Among the following 0.1 m aqueous solutions, | vedclass

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(D) The boiling point elevation is given by the formula $\Delta T_{b} = i 	imes K_{b} 	imes m$. Since the molality $(m)$ and the ebullioscopic const

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Sodium chloride

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(D) The boiling point elevation is given by the formula $\Delta T_{b} = i 	imes K_{b} 	imes m$. Since the molality $(m)$ and the ebullioscopic constant $(K_{b})$ are the same for all solutions,$\Delta T_{b} \propto i$,where $i$ is the van't Hoff factor.For complete ionization:$(A)$ $AlCl_3 ightarrow Al^{3+} + 3Cl^-$,so $i = 4$.$(B)$ $Al_2(SO_4)_3 ightarrow 2Al^{3+} + 3SO_4^{2-}$,so $i = 5$.$(C)$ $K_2SO_4 ightarrow 2K^+ + SO_4^{2-}$,so $i = 3$.$(D)$ $NaCl ightarrow Na^+ + Cl^-$,so $i = 2$.The solution with the lowest $i$ value will exhibit the lowest boiling point elevation. Thus,$NaCl$ has the lowest boiling point elevation.

Among the following $0.1 \ m$ aqueous solutions,which one will exhibit the lowest boiling point elevation,assuming complete ionization of the compound in solution?

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