4 mole of a mixture of Mohr’s salt and Fer(SO4)3 requires 500 ml of 1M K2Cr2O2 for complete oxidation in acidic medium. The mole % of the Mohr’s salt in the mixture is:

# 4 mole of a mixture of Mohr's salt and Fer(SO4)3 requires 500 ml of 1M K2Cr2O2 for complete oxidation in acidic medium. The mole % of the Mohr's salt in the mixture is:

1. A

25

2. B

50

3. C

60

4. D

75

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### Solution:

$+14{\mathrm{H}}^{+}⟶2{\mathrm{Cr}}^{3+}+6{\mathrm{Fe}}^{3+}+7{\mathrm{H}}_{2}\mathrm{O}$
Equivalent of Fe2+ = moles of Mohrs salt
= equivalent of K2Cr2O7
=500 x 10-3 x 6 x 1 = 3.0
Hence, mole per cent of Mohr's salt
$=\frac{3}{4}×100=75$

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