19(5 



Mr. M. M. Pattison Muir on 



By proceeding thus the following Table is prepared. In 



this table column I. expresses the relative affinity ^ c?rrl 



it ni Jtl 2 o<J 4 



column II. the relative affinity vr orf ; and column III. the 



relative affinity TT ! T ^ ■ 

 J H 2 N 2 6 



The relative affinities of columns I. and II. are calculated from 



the equation h—^- — , and those of column III. by dividing 

 II. into I. 1 ~ x 



(On account of the smallness of the difference v 1 — v 2 , the 

 affinities of Column III. could not be directly determined by 

 the volumetric method.) 



Table V. 

 Influence of bases upon Relative Affinities. 



Base. 



j H 2 N 2 6 

 " H 2 SO/ 



n K * cl 2 

 ' h 2 so; 



III. H * C1 s. 



H 2 N 2 O e 



Potash 



0*667 _ o . 00 

 0-333 " 



°J?67=200 



0-333 



°^ = l-88 

 0-348 



0-638 t 7P 

 0^36lT 176 



0-383 



0-591 _ 1>44 

 0"409~ i44 



0-659_ 1 . 9 



J 657 =1 . 92 



0-343 



°^U-81 

 0-356 



0-635 _ 

 0-365 



0-605_-,. 5 o 

 0^95~ 153 

 0^84 =1 Q 

 0-416 



1^=0-97 



2-00 



1-92 



rl= ' 95 



Soda 



Ammonia 



Magnesia 



Copper oxide ... 



From these results it appears that the affinity- proportion 

 H 2 S0 4 : H 2 N 2 6 and H 2 S0 4 : H 2 Cl 2 is dependent upon the 

 nature of the base, but that H 2 Cl 2 : H 2 N 2 6 is independent 

 of the base. From considerations regarding the volume- 

 changes accompanying the action of sulphuric acid upon sul- 

 phates, Ostwald shows that the whole mass of this acid is not 

 to be regarded in determining the affinity of the acid towards 

 bases, but only that part which is not converted into acid sul- 

 phate. Hence he concludes that probably the true relative 

 affinity of sulphuric acid, as that of nitric and hydrochloric 

 acids, is independent of the nature of the base neutralized. 



The influence of temperature upon the relative affinities of 

 the acids is set forth in the following Tables : — 



