774 
the value of 10-° of the bromine ion concentration is correct only 
in approximation. 
If we assume that the product of solubility of AgBrO, is 510, 
the concentration of the silver ions is 10-4 in 0.5 molecular KBrQ,. 
The current tension line of AgBrO, in KBrO, would not begin 
therefore before 0.57 V., and would therefore be a continuation of 
the one drawn in figure 1. 
5. Anodic formation of metal compounds in the solution. 
In the preparation of insoluble metal compounds by electrolytical 
way according to Lückow, we wish to attain that the precipitation 
does not form on the anode, but in the liquid. The conditions for 
this follow immediately from figure 5 of the first paper and from 
equation (43) 
It is clear that we shall have to work with a current density 
greater then the critical density hence: 
1.117 
engte: 
C 
The current density need only be little greater than this value 
to make all the precipitation form in the liquid. This condition 
will the sooner be satisfied as C, is smaller and d greater. That is 
to say that the concentration of the anion, which gives a precipitate 
with the metalion, must be small, and the liquid should not be 
stirred or only slightly. These are the very same conditions as 
Liickow gives for his mode of working. | 
(D,C, "he D,C,) . 
6. Electrolysis of solutions of complex salts. 
In the electrolysis of solutions of complex salts, e.g. Ag,(CN), 
dissolved in KCN, a precipitate can be formed on the anode under 
some circumstances, in this case of Ag,(CN),. 
This very greatly increases the resistance, and enfeebles the current, 
so that it is necessary to prevent the formation of this precipitate. 
It is now easy to indicate at what current density this precipitate 
will be formed. 
In a solution of Ag,(CNj, in KCN exist the equilibria: 
aE = De, 
Ag + 2CN = Ag (CN), 
and 
=. 45 a 
Ag(CN), + Ag ps Ag, (CN Jos 
ae — ae 
If we call the concentration of Ag(CN),, Ag,CN and Ag,(CN), 
C1, Gy, Gy ande, then 
’ 
1 
j 
d 
= 
