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(A) 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

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$K_4[Fe(CN)_6]$

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(A) 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 identical for all solutions,the boiling point depends on the van't Hoff factor $(i)$. For $K_4[Fe(CN)_6]$,$i = 5$ $(4K^+ + [Fe(CN)_6]^{4-})$. For $Na_2SO_4$,$i = 3$ $(2Na^+ + SO_4^{2-})$. For Urea,$i = 1$ (non-electrolyte). For $NaCl$,$i = 2$ $(Na^+ + Cl^-)$. Since $K_4[Fe(CN)_6]$ has the highest van't Hoff factor $(i=5)$,it will show the highest boiling point elevation and thus the highest boiling point.

Which of the following aqueous solutions has the highest boiling point,under identical conditions having a concentration of $0.03 \ m$?

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