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\( 5.5 \mathrm{~g} \) of a mixture of \( \mathrm{FeSO}_{4} .7 \mathrm{H}_{2} \mathrm{O} \) and \( \mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3} \cdot 9 \mathrm{H}_{2} \mathrm{O} \) requires \( 5.4 \mathrm{~mL} \) of \( 0.1 \mathrm{~N} \mathrm{KMnO}_{4} \) solution for complete oxidation. Calculate the number of moles of hydrated ferric sulphate in the mixture.
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Verified Answer
The correct answer is:
0.0095
will oxidise as is present in oxidation state.
In , is already present in oxidation state, so it will not oxidise.
Hence, milliequivalents of milliequivalents of
Amount of hydrated ferric sulphate
Number of moles Mass Molar mass
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