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Depression in Freezing Point

1.00 g of a n...

Question

1.00 g of a non-electrolyte solute $(m o l a r m a s s 250 g m o l^{- 1})$ was dissolved in 51.2 g of benzene. If the freezing point depression constant, $k_{f}$ of benzene is 5.12 K kg mol^{-1}\), the freezing point of benzene will be lowered by

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Solution

From the relation, we have
$Δ T_{f} = k_{f} \times W_{2} \times \frac{1000}{W_{1}} \times M_{2}$

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