If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water ( T_f - Chemistry MCQ AIEEE 2026 | ExamTest.live

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

Solution & Step-by-step Explanation

Sodium sulphate (Na_{2} SO_{4}) dissociates as: Na_{2} SO_{4} \to 2 Na^{+} + SO_{4}^{2 -} Van't Hoff factor i = 3 .Molality m = \frac{0.01 mol}{1 kg} = 0.01 m . Δ T_{f} = i \cdot K_{f} \cdot m Δ T_{f} = 3 \times 1.86 \times 0.01 = 0.0558 K

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

0.0372 K

0.0558 K

0.0744 K

0.0186 K

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