In which of the following solutions are ions present?

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 $.0$)

For a given electrolyte $A_xB_y$,the relationship between the degree of dissociation '$\alpha$' and the van't Hoff factor '$i$' is ........

Which of the following $0.1 \, M$ aqueous solutions has the lowest freezing point?

$A$ $0.01 \ M$ 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?

$A$ $0.5 \ m$ aqueous solution of a weak acid $(HX)$ is $20\%$ ionized. If $K_f$ for the solvent is $1.86 \ K \ kg \ mol^{-1}$,the depression in freezing point of the solution is ..... $K$.