To calculate the concentration of ion X in the solution using electrochemical methods, 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.The Nernst equation is given by:E = E - RT/nF * ln Q where:E = electrode potential at any point in timeE = standard electrode potentialR = gas constant 8.314 J/molK T = temperature in Kelvin, assuming 298 K or 25C n = number of electrons transferred in the redox reactionF = Faraday's constant 96,485 C/mol Q = reaction quotient, which is the ratio of the concentrations of the products to the reactantsSince we are given the electrode potential E and the concentration of ion X, we can rearrange the Nernst equation to solve for the concentration of ion X.Let's assume that the redox reaction for ion X is as follows:X^n+ + ne- -> XThe reaction quotient Q for this reaction would be:Q = [X] / [X^n+]Now, we can plug this into the Nernst equation:0.60 V = E - RT/nF * ln [X] / [X^n+] We are given the concentration of ion X^n+ as 0.1 M, so we can plug that into the equation:0.60 V = E - RT/nF * ln [X] / 0.1 At this point, we need to know the standard electrode potential E and the number of electrons transferred n in the redox reaction to solve for the concentration of ion X. Unfortunately, without this information, we cannot determine the exact concentration of ion X in the solution.