To calculate the corrosion potential of the stainless steel SS316 electrode in a 0.1 M NaCl solution at 25C and pH 7.2, we need to consider the Nernst equation. The Nernst equation is used to determine the potential of an electrochemical cell under non-standard conditions. The equation is as follows:E = E - RT/nF * ln Q where:E = corrosion potential under non-standard conditionsE = standard reduction potential -0.71 V for SS316 R = gas constant 8.314 J/mol K T = temperature in Kelvin 25C = 298 K n = number of electrons transferred in the redox reaction for SS316, n = 2 F = Faraday's constant 96485 C/mol Q = reaction quotient, which depends on the concentrations of the species involved in the redox reactionSince the pH of the solution is 7.2, we can calculate the concentration of H+ ions:[H+] = 10^-pH = 10^-7.2 = 6.31 x 10^-8 MNow, we need to determine the reaction quotient Q . For the corrosion of SS316 in NaCl solution, the redox reaction can be represented as:SS316 + 2H+ -> SS316 2+ + H2So, the reaction quotient Q can be expressed as:Q = [SS316 2+ ] [H2] / [SS316] [H+]^2Since we are interested in the corrosion potential, we can assume that the concentrations of SS316 and SS316 2+ are equal, and the concentration of H2 is constant. Therefore, Q can be simplified to:Q = 1 / [H+]^2Now, we can plug the values into the Nernst equation:E = -0.71 - 8.314 * 298 / 2 * 96485 * ln 1 / 6.31 x 10^-8 ^2 E = -0.71 - 0.0257 * ln 2.52 x 10^15 E -0.71 - 0.0257 * 34.62E -1.6 VSo, the corrosion potential of the stainless steel SS316 electrode in a 0.1 M NaCl solution at 25C and pH 7.2 is approximately -1.6 V vs. a standard hydrogen electrode SHE .