Prof. Anil Thomas and Prof. Santosh Yadav Solutions for Chapter: Solutions and Colligative Properties, Exercise 2: Critical Thinking

How many grams of $\mathrm{KCl}$ should be added to $1000 \mathrm{g}$ of water, so that the freezing point reduces to $–10 °\mathrm{C}$?

If $\text{α}$ is the degree of dissociation of ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}$, the value of Van’t Hoff’s factor ($\mathrm{i}$) will be:

Which of the following compound corresponds Van’t Hoff factor $\left(\mathrm{i}\right)$ to be equal to $2$ for dilute solution?

At higher altitudes, the boiling point of water lowers because:

Equimolal solutions of $\mathrm{A}$ and $\mathrm{B}$ show depression of freezing point in the ratio of  $2 :1$. $\mathrm{A}$ remains in normal state, the state of $\mathrm{B}$ in the solution is:

Which does NOT influence the solubility of a solid in a liquid solvent?

The ratio of the value of any colligative property for $\mathrm{KCl}$ solution to that of a sugar solution is nearly:

On dissolving $3.24 \mathrm{g}$ of sulphur in $40 \mathrm{g}$ of benzene, boiling point of solution was higher than that of benzene by $\mathrm{0.81 }\mathrm{K}. {\mathrm{K}}_{\mathrm{b}}$ value of benzene is $\mathrm{2.53 }\mathrm{K} \mathrm{kg} {\mathrm{mol}}^{\mathrm{-1}}$. Atomic mass of sulphur is $\mathrm{32 }\mathrm{g} {\mathrm{mol}}^{\mathrm{-1}}$. The molecular formula of sulphur is: