(1877) 
of the second metal, as has already been proved by the investigations 
of Meyer *), Richard and Lewis’) and Oee *). Therefore P, = Kv. 
The factor AK is unknown. For «—1 it becomes however = P7;. 
For small values of « however this is not necessarily the case, for 
it is to be expected that its value will be influenced by the nature 
of the first metal. 7 
The condition of equilibrium then becomes: 
uy Pil —2) A Ku 
atk Ps 
Ng Ke Use 
Vp V Ka 
or aye BN Ee C8 
ny ‘Gi ny 
Vo, VPid—a) 
: K « 
and for n,n, Ps en 
VNU: VEEN) 
In words: The ratio of the ions in the electrolyte is to that of 
the atoms in the metal as A: Py. 
When the ratio A: Py is very great, p,:p, will also be great, even 
when w has but a small value, that is to say that the electrolyte will 
contain almost exclusively cations of the baser metal even when 
the concentration of that metal in the electrode is small. 
In calculating the potential difference, the concentration of these 
Br Kye 
ions (p,) may, therefore, be taken as constant. oar i 
a logarithmic function of « and, for small values of v, will increase 
aen. dar REY 
rapidly with it. (Er ) 
Av Nn, & 
is then 
The graphic representation of this function is a curve rising rapidly 
from the potential of the nobler metal at a small distance from the 
a-axis. As wv increases, K approaches to the value P, becoming 
equal to P; when 2=1. The curve, therefore, bends sharply and 
after a small further rise reaches to the value of the potential of J/, in 
a solution of pure M,Z. 
The ratio of the ions in the coexisting electrolyte Ee increases 
| "  PitPs 
from O to nearly 1 for quite small values of wv. The curve, which 
represents a as a function of this ratio, runs, therefore, at a slight 
incline towards the ordinate representing these baser metal, finally 
approaching it almost asymptotically. 
My ay apis. Cl. 7, 417. 
Ps we) 4 „ 28, |. 
Oh Ge 
