A certain mass of substance in 10 g of benzene lowers the freezing point by `1.28^(@)C` and in 100 g of water lowers the freezing point by `1.395^(@)C` separately. If the substance has normal molecular weight in benzene and completely dissociated in water, calculate number of moles of ions formed by its 1 mole dissociation in water `(K_(f_("water"))=1.86, K_(f_("benzene"))=5.00)`

Explanation

To solve the problem step by step, we will use the formula for freezing point depression and apply it to both benzene and water.

### Step 1: Understand the formula for freezing point depression
The formula for freezing point depression is given by:
\[ \Delta T_f = i \cdot K_f \cdot m \]
where:
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