To calculate the exchange current density i at the interface between a silver electrode and an aqueous solution of silver ions, we can use the Butler-Volmer equation:i = n * F * k * C_red * C_ox ^0.5where:- n is the number of electrons transferred in the redox reaction for Ag+/Ag, n = 1 - F is the Faraday constant 96485 C/mol - k is the standard rate constant- C_red is the concentration of the reduced species Ag, which is in solid form, so we assume it to be 1 - C_ox is the concentration of the oxidized species Ag+, 0.025 M To find k, we can use the Nernst equation:E = E - RT/nF * ln Q where:- E is the reduction potential at the given conditions- E is the standard reduction potential +0.80 V for Ag+/Ag - R is the gas constant 8.314 J/molK - T is the temperature in Kelvin 25C = 298.15 K - Q is the reaction quotient C_red/C_ox Since the reaction is at equilibrium, E = 0 V. Therefore, we can solve for Q:0 = 0.80 - 8.314 * 298.15 / 96485 * ln Q ln Q = 0.80 * 96485 / 8.314 * 298.15 Q = exp 0.80 * 96485 / 8.314 * 298.15 Q 1.69 * 10^6Now, we can find the concentration of Ag:C_red = Q * C_oxC_red = 1.69 * 10^6 * 0.025C_red 4.23 * 10^4Since Ag is in solid form, we assume C_red to be 1.Now, we can use the Tafel equation to find k:E = E - RT/nF * ln k 0.80 = 0 - 8.314 * 298.15 / 96485 * ln k ln k = 0.80 * 96485 / 8.314 * 298.15 k = exp 0.80 * 96485 / 8.314 * 298.15 k 1.69 * 10^6Finally, we can calculate the exchange current density:i = n * F * k * C_red * C_ox ^0.5i = 1 * 96485 * 1.69 * 10^6 * 1 * 0.025 ^0.5i 1.63 * 10^11 A/mThe exchange current density at the interface between a silver electrode and an aqueous solution of silver ions is approximately 1.63 * 10^11 A/m.