To calculate the corrosion potential of copper in a seawater environment, we can use the Nernst equation. The Nernst equation relates the reduction potential of a half-cell reaction to the standard electrode potential, temperature, and concentrations of the reactants and products.For copper, the half-cell reaction is:Cu + 2e CuThe Nernst equation is given by:E = E - RT/nF * ln Q where:E = corrosion potentialE = standard electrode potential for Cu/Cu, it is +0.34 V R = gas constant 8.314 J/mol K T = temperature in Kelvin 25C = 298 K n = number of electrons transferred for Cu/Cu, it is 2 F = Faraday's constant 96485 C/mol Q = reaction quotient, which is the ratio of the concentrations of products to reactantsIn this case, the reaction quotient Q is given by:Q = [Cu] / [Cu]Since the concentration of copper ions in seawater is given as 2.5 x 10^-5 M, we can plug this value into the Nernst equation:E = 0.34 - 8.314 * 298 / 2 * 96485 * ln 2.5 x 10^-5 / [Cu] Assuming that the concentration of solid copper [Cu] is constant and can be set to 1, the equation simplifies to:E = 0.34 - 8.314 * 298 / 2 * 96485 * ln 2.5 x 10^-5 E = 0.34 - 0.0129 * ln 2.5 x 10^-5 E 0.34 - -0.0129 * 10.6E 0.34 + 0.137E 0.477 VThe corrosion potential of copper in a seawater environment with a pH of 8.2 and a temperature of 25C is approximately 0.477 V.