A galvanic cell is based on the following half reactions:
Ag+ + e2 → Ag(s) ϐo = 0.80 V Cu2+ + 2e2 → Cu(s) ϐo = 0.34 V
In this cell the silver compartment contains a silver electrode and excess AgCl(s) (Ksp = 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 25oC.
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 V at 25oC (assume no volume change on addition of NH3).
Cu2+(aq) + 4NH3(aq) ⇌ Cu(NH3)4 2+(aq) K = 1.0 × 1013