The freezing point depression constant for water is $1.86 ^\circ\text{C m}^{-1}$. If $5.00 \text{ g}$ $Na_2SO_4$ is dissolved in $45.0 \text{ g}$ $H_2O$, the freezing point is changed by $-3.82 ^\circ\text{C}$. The Van’t Hoff factor for $Na_2SO_4$ is:

Isotonic solutions have the same:

A solution containing $10 \text{ g/dm}^3$ of urea (molecular mass $= 60 \text{ g mol}^{-1}$) is isotonic with a $5 \%$ solution of a non-volatile solute. The molecular mass of this non-volatile solute is:

Which colligative property provides the most accurate method for determining the molecular weight of proteins and polymers?

The vapour pressure of a solvent decreased by 10 mm of Hg when a non-volatile solute was added to the solvent. The mole fraction of the solute in solution is 0.2. What would be the mole fraction of the solvent if the decrease in vapour pressure is 20 mm of Hg?

Which one is not equal to zero for an ideal solution?

The freezing point depression constant ($K_f$) of benzene is $5.12 \text{ K kg mol}^{-1}$. The freezing point depression for the solution of molality $0.078 \text{ m}$ containing a non-electrolyte solute in benzene is:

The molarity of a $0.2 \text{ N } Na_2CO_3$ solution will be:

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