Question

1 mole of $FeSO_{4}$ (atomic weight of $\text{Fe}$ is $\text{55} \text{.84} \, \text{g} \, \text{mol}^{- \text{1}}$ ) is oxidized to $Fe_{2}\left(\right.SO_{4}\left(\left.\right)_{3}$ . Calculate the equivalent weight of ferrous ion.

• A. 55.84
• B. 27.92
• C. 18.61
• D. 111.68

Answer 1

Answer: (A)

$\text{2} \overset{\text{+2}}{\text{Fe}} \left(\text{SO}\right)_{\text{4}} \rightarrow \text{2} \overset{\text{+3}}{\left(\text{Fe}\right)_{\text{2}}} \left(\left(\text{(SO}\right)_{\text{4}} \text{)}\right)_{\text{3}}$
Change in oxidation state per Fe atom is 1. So, equivalent weight = atomic weight.