78 S. E. Moody — Hydrolysis of Ammonium Molybdate. 



ence between the value of the standard acid and the residual 

 acid is the equivalent of the acid neutralized by the ammonia 

 produced in the process of hydrolysis. The results of the 

 experiments so modified are contained in the following table. 









Table III. 







Ammo- 









HoS0 4 



Drexel 



Mean 



nium 









neutralized 



flask 



of 



molyb- 







Time 



in terms 



I 



entire 



date 



KI 



KI0 3 



in 



of I 



found 



series 



grm. 



grm. 



cm 3 



min. 



grm. 



grm. 



grm. 



0-2000 



1-0 



15 



80 



0-1213 



0-2802 " 





0-2000 



1-0 



15 



90 



0-1197 



0-2809 





0-2000 



1-0 



15 



90 



0-1195 



0-2812 





0-2000 



1-0 



15 



90 



0-1207 



0-2810 





0-2000 

 0-2000 



1-0 

 1-0 



15 

 15 



90 

 90 



0-1202 

 0-1207 



0-2807 

 0-2811 



Y 0-280 



0-2000 



1-0 



15 



90 



0-1197 



0-2810 





0-2000 



1-0 



15 



90 



0-1207 



2809 





0-2000 



1-0 



15 



90 



0-1206 



0-2810 





0-2000 



1-0 



15 



90 



0-1197 



0-2806 





Thus it appears that ammonium molybdate may be hydro- 

 lyzed completely in the presence of potassium iodide and 

 potassium iodate and that the reaction does not proceed accord- 

 ing to the equation given by Glassman. Upon boiling a mixture 

 containing the molybdate, the iodide and the iodate, ammonia 

 passes to the distillate with the iodine liberated and there acts 

 upon three-sevenths of the iodine. The apparatus described 

 makes possible the determination of the total hydrolytic action 

 of the salt, the determination of the ammonia, and, by calcula- 

 tion, the complete analysis of ammonium molybdate. A single 

 operation requires about two hours. 



University of Wisconsin, Madison. 



