For a cell, Cu(s) Cu ^ 2 + (0 . 001M ) | Ag ^ + (0 . 01M)|Ag(s))the...

At anode $Cu \to {Cu}^{2 +} + 2{e}^{-}$

At cathode $2{Ag}^{+} + 2{e}^{-} \to 2Ag$

Cell reaction $\to Cu + 2{Ag}^{+} \to {Cu}^{2 +} + 2Ag$

${E}_{cell} = {E}_{cell}^{0} - \dfrac{0 . 06}{2}log\dfrac{\left[{Cu}^{2 +}\right]}{{\left[{Ag}^{+}\right]}^{2}}$

$0 . 43 = {E}_{cell}^{0} - \dfrac{0 . 06}{2}log\dfrac{\left(0 . 001\right)}{{\left(0 . 01\right)}^{2}}$

${E}_{cell}^{0} = 0 . 46$

${E}_{cell}^{0} = {E}_{{Ag}^{+} / Ag}^{0} - {E}_{{Cu}^{2 +} / Cu}^{0}$

$0 . 46 = 0 . 80 - {E}_{{Cu}^{2 +} / Cu}^{0}$

${E}_{{Cu}^{2 +} / Cu}^{0} = 0 . 34$ volt

${E}_{{Cu}^{2 +} / Cu}^{0} = 34 \times {10}^{- 2}$