To calculate the standard electrode potential for a silver electrode in contact with a silver ion solution of concentration 0.010 M, we can use the Nernst equation. The Nernst equation relates the reduction potential of an electrochemical reaction half-cell or full cell reaction to the standard electrode potential, temperature, and activities of the chemical species undergoing reduction and oxidation.The Nernst equation is given by:E = E - RT/nF * lnQwhere:E = electrode potentialE = standard electrode potentialR = gas constant 8.314 J/molK T = temperature in Kelvin, 298 K for room temperature n = number of electrons transferred in the half-reaction 1 for Ag+ + e- Ag F = Faraday's constant 96485 C/mol Q = reaction quotient, which is the ratio of the concentrations of the products to the reactantsFor the reduction half-equation Ag+ + e- Ag, the standard electrode potential E for silver is +0.7996 V.The reaction quotient Q for this half-reaction is given by:Q = [Ag]/[Ag+]Since the concentration of solid silver [Ag] is constant and does not affect the reaction quotient, we can simplify the equation to:Q = 1/[Ag+]The concentration of silver ions [Ag+] is given as 0.010 M. Therefore, Q = 1/0.010 = 100.Now we can plug the values into the Nernst equation:E = 0.7996 - 8.314 * 298 / 1 * 96485 * ln 100 E = 0.7996 - 0.0257 * ln 100 E = 0.7996 - 0.0257 * 4.605E 0.7996 - 0.1183E 0.6813 VThe standard electrode potential for a silver electrode in contact with a silver ion solution of concentration 0.010 M is approximately 0.6813 V.