The relationship between the van’t Hoff factor $(i)$ and the degree of dissociation $(\alpha)$ is:

Calculate the molality of an aqueous solution of an electrolyte that freezes at $-0.93 \text{ }^\circ\text{C}$. Given that $K_f$ for water is $1.86 \text{ K kg mol}^{-1}$ and the van't Hoff factor $(i)$ is $1.25$. (Freezing point of pure water $= 0 \text{ }^\circ\text{C}$) (in $\text{ m}$)

$0.01 \ M$ solutions of glucose,phenol,and potassium chloride were prepared in water. The boiling points of these solutions follow the order:

The elevation of boiling point of $0.10 \ m$ aqueous $CrCl_{3} \cdot xNH_{3}$ solution is two times that of $0.05 \ m$ aqueous $CaCl_{2}$ solution. The value of $x$ is.........
[Assume $100 \%$ ionisation of the complex and $CaCl_{2},$ coordination number of $Cr$ as $6,$ and that all $NH_{3}$ molecules are present inside the coordination sphere $]$

Which of the following $0.05 \ M$ aqueous solution will have the lowest freezing point?

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 $1.86 \ K \ kg \ mol^{-1}$.