Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr₂ in 200 g of water (Molar mass of MgBr₂ is 184 g) (K_f for water is 1.86 K kg /mol)

Q. Sodium sulphate dissolves in water with evoluation of heat. Consider a saturated solution of sodium sulphate. If the temperature is raised, then according to Le-chatelier principal

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lf sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water (ΔTf), when 0.01 mol of sodium sulphate is dissolved in 1 kg of water, is: [Kf=186 K−kgmo1−1]

The correct option is C 5.58 KNa2SO4⟶2Na++SO42−Vant Hoff's factor (i) for Na2SO4=3ΔTf=i×Kf×mΔT=3×186×0.011=5.58 KOption B is correct.

lf 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:

$[K_{f} = 186 K - k g m o 1^{- 1}]$

The correct option is C $5.58 K$
$N a_{2} S O_{4} ⟶ 2 N a^{+} + {S O}_{4}^{2 -}$

Vant Hoff's factor (i) for $N a_{2} S O_{4} = 3$

$Δ T_{f} = i \times K_{f} \times m$

$Δ T = 3 \times 186 \times \frac{0.01}{1} = 5.58 K$

Option B is correct.