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Question

5 moles of a mixture of FeSO4 and Fe2(SO4)3 required 150 mL of 1.0 M KMnO4 in acidic medium for the complete neutralisation. Calculate the mole fraction of FeSO4 in the initial mixture.

A
0.2
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B
0.33
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C
1.5
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D
0.15
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Solution

The correct option is D 0.15
As we know, MnO4 will only oxidise Fe2+ not Fe3+.
+7MnO4++2Fe2+H++2Mn2+++3Fe3+

nf=(|Change in O.S.|)×Number of atoms
nfMnO4=|+2(+7)|×1=5
nfFe2+=|+3(+2)|×1=1

From the law of equivalence,
Equivalents of Fe2+=Equivalents of MnO4
nFe2+×1=1.0×150×51000
nFe2+=0.75 mol
Mole fraction of FeSO4=Mole fraction of Fe2+=0.755=0.15

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