For 0.01 M solutions of urea,NaCl,and Na_2SO | vedclass

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(C) The depression in freezing point $(\Delta T_f)$ is given by the formula $\Delta T_f = i 	imes K_f 	imes m$. Since the molality $(m)$ and the cry

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$1 : 2 : 3$

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(C) The depression in freezing point $(\Delta T_f)$ is given by the formula $\Delta T_f = i 	imes K_f 	imes m$. Since the molality $(m)$ and the cryoscopic constant $(K_f)$ are the same for all solutions,$\Delta T_f$ is directly proportional to the van't Hoff factor $(i)$. For urea (non-electrolyte),$i = 1$. For $NaCl$ (dissociates into $Na^+$ and $Cl^-$),$i = 2$. For $Na_2SO_4$ (dissociates into $2Na^+$ and $SO_4^{2-}$),$i = 3$. Thus,the ratio of depression in freezing point is $1 : 2 : 3$.

For $0.01 \ M$ solutions of urea,$NaCl$,and $Na_2SO_4$,the ratio of their depression in freezing point is .......

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