Chemistry. — “The influence of different substances on the decom 
position of monoses by an alkah and on the inversion of cane 
sugar by hydrochloric acid.” By Prot. H. 1. Waterman and J. Groor. 
(Communicated by Prof. J. BörsEKEN.) 
(Communicated at the meeting of January 31, 1920). 
When the strength of the acid and of the alkali, from which the 
salt is formed, are known as well as the nature of the ions, we 
ean calculate the percentage of the hydrolysis. The decomposition 
of monoses by an alkali can be controlled polarimetrically, so that 
this method as well as the often used inversion of cane sugar gives 
us a sensitive means to determine the percentage of the hydrolysis.’) 
Applying the law of mass-action to the electrolytic dissociation- 
equilibria that occur in such a solution, we can calculate the hydro- 
lysis. Using 
[B] [C, H, O”] 
[C, H, OH] 
and assuming the bydrolysis to be weak and the non hydrolized 
sodium-phenolate to be perfectly dissociated, we find for 4, N sodium- 
phenolate solution, [OH’] = rather more than 3.103, 7) 
When the hydrolysis of the sodium-phenolate in a + N solution 
10 
were perfect, then [OH’| would be 10-1. From this we learn, that 
=1,3.10- and [H][OH'] =1,2.10-"4 
Kabaal ei 
100 
of the sodium-phenolate only ne 3.10? = 3. Ui vies. hydrolized. 
For more diluted solutions the percentage of this hydrolysis is higher. 
For ;4, N potassium-phenolate at 25° the hydrolysis is 3,1 °/,.°) 
_ These results are in agreement with the experiments on phenol, 
which taught that in an alkalie medium phenol practically behaves 
like a monobasic acid. 
In this way the hydrolysis of many of the compositions treated 
up till now in the above mentioned investigations could be calculated 
when only enough data were at our disposition with regard to the 
strength of the respective acids and bases expressed in the well- 
known units. 
1) H. I. WarerMAN, These Proceedings XX (1917) p. 88, 382, 581. 
2) J. WaLKER, Introduction to physical chemistry 1919, p. 330 and 336. 
