Which of the following solutions boils at the | vedclass

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(C) $BaCl_2$ dissociates into $3$ ions $(Ba^{2+} + 2Cl^{-})$,whereas $NaCl$ dissociates into $2$ ions $(Na^{+} + Cl^{-})$. Glucose and Urea are non-el

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$0.1 \ M$ $BaCl_2$

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(C) $BaCl_2$ dissociates into $3$ ions $(Ba^{2+} + 2Cl^{-})$,whereas $NaCl$ dissociates into $2$ ions $(Na^{+} + Cl^{-})$. Glucose and Urea are non-electrolytes $(i = 1)$. Since boiling point elevation is given by $\Delta T_b = i \cdot K_b \cdot m$,the solution with the highest van't Hoff factor $(i)$ will have the highest boiling point. Comparing the values of $i$: For $BaCl_2$,$i = 3$. For $NaCl$,$i = 2$. For glucose and urea,$i = 1$. Therefore,$0.1 \ M$ $BaCl_2$ has the highest boiling point.

Column-$I$	Column-$II$
$A$. Beckmann method	$1$. Osmotic pressure
$B$. Ostwald-Walker method	$2$. Elevation in $B$.$P$.
$C$. Berkeley-Hartley method	$3$. Depression in $F$.$P$.
$D$. Landsberger method	$4$. Relative lowering of vapour pressure

Which of the following solutions boils at the highest temperature?

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