A sample of an iron ore is dissolved in acid, and the iron is oxidized to Fe^2. The iron (II) ion is then titrated with 47.20 ml of 0.02240 M MnO4^– solution. The redox reaction that occured is as follows:MnO4^– + 5Fe^2 + 8H^+ -----gt; Mn^2 + 5Fe^3 + 4H2O ^–a. How many grams of iron were in the sample ?b. If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample ?This is a homework problem, and I have a quiz tomorrow. Can you please explain to me how to solve this problem?
MnO4{-} + 5 Fe{2+} + 8 H{+} → Mn{2+} + 5 Fe{3+} + 4 H2O a. (0.04720 L) x (0.02240 mol/L MnO4{-}) x (5 mol Fe / 1 mol MnO4{-}) x (55.8452 g Fe/mol) 0.2952 g Fe b. (0.2952 g) / (0.8890 g) 0.3321 33.21% Fe
