S 1. Write the balanced oxidation/reduction reaction for the reaction between MnO4 ions and HC2O4 in acidic conditions. 2. How many moles of Fe2+ ions will be oxidized by 0.043 moles of MnO4* ions? 3. Iron can be analyzed by dissolving it in acid to convert Fe(o) to Fe+ ions and then titrating the Fe+ ions with KMnO4. 1.630 g of iron ore are dissolved in an acidic solution. This solution is titrated to a pink endpoint with 27.15 mL of a 0.020 M KMnO4 solution. (a) How many moles of MnO4 ions were consumed? (b) How many moles of Fe2+ were in the iron ore sample? (c) What is the percent of iron in the iron ore sample