To calculate the corrosion potential E_corr for a silver metal electrode in a 0.1M silver nitrate AgNO3 solution of pH 5.5 and temperature 25C, we need to consider 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 often approximated by concentrations of the chemical species undergoing reduction and oxidation.For the silver metal electrode, the half-cell reaction is:Ag+ + e- Ag s The standard electrode potential E for this reaction is +0.7996 V vs. SHE.The Nernst equation is given by:E = E - RT/nF * ln Q where:E = corrosion potentialE = standard electrode potential +0.7996 V for Ag+/Ag R = gas constant 8.314 J/molK T = temperature in Kelvin 25C = 298.15 K n = number of electrons transferred 1 for Ag+/Ag F = Faraday's constant 96485 C/mol Q = reaction quotient, which is equal to [Ag+]/[Ag] for this reactionSince the silver metal electrode is in a 0.1M AgNO3 solution, the concentration of Ag+ ions is 0.1M. The concentration of Ag is not relevant in this case, as it is a solid and its activity is considered constant.Now, we can plug in the values into the Nernst equation:E = 0.7996 - 8.314 * 298.15 / 1 * 96485 * ln 0.1 E 0.7996 - 0.0257 * ln 0.1 E 0.7996 + 0.0592E 0.8588 VSo, the corrosion potential E_corr for a silver metal electrode in a 0.1M silver nitrate AgNO3 solution of pH 5.5 and temperature 25C, assuming the electrode as standard hydrogen electrode SHE reference, is approximately 0.8588 V.