5.5 g of a mixutre of `FeSO_4.7H_2O` and `Fe_2(SO_4)_3.9H_2O` requires 5.4 " mL of " `0.1 N KMnO_4` solution for complete oxidation. Calculate the number of gram moles of hydrated ferric sulphate in the mixture.

Explanation

To solve the problem step by step, we will follow the stoichiometric principles and the information provided in the question.

### Step 1: Understand the Reaction
The reaction involves the oxidation of ferrous ions (from `FeSO4.7H2O`) to ferric ions (from `Fe2(SO4)3.9H2O`) by potassium permanganate (`KMnO4`). The balanced half-reactions are:
- For `KMnO4`:
\[ \text{Mn}^{7+} + 5e^- \rightarrow \text{Mn}^{2+} \]
...