Chapter 17, Problem 149CP

A galvanic cell is based on the following half-reactions:

In this cell, the silver compartment contains a silver electrode and excess AgCl(s) (K_sp = 1.6 × 10⁻¹⁰), and the copper compartment contains a copper electrode and [Cu²⁺] = 2.0 M.

a. Calculate the potential for this cell at 25°C.

b. Assuming 1.0 L of 2.0 M Cu²⁺ in the copper compartment, calculate the moles of NH₃ that would have to be added to give a cell potential of 0.52 Vat 25°C (assume no volume change on addition of NH₃).

$\begin{array}{cc}{\text{Cu}}^{2+}\left(aq\right)+4{\text{NH}}_3\left(aq\right)\rightleftharpoons \text{Cu}{\left({\text{NH}}_3\right)}_4{}^{2+}\left(aq\right)& K=1.0\times {10}^{13}\end{array}$