A sample of an iron ore is dissolved in acid, and the iron is converted to Fe^2. The sample is then titrated with 47.20 ml of 0.02240 M MnO_4 solution. The oxidation-reduction reaction that occured during titration is as follows:MnO_4(aq) + 5Fe^2(aq) + 8H^+(aq) -----gt; Mn^2(aq) + 5Fe^3(aq) + 4H_2O(l)a. How Many moles of MnO_4 were added to the solution ?b. How many moles of Fe^2 were in the sample ?c. How many grams of iron were in the sample ?d. If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample ?
