The freezing point of equimolal aqueous solut | 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 solutions are equimolal, $m$ is constant.

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urea

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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 solutions are equimolal, $m$ is constant. $K_f$ is also constant for water. Thus, $\Delta T_f$ depends on the van't Hoff factor $(i)$. For $BaCl_2$, $i = 3$. For $Ca(NO_3)_2$, $i = 3$. For urea, $i = 1$ (as it is a non-electrolyte). For $Na_2SO_4$, $i = 3$. Since urea has the minimum value of $i$, it will have the minimum depression in freezing point $(\Delta T_f)$. Therefore, the freezing point $(T_f = T_f^0 - \Delta T_f)$ will be the highest for urea.

The freezing point of equimolal aqueous solution will be highest for

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