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Question

KMnO4 reacts with ferrous sulphate according to the following equation:
MnO4+5Fe2++8H+Mn2++5Fe3++4H2O
here, 10 mL of 0.1 M KMnO4 is equivalent to [CPMT1999]

A
50 mL of 0.1 M FeSO4
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B
20 mL of 0.1 M FeSO4
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C
40 mL of 0.1 M FeSO4
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D
30 mL of 0.1 M FeSO4
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Solution

The correct option is B 50 mL of 0.1 M FeSO4
KMnO4 reacts with ferrous sulphate according to the following equation,

MnO4+5Fe2++8H+Mn2++5Fe3++4H2O

2KMnO4+10FeSO4+8H2SO4K2SO4+2MnSO4+5Fe2(SO4)3+8H2O

2 moles of KMnO4 reacts with 10 moles of FeSO4.

The number of moles of KMnO4 in 10 ml of 0.1 M =0.1×0.01=103 moles

Therefore, 103 moles KMnO4 reacts with (5×103) moles of FeSO4.

Hence, option A(50 ml of 0.1 M FeSO4=5×103 moles of FeSO4) is correct.

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