NATURE OF SOLUTION. 611 
temperature attained. As the temperature rose no peroxide was seen till after 
the maximum was passed, when small quantities began to form. This renders 
the numbers rather high between 0° and 30°, although not very much so, as the 
formation of peroxide ceased shortly after the maximum point was passed. 
This would seem to show that the formation of peroxide is due to the decom- 
position of chlorine hydrate, and suggests hypochlorous acid as the oxidising 
agent. According to SoprERO and SELMI,* no peroxide of manganese is 
formed by passing chlorine through a solution of pure manganese chloride ; but 
evidently the formation of hydrate of chlorine, and its subsequent decomposition 
in presence of manganese chloride, causes the production of the peroxide. 
MnCl, 
t p Na,S,0, a 
— 5:0 768°6 15:0 1:6208 
— 02 21:9 2°3664 
+11 27 2:3448 
29 19°7 2:1287 
Ser 18:5 19990 
16:0 14-7 15884 
24:7 12°8 13831 
31:4 8:7 09401 
1 c.e.=0°01243 gm. iodine. 
Cadmium Chloride.—With this solution chlorine hydrate was easily formed, 
and examined undecomposed up to 8”. 
CdCl, 
t° p Na,S,0, a 
—1°5 769 57 06156 
+1:3 74 0°7992 
3°2 88 0°9509 
12:2 12"1 13068 
16:0 11°35 1:2258 
25°4 Sry 1:0476 
318 8°6 0:9288 
1 c.c.=0°01243 gm. iodine. 
Zine Chloride.—An attempt was made to estimate the solubility in solution 
of zine chloride, prepared from carbonate, but it was found that a small 
quantity of iron was present, and time did not permit purification. A few 
determinations showed the maximum to be at about 3°. 
LInthiwm Chloride.—Chlorine hydrate appeared in this solution at —5°, and 
began to decompose between —5° and —4’, disappearing completely below 0°. 
An inspection of the curve of solubility will show that chlorine dissolves in 
* Ann. Ch. Phys. [3], xxxix. 161. 
