What happens to the CuSO4 concentrations in the electrodes after a cell operates for some time?

In an electrochemical cell, the operation involves oxidation and reduction reactions that alter the concentration of electrolytes in the half-cells over time. In this case, as the cell operates, copper ions (Cu²⁺) from the CuSO4 solution are either deposited on the cathode (reduction) or are oxidized and dissolved back into the solution at the anode.

During the operation, as copper is reduced at the cathode, Cu²⁺ ions are consumed, leading to a decrease in concentration in that half-cell. Simultaneously, at the anode, oxidation causes an increase in Cu²⁺ ions as solid copper dissolves into the solution, increasing its concentration there. If the cell operates under equilibrium conditions, the concentrations of Cu²⁺ in both half-cells will reach a balancing point, where the rates of oxidation and reduction become equal, leading to a scenario in which their concentrations become equal over time.

This means that while concentrations may initially be different and can change throughout operation, the cell is designed to bring them to an equilibrium state. Hence, after sufficient time operating, the concentrations of CuSO4 on both sides of the cell will balance out, leading to equal concentrations in both half-cells