Calculate the amount of $KCl$ $(MW=74.5 \ g \ mol^{-1})$ required to depress the freezing point of $500 \ g$ of water by $2 \ K$ (in $g$)? $(K_f=1.86 \ K \ kg \ mol^{-1})$

Which of the following solutions has the lowest freezing point?

Which of the following has the highest boiling point?

The addition of a polar solvent to a solid electrolyte results in

An aqueous solution is prepared by dissolving $0.1 \ mol$ of an ionic salt in $1.8 \ kg$ of water at $35^{\circ} C$. The salt remains $90 \%$ dissociated in the solution. The vapour pressure of the solution is $59.724 \ mm \ Hg$. Vapor pressure of water at $35^{\circ} C$ is $60.000 \ mm \ Hg$. The number of ions present per formula unit of the ionic salt is . . . . . .

Calculate the van't Hoff factor $(i)$ of a centimolar solution of potassium ferrocyanide $(K_4[Fe(CN)_6])$ if it is $60\%$ dissociated at $300\text{ K}$.