(D) The correct answer is $(d)$.Freezing point depression $(\Delta T_f)$ is a colligative property given by $\Delta T_f = K_f \times m$,where $K_f$ is

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Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression.

(D) The correct answer is $(d)$.Freezing point depression $(\Delta T_f)$ is a colligative property given by $\Delta T_f = K_f \times m$,where $K_f$ is the cryoscopic constant of the solvent and $m$ is the molality.Since $K_f$ is a characteristic property of the solvent,it varies from one solvent to another.Therefore,even if the molality $(m)$ is the same,the freezing point depression will differ if the solvents are different.

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Which one of the following statements is $FALSE$?

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A
The correct order of osmotic pressure for $0.01 \ M$ aqueous solution of each compound is $BaCl_2 > KCl > CH_3COOH >$ sucrose.
B
The osmotic pressure $(\pi)$ of a solution is given by the equation $\pi = MRT$ where $M$ is the molarity of the solution.
C
Raoult's law states that the vapour pressure of a component over a solution is proportional to its mole fraction.
D
Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression.

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Statement $1$: The cold pack used by athletes to treat injuries on the field works by dissolving a solute in water,which causes the temperature to decrease. Statement $2$: Adding a non-volatile solute to a solvent decreases its freezing point.

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After adding a solute,the freezing point of the solution decreases to $-0.186 \ ^{\circ}C$. Calculate $\Delta T_b$ if $K_f = 1.86 \ K \ kg \ mol^{-1}$ and $K_b = 0.521 \ K \ kg \ mol^{-1}$. (Assume the freezing point of pure solvent is $0 \ ^{\circ}C$)

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Pick the correct statement.

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$PbCl_2$ is dissolved in water to make its saturated solution. What will be the freezing point of this solution?
Given: $K_f (H_2O) = 2 \ K \ kg \ mol^{-1}$,$K_{sp} (PbCl_2) = 4 \times 10^{-6}$
(Assume molarity to be equal to molality) $..... ^oC$

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$A$ liquid freezes at $7^{\circ} C$ and boils at $77^{\circ} C$. If $K_{f}$ and $K_{b}$ values for the liquid are $5.6$ and $2.5 \ ^{\circ} C \ kg \ mol^{-1}$ respectively,then the ratio of latent heat of vaporisation of the liquid to the latent heat of fusion is $:-$

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Which one of the following statements is $FALSE$?

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Statement $1$: The cold pack used by athletes to treat injuries on the field works by dissolving a solute in water,which causes the temperature to decrease. Statement $2$: Adding a non-volatile solute to a solvent decreases its freezing point.

After adding a solute,the freezing point of the solution decreases to $-0.186 \ ^{\circ}C$. Calculate $\Delta T_b$ if $K_f = 1.86 \ K \ kg \ mol^{-1}$ and $K_b = 0.521 \ K \ kg \ mol^{-1}$. (Assume the freezing point of pure solvent is $0 \ ^{\circ}C$)

Pick the correct statement.

$PbCl_2$ is dissolved in water to make its saturated solution. What will be the freezing point of this solution?Given: $K_f (H_2O) = 2 \ K \ kg \ mol^{-1}$,$K_{sp} (PbCl_2) = 4 \times 10^{-6}$(Assume molarity to be equal to molality) $..... ^oC$

$A$ liquid freezes at $7^{\circ} C$ and boils at $77^{\circ} C$. If $K_{f}$ and $K_{b}$ values for the liquid are $5.6$ and $2.5 \ ^{\circ} C \ kg \ mol^{-1}$ respectively,then the ratio of latent heat of vaporisation of the liquid to the latent heat of fusion is $:-$

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$PbCl_2$ is dissolved in water to make its saturated solution. What will be the freezing point of this solution?
Given: $K_f (H_2O) = 2 \ K \ kg \ mol^{-1}$,$K_{sp} (PbCl_2) = 4 \times 10^{-6}$
(Assume molarity to be equal to molality) $..... ^oC$