Consider the following concentration cell. 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

Consider the following concentration cell.M(s) | M+(satd MX) || M+(0.100 M)| M(s) Ecell = 0.417 VAt 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 isReduction: M+(0.100 M) + e- _ M(s)Oxidation: M(s) _ M+(satd MX) + e-From this information, calculate the Ksp of MX.