To calculate the concentration of Cu2+ ions in the solution, we can use the Nernst equation, which relates the cell potential E to the standard reduction potential E and the concentrations of the species involved in the redox reaction. The Nernst equation is:E = E - RT/nF * ln Q where:E = cell potential 0.78 V E = standard reduction potential of Cu2+/Cu given R = gas constant 8.314 J/molK T = temperature 25C = 298.15 K n = number of electrons transferred in the redox reaction for Cu2+/Cu, n = 2 F = Faraday's constant 96485 C/mol Q = reaction quotient, which is the ratio of the concentrations of the products to the reactants raised to their stoichiometric coefficientsFor the Cu2+/Cu redox couple, the half-reaction is:Cu2+ + 2e- -> CuThe reaction quotient Q for this half-reaction is:Q = [Cu]/[Cu2+]Since we are looking for the concentration of Cu2+ ions, we can rewrite the Nernst equation as:0.78 V = E - RT/2F * ln [Cu]/[Cu2+] We need the standard reduction potential E for the Cu2+/Cu couple. If it is not provided, you can look it up in a standard reduction potential table. For this example, let's assume the standard reduction potential is +0.34 V.Now, we can plug in the values and solve for [Cu2+]:0.78 V = 0.34 V - 8.314 J/molK * 298.15 K / 2 * 96485 C/mol * ln [Cu]/[Cu2+] 0.44 V = - 2.303 * 10^-3 V * ln [Cu]/[Cu2+] -191.3 = ln [Cu]/[Cu2+] Now, we need to know the concentration of Cu in the solution. Since the problem states that the solution is 0.1 M CuSO4, we can assume that the concentration of Cu is negligible compared to the concentration of Cu2+ ions. Therefore, we can simplify the equation as:-191.3 = ln 1/[Cu2+] To solve for [Cu2+], we can take the exponent of both sides:[Cu2+] = e^-191.3 [Cu2+] 1.45 10^-83 MThe concentration of Cu2+ ions in the 0.1 M CuSO4 solution is approximately 1.45 10^-83 M. However, this value seems unrealistic, as it is extremely low compared to the initial concentration of CuSO4. It is possible that there is an error in the given cell potential or standard reduction potential, or that the assumptions made in the calculation are not valid for this particular system.