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 disso

Question

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 $(K_{f} = 1.86 K kg mol^{- 1})$

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Answer:

B

Solution:

Vant Hoff's factor (i) for $Na_{2} SO_{4} = 3$ $∴ Δ T_{f} = (i) k_{f} m = 3 \times 1.80 \times \frac{0.01}{1} = 0.0558 K$

TestHub · Accepted Answer

Vant Hoff's factor (i) for Na 2 ​ SO 4 ​ = 3 ∴ Δ T f ​ = ​ (i) k f ​ m = 3 × 1.80 × 1 0.01 ​ = 0.0558 K ​

Chemistry - Liquid Solution Question with Solution | TestHub

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