At 25°C, the solubility product of CuCl is 2.0 × 10^–7 and E°_Cl–\|CuCl\|Cu is 0.128 V. The value of — Electrochemistry Chemistry Question

💡 Solution & Explanation

The standard potential of a metal-insoluble salt electrode is related to its metal ion reduction potential by: $E^\circ_{Cl^-\|CuCl\|Cu} = E^\circ_{Cu^+\|Cu} + \frac{0.0591}{1} \log K_{sp}$. Substituting values: $0.128 = E^\circ_{Cu^+\|Cu} + 0.06 \log(2.0 \times 10^{-7})$. Since $\log(2 \times 10^{-7}) = 0.3 - 7 = -6.7$, the term is $0.06 \times (-6.7) = -0.402$ V. Thus, $0.128 = E^\circ_{Cu^+\|Cu} - 0.402$, giving $E^\circ_{Cu^+\|Cu} = 0.530$ V.