The molal elevation constant of water is $0.51 \ K \ kg \ mol^{-1}$. The boiling point of a $0.1 \ m$ aqueous $NaCl$ solution is approximately ......... $^oC$.

Which one of the following $0.10 \ M$ aqueous solutions will exhibit the largest freezing point depression?

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 $\text{ m}$)

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

Which of the following aqueous solutions exhibits the minimum freezing point depression upon complete dissociation?

The freezing point depression constant for water is $1.86 \, ^\circ C \, m^{-1}$. If $5.00 \, g$ of $Na_2SO_4$ is dissolved in $45.0 \, g$ of $H_2O$,the freezing point is changed by $3.82 \, ^\circ C$. Calculate the van't Hoff factor $(i)$ for $Na_2SO_4$.