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A $$0.2\:molal$$ aqueous solution of a weak acid $$HX$$ is $$20\%$$ ionized. The freezing point of the solutions is :
[$$k_f\,=\,1.86\:k\:kg\:mole^{-1}$$ for water]


A
0.45C
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B
0.9C
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C
0.31C
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D
0.53C
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Solution

The correct option is A $$\;-0.45^{\circ}C$$
We know, $$\Delta T_{f} = \, i K_{f}\, m$$

$$\therefore \Delta T_{f} = 1.86\times 0.2\times 1.2$$

$$\Delta T_{f} = 0.45 45^{\circ}C$$

Freezing point of the solution $$= 0 - 0.45 = - 0. 45^{\circ}C$$

Therefore, the correct option is A.

Chemistry

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