The standard reduction potential of a copper electrode in a 1 M Cu2+ solution at 25C can be found in standard reduction potential tables. For the half-reaction:Cu2+ aq + 2e- Cu s The standard reduction potential E is +0.34 V.To determine how the standard reduction potential would change if the copper concentration was changed to 0.1 M Cu2+, we can use the Nernst equation:E = E - RT/nF * ln Q Where:E = the reduction potential at the given conditionsE = the standard reduction potential +0.34 V for Cu2+/Cu R = the gas constant 8.314 J/molK T = the temperature in Kelvin 25C = 298 K n = the number of electrons transferred in the half-reaction 2 for Cu2+/Cu F = Faraday's constant 96,485 C/mol Q = the reaction quotient, which is [Cu2+]/[Cu] since Cu is a solid, its concentration is considered 1 For a 0.1 M Cu2+ solution, Q = [0.1]/[1] = 0.1. Plugging the values into the Nernst equation:E = 0.34 - 8.314 * 298 / 2 * 96485 * ln 0.1 E 0.34 + 0.0295 * log10 0.1 E 0.34 + 0.0295 * -1 E 0.34 - 0.0295E 0.3105 VSo, the reduction potential of the copper electrode in a 0.1 M Cu2+ solution at 25C would be approximately 0.3105 V.