A sample of
an iron ore is dissolved in acid, and the iron is converted to Fe2+. The sample is then titrated with 47.20 mL of
0.02240 M
MnO4- solution. The oxidation-reduction reaction
that occurs during titration is
MnO4-(aq) + 5 Fe2+(aq) + 8 H+(aq)
→ Mn2+(aq) + 5 Fe3+(aq) + 4 H2O(l)
(a) How many moles of
MnO4- were added to the solution?
(b) How many moles of
Fe2+ 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?