Question

A voltaic cell consists of a copper electrode in a solution of copper(II) ions with unknown concentration, and a palladium electrode in a 0.1 M solution of palladium(II) ions. The palladium electrode is the cathode and its reduction potential is 0.951 V, the Cu electrode is the anode. (7 points)

(a) Write the half-reaction that occurs at the anode and the cathode, as well as the overall cell reaction.

b) What is the concentration of Cu2+ ions in the anode if the cell potential is 0.584 V? What is the error in the Cu2+ concentration if the cell potential measurement has an error of ±2 mV?

(c) What is the equilibrium constant (Keq) for this reaction?