Which of the following has the lowest freezin | vedclass

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

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$0.1 \ M$ aqueous solution of $NaCl$

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(B) The freezing point depression 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,the freezing point depends on the van't Hoff factor $(i)$. Lower freezing point corresponds to a higher value of $i$. For glucose and urea,$i = 1$. For $NaCl$,$i = 2$ $(NaCl ightarrow Na^+ + Cl^-)$. For $ZnSO_4$,$i = 2$ $(ZnSO_4 ightarrow Zn^{2+} + SO_4^{2-})$. However,$NaCl$ is a strong electrolyte with a higher degree of dissociation compared to $ZnSO_4$ in this concentration range,leading to a greater depression in freezing point. Thus,the $0.1 \ M$ aqueous solution of $NaCl$ has the lowest freezing point.

Which of the following has the lowest freezing point?

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