Ag⁺ + E^- $\rightarrow$ Ag(s) E° = 0 $\rightarrow$ Cu(s) E° = 0

Ag⁺ + e^- $\rightarrow$ Ag(s) E° = 0.80 V
Cu²⁺ + 2e^- $\rightarrow$ Cu(s) E° = 0.34 V
In a galvanic cell, the silver compartment contains a silver electrode and excess AgCl(s) (K_sp = 1.6 * 10^-10). 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 how many moles of NH₃ would have to be added to establish the cell potential at 0.52 V at 25°C (assume no volume change on addition of NH₃).
Cu²⁺ + 4NH₃ Cu(NH₃)₄²⁺ K_f = 1.0 * 10¹³