A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Fe2+ in acid and then titrating the Fe2+ with MnO4-. A 1.3271 g sample was dissolved in acid and then titrated with 47.02 mL of 0.03740 M KMnO4. The balanced equation is given below.8 H+(aq) + 5 Fe2+(aq) + MnO4-(aq) 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(l)Calculate the mass percent of iron in the ore. ______________ %
If all the three are modern-day at the same time in a unmarried pattern, you won't be able to derive through calculation. complete Fe and FeO could be analysed moist chemically. decision of Fe3O4, Fe2O3 and FeCO3 want area diagnosis (XRD technique) to make sure.
Moles KMnO4 0.04702 L x 0.03740 M 0.001759 Moles Fe2+ 5 x 0.001759 0.008795 Mass Fe 0.008795 mol x 55.847 g/mol 0.4912 g % 0.4912 x 100 / 1.3271 37.01
If all the three are modern-day at the same time in a unmarried pattern, you won't be able to derive through calculation. complete Fe and FeO could be analysed moist chemically. decision of Fe3O4, Fe2O3 and FeCO3 want area diagnosis (XRD technique) to make sure.
Moles KMnO4 0.04702 L x 0.03740 M 0.001759 Moles Fe2+ 5 x 0.001759 0.008795 Mass Fe 0.008795 mol x 55.847 g/mol 0.4912 g % 0.4912 x 100 / 1.3271 37.01
