The depression in freezing point of a solutio | vedclass

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(C) The depression in freezing point is given by the formula: $\Delta T_f = i 	imes K_f 	imes m$. Since the molality $(m = 0.01 \ mol \ kg^{-1})$ is

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Carbon tetrachloride $(31.8)$

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(C) The depression in freezing point is given by the formula: $\Delta T_f = i 	imes K_f 	imes m$. Since the molality $(m = 0.01 \ mol \ kg^{-1})$ is constant and the van't Hoff factor $(i)$ is $1$ for non-electrolytic solutes in these solvents,the depression in freezing point is directly proportional to the cryoscopic constant $(K_f)$: $\Delta T_f \propto K_f$. Comparing the given $K_f$ values: Water: $1.86$ Benzene: $5.12$ Carbon tetrachloride: $31.8$ Cyclohexane: $20.0$ Since carbon tetrachloride has the highest $K_f$ value $(31.8)$,the depression in freezing point will be the highest for this solvent.

The depression in freezing point of a solution of molality $0.01 \ mol \ kg^{-1}$ is highest with respect to which of the following solvents? (The $K_f$ value is given in brackets)

Similar Questions

Which of the following solutions exhibits the highest freezing point depression?

Calculate $\Delta T_f$ of $0.15 \ m$ solution of nonvolatile solute $\left[K_f = 1.5 \ K \ kg \ mol^{-1}\right]$ (in $K$)

Which of the following aqueous solutions has the highest freezing point?

Calculate the cryoscopic constant $(K_f)$ of a solvent if the depression in freezing point of a $0.4 \ m$ solution of a non-volatile solute is $1.8 \ K$.

Give the unit of $K_f$.

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