The solubility product for CuI(s) is 1.1x10ˉ¹². Calculate E˚ for the half reaction CuI + eˉ → Cu + Iˉ?
Question:
Answer:
For CuI Ksp = [Cu+][I-] = 1.1 x 10^-12
For the reaction CuI + e- ===> Cu + I-
E = Eo -0.0591log[I-]
For Cu+ + e- ===> Cu Eo = 0.52 V
E = 0.52 + 0.0591log[Cu+]
At equilibrium Eo -0.0591log[I-] = 0.52 + 0.0591log[Cu+]
Solving for Eo
Eo = 0.52 + 0.0591log([Cu+][I-]) = 0.52 + 0.0591 log Ksp
Thus Eo = -0.187 V
K for the half reaction is the Ksp or 1.1 x 10^-12
Now use the Nernst eqn.
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