To calculate the corrosion potential of copper metal submerged in seawater at 25C with a pH level of 8.2, we will use the Nernst equation. The Nernst equation is given by:E = E - RT/nF * ln Q where:E = corrosion potentialE = standard reduction potentialR = gas constant 8.314 J/mol K T = temperature in Kelvin 25C + 273.15 = 298.15 K n = number of electrons transferred in the redox reactionF = Faraday's constant 96485 C/mol Q = reaction quotientThe redox reaction for copper in seawater is:Cu2+ + 2e- -> Cu s The standard reduction potential E for this reaction is +0.337 V. The number of electrons transferred n is 2.The reaction quotient Q can be calculated using the concentration of Cu2+ ions in seawater. The concentration of Cu2+ ions in seawater is approximately 2.3 x 10^-9 M.Now we can plug these values into the Nernst equation:E = 0.337 - 8.314 * 298.15 / 2 * 96485 * ln 2.3 x 10^-9 E = 0.337 - 0.043 / 2 * ln 2.3 x 10^-9 E = 0.337 - 0.0215 * -19.98 E = 0.337 + 0.4297E 0.767 VThe corrosion potential of copper metal submerged in seawater at 25C with a pH level of 8.2 is approximately 0.767 V.