained 



from the dilute hydrochloric acid solution 



of the above barium salt. 



The substance was analyzed after drying at 105° in vacuum over 

 phosphorus pentoxide and the following result obtained: C = 6.25; 

 H = 0.81 ; P = 0.95 ; Ba = 55.32 per ct. 



The phosphorus was present in organic combination. The ash 

 was found to consist principally of barium carbonate. When some 

 of the substance was heated with concentrated sulphuric acid a gas 

 was liberated which caused a white precipitate of barium carbonate 

 when led into barium hydroxide solution. 



Judging by the analysis and reactions the crystalline substance 

 was an impure barium oxalate mixed with some of the barium salt 

 of the organic phosphoric acid. 



The crude barium salt of the organic phosphoric acid first obtained 

 contained therefore about 12 per ct. of barium oxalate. 



That the substance was barium oxalate was further confirmed by 

 the following experiments: It was recrystallized several times 

 from hot dilute hydrochloric acid by partially neutralizing with 

 ammonia. It was then transformed into silver salt as follows: the 

 barium oxalate was dissolved in a little hot dilute nitric acid, diluted 

 with water and silver nitrate added which caused a heavy white 

 granular precipitate. This was filtered off, washed in water, alcohol 

 and ether and dried in the air. This substance showed all the 

 properties of silver oxalate, viz: it was very insoluble in dilute 

 nitric acid and on heating the dry substance it exploded. It was, 

 however, not free from phosphorus. It contained 68.41 per ct. of 

 silver while silver oxalate contains 71.05 per ct. of silver. ^\ 



The balance of the barium salt was then transformed into calcium 

 oxalate and the latter was recrystallized many times from boiling 



