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(D) The depression in freezing point $(\Delta T_f)$ is a colligative property,which is directly proportional to the van't Hoff factor $(i)$,where $\De

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$C_6H_{12}O_6$ (glucose)

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(D) The depression in freezing point $(\Delta T_f)$ is a colligative property,which is directly proportional to the van't Hoff factor $(i)$,where $\Delta T_f = i 	imes K_f 	imes m$. For equimolal solutions,the freezing point is highest when the depression in freezing point is minimum. This occurs when the number of particles produced in the solution is minimum. $C_6H_{12}O_6$ (glucose) is a non-electrolyte,so $i = 1$. $C_6H_5NH_3^+Cl^-$ dissociates into $2$ ions $(i = 2)$. $Ca(NO_3)_2$ dissociates into $3$ ions $(i = 3)$. $La(NO_3)_3$ dissociates into $4$ ions $(i = 4)$. Since glucose has the lowest $i$ value,it shows the minimum depression in freezing point,resulting in the highest freezing point.

The freezing point of an equimolal aqueous solution will be highest for:

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