Another example of a redox titration is the reaction below,
MnO,- (aq) + 5Fe2+ (aq) + 8H+(aq) → Mn2+ (aq) + 5Fe3+ (aq) + 4H2O(l)
(purple)
(colorless)
This titration can be used to estimate the amount of iron in iron suppleme
ent If it takes 29.35 mL of
0.125M MnO4 solution to titrate 35 mL of Fe2+ solution, what is the molar concen
solution?
the molar concentration of the Fe2+

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g