328 IiEPORT OF THE DEPARTMENT OF CHEMISTRY OF THE 



These percentages agree fairly closely with the composition cal- 

 culated for inosite hexaphosphate, viz: 



C = 10.90; H = 2.72; P = 28.18 per ct. 



To the remaining portion of the acid (about 5 c.c.) 300 c.c. of 

 alcohol was added.* The solution remained perfectly clear. The 

 alcohol was evaporated on the water-bath and the residue taken up 

 in 100 c.c. of water in which it gave a slightly cloudy solution and 

 which had a faint, aromatic odor. The acid had possibly been 

 esterified to a slight extent. It was filtered and neutralized to 

 litmus with ammonia and precipitated with silver nitrate; the 

 precipitate filtered, washed in water and dried as before. The 

 appearance of the precipitate was identical with the first one. On 

 moist litmus paper it also showed a strong acid reaction and it was 

 free from ammonia. For analysis it was dried as above. 



0.4008 gram subst. gave 0.0176 gram H 2 and 0.0600 gram C0 2 . 

 0.1481 gram subst. gave 0.1241 gram AgCl and 0.0548 gram 

 Mg 2 P 2 7 . 



Found: C = 4.08; H=0.49; P = 10.31; Ag = 63.06 per ct. 



Calculated to the free acid as before the following percentages 

 are obtained: 



C = 10.88; H = 2.84; P = 27.52 per ct. 



That the silver precipitates obtained under above conditions do 

 not represent homogeneous salts may be seen by comparing the 

 percentages found with the calculated composition of the following 

 silver salts of inosite hexaphosphate: 



C 6 H 7 24 P6Agn = 1836. 



Calculated: C = 3.92; H = 0.38; P = 10.13; Ag = 64.65 per ct. 



C 6 H 8 2 4P6Agio = 1729. 



Calculated: C = 4.16; H = 0.45; P = 10.75; Ag = 62.40 per ct. 



Judging by the analytical results the amorphous silver precipitates 

 appear to be mixtures of the above silver salts. 



*Note: Mr. Rather found that his acid preparations gave a precipitate on addition 

 of alcohol. This was no doubt due to the fact that inorganic bases had not been 

 completely removed by his method of purification; hence an acid salt of the organic 

 phosphoric acid was precipitated on the addition of alcohol. The acid prepared 

 from our purified and recrystallized barium salts is completely soluble in alcohol. 



