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Question

A 5g sample containing Fe3O4(FeO+Fe2O3) and an inert impurity is treated with excess of KI solution in the presence of dilute H2SO4. The entire iron converted to Ferrous ion along with the liberation of Iodine. The resulting solution is diluted to 100 mL. 20 mL of the diluted solution requires 10mLof0.5MNa2S2O3 solution to reduce the iodine present. Calculate approximate percentage of Fe2O3?

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Solution

Let the moles of Fe3O4 is x.So mole of Fe2O3(in Fe3O4)=x
eq of Fe2O3(in Fe3O4)=eq of KI=eq of I2=eq of Na2S2O3.
or 2x=0.025
orx=0.0125molofFe2O3
So mass of Fe2O3=0.0125×160=2g
% ofFe2O3=25×100=40%

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