Which of the following aqueous solutions should have the highest boiling point?

Calculate the amount of $KCl$ $(M_w = 74.5 \ g \ mol^{-1})$ in grams required to depress the freezing point of $1000 \ g$ of water by $2 \ K$. (Given: $K_f = 1.86 \ K \ kg \ mol^{-1}$) (in $.0$)

$A$ $0.01 \ M$ solution of $KCl$ and $BaCl_2$ is prepared in water. If the freezing point of the $KCl$ solution is $-2 \ ^\circ C$,what will be the freezing point of the $BaCl_2$ solution,assuming complete ionization?

Calculate the approximate $\Delta T_b$ (in $K$) for $0.001 \ m$ $KCl$ solution,if its van't-Hoff factor is $1.98$ [$K_b$ of water is $0.52 \ K \ kg \ mol^{-1}$].

In equimolar solutions of glucose,$NaCl$,and $BaCl_2$,the order of osmotic pressure is as follows:

$80$ mole percent of $MgCl_2$ is dissociated in aqueous solution. The vapour pressure of $1.0$ molal aqueous solution of $MgCl_2$ at $38^{\circ} C$ is $.........$ $mm$ $Hg$. (Nearest integer)
Given : Vapour pressure of water at $38^{\circ} C$ is $50$ $mm$ $Hg$.