136 
Now we imagine the case that the metal is so rapidly dissolved 
anodically or in another way, that the reaction 
MM" + v6 
does not proceed rapidly enough to supply the abducted electrons | 
aud metal ions, so that the metal gets poorer in these two electrical 
components. If we now consider that the electrons and the metal 
ions always neutralize each other electrically, with the exception of 
only an exceedingly small fraction, then a closer examination of 
equation (14) gives the following conclusion. 
Suppose that the metal ion concentration in the metal (M'S) becomes 
n-times smaller by anodic solution ete., then the electron concen- 
tration (@s) also becomes „-times smaller, so that the numerator of 
(14) will become »’+! times smaller in consequence of this. 
If we further assume, what is allowed for a sufficient quantity 
of solution, that the ion concentration (7) is constant in the coexis- 
ting electrolyte, (97) will have to become n’+! times as small, 
from which it appears that the electron concentration in the coexisting 
electrolyte (AL) will decrease to a greater extent than that in the metal (Os). 
From equation 
A=— oa ln Kise. (Ms) aT TET ie Beense ND 
vil (M7) 
follows that when (M$) becomes smaller, and (J/7) remains constant, 
the potential difference will become less negative or greater positive. 
When (MS) decreases, the result is — as we have seen just now — 
(As) : 
that (1) becomes yreater, from which appears in connection with 
L 
the formula: 
EE OE Me oR 
Pe ten 
that the potential difference will become less negative or greater positive. 
As was already set forth at length in the preceding communica- 
tion in the discussion of a univalent metal, this points to the possi- 
bility of anodic polarisation and passivity, while perfectly analogous 
considerations lead to the cathodic polarisation. 
These phenomena must then be explained by a too slow esta- 
blishment of the internal equilibrium between metal atoms, metal 
ions, and electrons. 
5. The metal contains ions of different valency. 
We shall now suppose that ions of different valency occur in the 
metal, viz. the ions M*“ and M*. 
