A chemical engineer determines the mass percent of iron in an unkown iron oxide

Question

A chemical engineer determines the mass percent of iron in an unkown iron oxide sample by converting Fe2+ (aq) in acid, then titrating the Fe2+ with MnO4-(aq).The unbalanced equation is given below. H+(aq) + Fe2+(aq) + MnO4-(aq) Fe3+(aq) + Mn2+(aq) + H2O(l) Balance the net ionic equation and solve the next question. 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 1.081 g sample was dissolved in acid and then titrated with 45.0 mL of 0.0542 M MnO4. . Calculate i) the number of moles of iron in the iron oxide sample; and ii) the mass percent of iron in the iron oxide sample.

Explanation / Answer

Moles KMnO4 = 0.045 L x 0.0542 M = 0.002439
Moles Fe2+ = 1 x 0.002439 =0.002439 moles...............(i)
Mass Fe = 0.002439 mol x 55.847 g/mol =0.1362 g

% = 0.1362 x 100/1.081 =12.6%..............(ii)

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