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Q.

When 9.45g of $C l C H_{2} C O O H$ is added to 500ml of water; it’s freezing point drops by ${0.5}^{o} C .$
The dissociation constant of $C l C H_{2} C O O H$ is $x \times 10^{- 3} .$ The value of $x$ is_____ $[K_{f} (H_{2} O) = 1.86 K k g m o l^{- 1}]$

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Detailed Solution

Given $Δ T_{f} = {0.5}^{o} C, K_{f} = 1.86 K k g / m o l$

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When 9.45g of ClCH2COOH is added to 500ml of water; it’s freezing point drops by 0.5oC. The dissociation constant of ClCH2COOH is x×10−3. The value of x is_____ [Kf(H2O)=1.86K kg mol−1]