In the electrolysis of a concentrated solution containing H\(^+\), Cu\(^{2+}\), OH\(^-\) and Cl\(^-\) ions using platinum electrodes, the Cu\(^{2+}\) ions will be discharged at the cathode. During electrolysis, ions migrate towards the oppositely charged electrode. Positive ions (cations) like H\(^+\) and Cu\(^{2+}\) will be attracted to the negative electrode (cathode). At the cathode, the ion that is easier to reduce (requires less energy to gain electrons) will be discharged first. In this case, Cu\(^{2+}\) ions are more easily reduced to Cu(s) than H\(^+\) ions are to H\(_2\)(g). The reaction at the cathode will be the reduction of Cu\(^{2+}\) ions: Cu\(^{2+}\)(aq) + 2e\(^-\) → Cu(s). Anode reaction: The reaction at the anode will be the oxidation of water: 2H\(_2\)O(l) → O\(_2\)(g) + 4H\(^+\)(aq) + 4e-