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A concentration cell consists of two half-cells with identical electrodes but different ion concentrations. Consider the following concentration cell (pictured below). M(s) | M*(satd MX) || M*(0.100 M) M(s) Ecell = 0.417 V At the anode, a metal electrode (M) is placed in a saturated aqueous solution containing ions of the same metal (M) and a halogen (X), MX. At the cathode, a second electrode of the same metal (M) is placed in a solution with [M*] = 0.100 M.The two half-cells are connected by a salt bridge, and the measured cell voltage is 0.417 V. The cell reaction occurring in this concentration cell is Reduction: M*(0.100 M) + e M(s) Oxidation: M(s) M*(satd MX) + e From this information, calculate the Ksp of MX.