To calculate the corrosion potential for a pure iron Fe electrode in a 1 M HCl solution at 25C, we can use the Nernst equation. The Nernst equation relates the reduction potential of a half-cell at any point in time to the standard electrode potential, temperature, and reaction quotient for the redox reaction.The Nernst equation is given by:E = E - RT/nF * ln Q where:E = corrosion potentialE = standard reduction potential -0.44 V for Fe in acidic solution R = gas constant 8.314 J/molK T = temperature in Kelvin 25C = 298.15 K n = number of electrons transferred in the redox reaction 2 for Fe F = Faraday's constant 96485 C/mol Q = reaction quotientFor the redox reaction of iron in an acidic solution, the balanced half-reaction is:Fe + 2e FeThe reaction quotient Q for this reaction is given by:Q = [Fe]Since the iron electrode is pure, the concentration of Fe ions is negligible, and we can assume that Q is very close to 0. However, we cannot use 0 in the Nernst equation, as it would result in a division by zero. Instead, we can use a very small value for Q, such as 10^-6 M.Now, we can plug the values into the Nernst equation:E = -0.44 - 8.314 * 298.15 / 2 * 96485 * ln 10^-6 E -0.44 - -0.0857 E -0.3543 VTherefore, the corrosion potential for a pure iron electrode in a 1 M HCl solution at 25C is approximately -0.3543 V.