Textbook Problem

Consider the standard galvanic cell based on the following half-reactions:

$\begin{array}{c}{\text{Cu}}^{2+}+2{\text{e}}^{-}\to \text{Cu}\\ {\text{Ag}}^{+}+{\text{e}}^{-}\to \text{Ag}\end{array}$

The electrodes in this cell are Ag(s) and Cu(s). Does the cell potential increase. decrease. or remain the same when the following changes occur to the standard cell?

a. CuSO₄(s) is added to the copper half-cell compartment (assume no volume change).

b. NH₃(aq) is added to the copper half-cell compartment (Hint: Cu²⁺ reacts with NH₃, to form Cu(NH₃)₄²⁺(aq).]

c. NaCl(s) is added to the silver half .cell compartment (Hint: Ag⁺ reacts with Cl⁻ to form AgCl(s).]

d. Water is added to both half-cell compartments until the volume or solution is doubled.

e. The silver electrode is replaced with a platinum electrode