The Van't Hoff factor of $Ca(NO_3)_2$ is

Calculate the freezing point (in ${}^{\circ}C$) of a solution obtained by dissolving $0.1 \ g$ of potassium ferricyanide (molecular weight $= 329$) in $100 \ g$ of water. Given that $K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$.

What is the freezing point of a solution containing $8.1 \ g \ HBr$ in $100 \ g$ water,assuming the acid to be $90 \ \%$ ionised ($K_f$ for water $= 1.86 \ K \ kg \ mol^{-1}$)?

Which of the following is not a non-electrolyte?

Of the following $0.10 \ m$ aqueous solutions,which one will exhibit the largest freezing point depression?

We have three aqueous solutions of $NaCl$ labelled as $A$,$B$ and $C$ with concentrations $0.1 \ M$,$0.01 \ M$ and $0.001 \ M$,respectively. The value of van 't Hoff factor $(i)$ for these solutions will be in the order: