[NYM]

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 E^o is 1.56 V. Determine [Ag⁺].


Nernst equation:
E = E^o - 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?

[LQ43]

Nernst equation:
E = E^o - 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?

recalculate using 0.0592

[NYM]

Nernst equation:
E = E^o - 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?

recalculate using 0.0592

D'oh! Thank you for pointing that out