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Question

Fe2+ as well as HNO2 can be used to estimate MnO4 in acidic medium. If 100 mL of 1 M Fe2+ can be oxidised by V mL of 1 M MnO4/H+ solution, calculate volume of 1 M HNO2 that can be oxidises by VmL of 1 M MnO4/H+ solution.

A
40mL
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B
25mL
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C
50mL
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D
none of these
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Solution

The correct option is B 50mL
The balanced chemical equations are as shown.
10FeSO4+2KMnO4+8H2SO45Fe2(SO4)3+8H2O+K2SO4+2MnSO45HNO2+2KMnO4+3H2SO42MnSO4+5HNO3+K2SO4+3H2O
From above equations, we can say that 10 mole FeSO4= 5 mole HNO2
or 2 mole FeSO4= 1 mole HNO2
Since same volume and same concentration of KMnO4 is used for titration of Fe2+ ions and HNO2, the volume of HNO2 required will be 100mL×1M2moleFe2+1moleHNO2×1M=50mL

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