Which of the following 0.05 , M aqueous solut | vedclass

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

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Aluminium oxalate

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(D) The depression in freezing point is given by the formula $\Delta T_f = i 	imes K_f 	imes m$. Since the molality $(m)$ and the freezing point depression 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 $\Delta T_f$,which means a higher value of $i$. Let us calculate $i$ for each solute: $1$. Potassium iodide $(KI)$: $KI ightarrow K^+ + I^-$,so $i = 2$. $2$. Sodium sulphate $(Na_2SO_4)$: $Na_2SO_4 ightarrow 2Na^+ + SO_4^{2-}$,so $i = 3$. $3$. Sucrose $(C_{12}H_{22}O_{11})$: Non-electrolyte,so $i = 1$. $4$. Aluminium oxalate $(Al_2(C_2O_4)_3)$: $Al_2(C_2O_4)_3 ightarrow 2Al^{3+} + 3C_2O_4^{2-}$,so $i = 5$. Since Aluminium oxalate has the highest van't Hoff factor $(i = 5)$,it will have the maximum depression in freezing point and thus the lowest freezing point.

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

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