The quantitative relationship between electrolyte concentration
and cell potential is given by the following Nernst
Equation:Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â
Ecell = Eocell - (RT/nF)
lnQ;Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â
Ecell is cell potential under non-standard
conditions, while Eocell is cell potential
under standard conditions (calculated from standard reduction
potentials), R = 8.314 J/(mol.K), F = 96,485 C/mol, is the
Faraday’s constant; Q is the reaction quotient.
For the given half cell Ag+ + e- = Ag,
Q = 1/ [Ag+] , Eocell = 0.80V,
T= 312K, n=1
Ecell = Eocell - (RT/nF)
lnQ;
       = 0.8 -
(8.314)(312)/96500 [ln(1/ [Ag+] )]
0.01323 v = 0.8v - 0.0268[ln(1/[X])
    [log(1/[X]) = 29.4
       1/x =
10-29.4
         X
= 1/10-29.4
              Â
