Question

10. A sample of an iron ore is dissolved in acid, and the iron isconverted to Fe2+. The sample is then titrated with 47.20 mL of0.02240 M MnO4– solution. The oxidation-reduction reaction thatoccurs during titration is
MnO4–(aq) + 5 Fe2+(aq) + 8 H+(aq) Mn2+(aq) + 5 Fe3+(aq) + 4H2O(l)
(a) How many moles of MnO4– were added to the solution? (b) Howmany moles of Fe2+
were in the sample?
(c) How many grams of iron were in the sample? (d) If the samplehad a mass of 0.8890 g, what is the percentage of iron in thesample?