If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution , the change in freezing point of water `(DeltaT_(f))` when `0.01` mole of sodium sulphate is dissociated in 1 kg of water is : (`K_(f) = 1.86` K kg `mol^(-1)`)

Options

A. 0.0372K
B. 0.0558K
C. 0.0744 K
D. 0.0186 K

Explanation

To solve the problem of determining the change in freezing point of water when 0.01 moles of sodium sulfate (Na₂SO₄) is dissolved in 1 kg of water, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the dissociation of sodium sulfate:**
Sodium sulfate dissociates in water according to the following reaction:
\[
\text{Na}_2\text{SO}_4 \rightarrow 2\text{Na}^+ + \text{SO}_4^{2-}
...