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

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 Tf), when 0.01 mol of sodium sulphate is dissolved in 1 kg of water, is (Kf = 1.86 K kg mol-1) (A) 0.0372 K (B) 0.0558 K (C) 0.0744 K (D) 0.0186 K

Tardigrade Admin · Accepted Answer

Vant Hoffâs factor (i) for Na2SO4 = 3 ∴ Δ Tf = (i) kf m = 3×1.80× (0.01/1) = 0.0558 K

Q. 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 $0.01 m o l$ of sodium sulphate is dissolved in $1 k g$ of water, is $(K_{f} = 1.86 K k g m o l^{- 1})$

$0.0372 K$

$0.0558 K$

$0.0744 K$

$0.0186 K$

Vant Hoff’s factor (i) for $N a_{2} S O_{4} = 3$
$∴ Δ T_{f} = (i) k_{f} m$
$= 3 \times 1.80 \times \frac{0.01}{1} = 0.0558 K$

Q. If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water (ΔTf​), when 0.01mol of sodium sulphate is dissolved in 1kg of water, is (Kf​=1.86Kkgmol−1)

0.0372K

0.0558K

0.0744K

0.0186K