To calculate the standard potential of a silver electrode in a 0.1 M silver nitrate solution at 25C, we can use the Nernst equation:E = E - RT/nF * ln Q Where:E = the potential of the electrodeE = the standard reduction potential of the half-reactionR = the gas constant 8.314 J/molK T = the temperature in Kelvin 25C + 273.15 = 298.15 K n = the number of electrons transferred in the half-reaction 1 for Ag F = Faraday's constant 96,485 C/mol Q = the reaction quotient, which is the ratio of the concentrations of the products to the reactantsFor the given half-reaction, Ag aq + e Ag s , the standard reduction potential E of silver is +0.7996 V.The reaction quotient Q can be calculated as follows:Q = [Ag s ] / [Ag aq ]Since the concentration of a solid Ag is considered to be constant and equal to 1, the reaction quotient becomes:Q = 1 / [Ag aq ]Given that the silver nitrate solution is 0.1 M, the concentration of Ag ions is also 0.1 M:Q = 1 / 0.1 = 10Now, we can plug all the values into the Nernst equation:E = 0.7996 - 8.314 * 298.15 / 1 * 96,485 * ln 10 E = 0.7996 - 0.0257 * ln 10 E = 0.7996 - 0.0257 * 2.303E 0.7996 - 0.0592E 0.7404 VTherefore, the standard potential of a silver electrode in a 0.1 M silver nitrate solution at 25C is approximately 0.7404 V.