To calculate the corrosion potential of iron in a 0.1 M HCl solution, we can use the Nernst equation. The Nernst equation relates the reduction potential of a half-cell at any point in time to the standard electrode potential, temperature, and the activities of the chemical species involved in the redox reaction.For the Fe2+/Fe redox couple, the half-cell reaction is:Fe s Fe2+ aq + 2e-The Nernst equation for this redox couple is:E = E - RT/nF * ln Q where:E is the corrosion potentialE is the standard electrode potential -0.44 V for Fe2+/Fe R is the gas constant 8.314 J/molK T is the temperature in Kelvin 25C = 298.15 K n is the number of electrons transferred in the half-cell reaction 2 for Fe2+/Fe F is the Faraday constant 96485 C/mol Q is the reaction quotient, which is equal to [Fe2+]/[Fe] for this reactionSince the iron is in its solid form, its activity is considered to be 1. In a 0.1 M HCl solution, the concentration of H+ ions is 0.1 M. The reaction between iron and H+ ions can be represented as:Fe s + 2H+ aq Fe2+ aq + H2 g Assuming that the concentration of Fe2+ ions is negligible compared to the concentration of H+ ions, we can approximate the reaction quotient Q as:Q [Fe2+]/[Fe] [H+]/2 0.1/2 = 0.05Now we can plug the values into the Nernst equation:E = -0.44 - 8.314 * 298.15 / 2 * 96485 * ln 0.05 E -0.44 - -0.021 * ln 0.05 E -0.44 + 0.060E -0.38 VThe corrosion potential of iron in a 0.1 M HCl solution at 25C is approximately -0.38 V.Since the corrosion potential is more negative than the standard hydrogen electrode potential 0 V , there is a thermodynamic driving force for the iron to corrode in this environment. The likelihood of iron corrosion in this environment is high.