A 0.2 , m aqueous solution of a weak acid (HX | vedclass

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(A) For the weak acid $HX$,the dissociation is $HX \rightleftharpoons H^+ + X^-$. Here,$n = 2$.The degree of dissociation $\alpha = 0.20$.The van't Ho

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$-0.45$

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(A) For the weak acid $HX$,the dissociation is $HX ightleftharpoons H^+ + X^-$. Here,$n = 2$.The degree of dissociation $\alpha = 0.20$.The van't Hoff factor $i = 1 + \alpha(n - 1) = 1 + 0.20(2 - 1) = 1.2$.The depression in freezing point is given by $\Delta T_f = i 	imes K_f 	imes m$.$\Delta T_f = 1.2 	imes 1.86 \, K \cdot kg \cdot mol^{-1} 	imes 0.2 \, mol \cdot kg^{-1} = 0.4464 \, K$.Since the freezing point of pure water is $0 \, ^oC$,the freezing point of the solution is $0 - 0.4464 = -0.4464 \, ^oC \approx -0.45 \, ^oC$.

$A$ $0.2 \, m$ aqueous solution of a weak acid $(HX)$ is $20 \%$ ionised. The freezing point of this solution is .......... $^oC$. ($K_f = 1.86 \, K \cdot kg \cdot mol^{-1}$ for water) :-

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$A$ $0.2 \, m$ aqueous solution of a weak acid $(HX)$ is $20 \% $ ionised. The freezing point of this solution is .............. $^o C$ (Given ${K_f} = 1.86 \, ^o C/m$ for water)

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