An electrochemical cell consists of a Zn electrode in 0.200 M Zn2+ (aq) and a Ag electrode in 0.100 M Ag+ (aq).
KCl (s) is added to the Ag electrode. E is measured to 1.04 V and Eo is 1.56 V. Determine [Ag+].
E = Eo - 0.059 V/2 * log ([Zn2+]/[Ag+]) =>
1.04 V = 1.56 V - 0.059V/2 * log (0.200/[Ag+]2 =>
[Ag+] = 6.87*10-10 M.
The right answer is 7.36*10-10 M. What am I doing wrong here?