1. The problem statement, all variables and given/known data The solubility product for CuI(s) is 1.1 x 10^-12. Calculate the value of cell potential for the half-reaction CuI + e- => Cu + I- I find the other half reaction is Cu+ + e- => Cu E=0.52V 2. Relevant equations I use the Nernst equation to solve for the standard cell potential, then fill in E = E(cathode) - E(anode) to solve the remaining unknown. 3. The attempt at a solution Heads up I found the solution to be 0.18675 Volts through trial and error, the solutions at the back of the textbook say 0.19V. I had a hard time reasoning which is the anode/cathode. How do I find this? Is it beacuse when solving for the standard cell potential in the Nernst equation that I get E = -0.707V? Also, I'm not sure if this is an electrolytic cell or galvanic cell but does that matter when solving?