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(D) 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_

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Aluminium oxalate

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(D) 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 $i$. $A$ lower freezing point corresponds to a higher value of $i$. $1$. Potassium iodide $(KI)$: $i = 2$ $(K^+ + I^-)$. $2$. Sodium sulphate $(Na_2SO_4)$: $i = 3$ $(2Na^+ + SO_4^{2-})$. $3$. Sucrose $(C_{12}H_{22}O_{11})$: $i = 1$ (non-electrolyte). $4$. Aluminium oxalate $(Al_2(C_2O_4)_3)$: $i = 5$ $(2Al^{3+} + 3C_2O_4^{2-})$. Since Aluminium oxalate has the highest van't Hoff factor $(i = 5)$,it will cause the greatest depression in freezing point,resulting in the lowest freezing point.

Which of the following $0.05 \ M$ aqueous solution will have the lowest freezing point?

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