508 
PROFESSOR J. J. THOMSON ON SOME APPLICATIONS OF 
n 
y 
r 
y 
8 
1-93 
28-1 
4 
2-89 
28'9 
2 
2-90 
13-05 
1 
3A7 
6-8 
1 
2 
4-1 
3-2 
1 
4 
4-1 
1-0 
It is evident from the above Table that, except when the amount of nitric acid 
originally present is very small, the second equation, which requires y to be constant, 
does not agree with the experiments, while the first, which requires y to be constant, 
does agree fairly well, except in those cases where the quantity of nitric acid present 
is originally small. 
Hence we conclude that, except in these cases, the molecule and the equivalent 
coincide, that is, the molecule of nitric acid in the solution is represented by H 3 N 3 0 6 ; 
a similar conclusion applies to tire molecule of sodium nitrate, the molecule of which 
in the solution has to be represented by Na 3 N 3 0 6 . When the quantity of nitric acid 
initially present is very small, the second equation seems to agree with the experiments 
better than the first, so that it might seem as if, when the quantity of nitric acid was 
very small, the molecule was HN0 3 and not H 3 N 3 0 6 ; but, as in this case a very 
small error in the experiments would make a large error in y or y', too much weight 
must not be attached to it. It seems quite possible that there are molecules of both 
types, and that in concentrated solutions those of the type H 3 1S1 3 0 6 are by far the 
most numerous. 
Cases when one or more of the Reagents are insoluble . 
§ 13. Let us suppose that A is insoluble; then for A the positional part of the 
kinetic energy equals 
a dp 
n — V 
a de ’ 
where dp/oO is the mean value of bp/b9 (v constant), and v is the volume. If <x be 
the density of A, we may write this 
ffip m iP% 
6 W~' 
Hence L for the system equals 
a I bp 
\be 
Po'Q 
+ m 2 <l c 2l + K ^ lo g^ + m s rc d + Krt log ^ + m+sc+e + Kselo ; 
"Q 
(7 
Po"Q 
mp'e 
— IV. 
