332 Eepokt of the Department of Chemistry of the 



soluble to a considerable extent in cold water. On moist litmus 

 paper it shows a strong acid reaction. Heated with hydrochloric 

 acid and phloroglucine, no appreciable color reaction developed. 

 After boiling with dilute sulphuric acid for several minutes, filtering 

 and neutralizing, it did not reduce Fehling's solution. It contained 

 neither nitrogen nor sulphur and gave no reaction for chlorides. 

 Dissolved in dilute nitric acid it gave no reaction with ammonium 

 molybdate even after being kept at a temperature of 65° for some 

 time and standing at room temperature for several days, showing 

 that inorganic phosphates were absent. Bases, other than barium, 

 could not be detected in 0.5 gram of the substance. 



Owing to loss in purification the yield is rather unsatisfactory. 

 In one case 13 grams were obtained from 5 kg. of oats; in another 

 case 20 grams were obtained from 10 kg. In all, four preparations 

 were made, which gave a total of about 140 grams of the barium 

 salt. 



Much time was expended in an endeavor to obtain the substance 

 in crystalline form but as already mentioned it showed no tendency 

 whatever to crystallize. The amorphous preparations were therefore 

 analyzed after previous drying to constant weight at 105° in vacuum 

 over phosphorus pentoxide. The following results were obtained: 



1st preparation: C = 8.84; H = 1.67; P = 15.88; Ba = 36.72 

 per ct. 



2d preparation: C = 8.27; H = 1.47; P = 16.28; Ba = 37.26 

 per ct. 



3d preparation: C = 8.37; H = 1.60; P = 16.48; Ba = 36.79 

 per ct. 



4th preparation: C = 8.44; H = 1.61; P = 16.35; Ba = 36.61 

 per ct. 



These results are fairly concordant but the composition differs 

 considerably from that required for tribarium phytate. Calculated 

 for C 6 H 18 2 7P6Ba 3 : C = 6.42; H = 1.60; P = 16.60; Ba = 36.78 

 per ct. 



further purification of the barium salt. 

 In order to determine whether the composition of the substance 

 would change on further treatment, the following experiment was 

 tried. A portion of the first preparation was used. The barium 

 was precipitated with slight excess of sulphuric acid, the barium 

 sulphate filtered off and the filtrate precipitated with excess of copper 

 acetate. The copper salt was filtered and thoroughly washed in 

 water and then suspended in water and decomposed with hydrogen 

 sulphide. After removing the copper sulphide, the filtrate was 

 boiled to expel hydrogen sulphide and then precipitated with a 

 solution of recrystallized barium hydroxide. Dilute hydrochloric 



