Question: A quantity of 25.0mL of a solution containing both Fe2+ and Fe3+ ions is titrated with 23.0mL of 0.0200 M KMnO4 (in dilute sulfuric acid).

A quantity of 25.0mL of a solution containing both Fe2+ and Fe3+ ions is titrated with 23.0mL of 0.0200 M KMnO4 (in dilute sulfuric acid). As a result, all of the Fe2+ ions are oxidized to Fe3+ ions. Next, the solution is treated with Zn metal to convert all of the Fe3+ ions to Fe2+ ions. Finally, the solution containing only the Fe2+ ions requires 40.0mL of the same KMnO4 solution for oxidation to Fe3+. Calculate the molar concentrations of Fe2+ and Fe3+ in the original solution. The net ionic equation is

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