Embibe Experts Solutions for Chapter: Solutions, Exercise 1: Level 1

The boiling point of $0.001 \mathrm{M}$ aqueous solution of $\mathrm{NaCl}, {\mathrm{Na}}_2{\mathrm{SO}}_4, {\mathrm{K}}_3{\mathrm{PO}}_4$ and ${\mathrm{CH}}_3\mathrm{COOH}$ should follow the order:

The freezing point of pure benzene is $5.5 °\mathrm{C}$. When $2.9 \mathrm{g}$ of butane is dissolved in $200 \mathrm{g}$ of benzene, the freezing point of benzene decreases to $4 °\mathrm{C}$. To lower the freezing point of benzene by another $1.5 °\mathrm{C}$, the amount of butane that has to be added to mixture is:

The boiling points of two miscible liquids, which do not form an azeotropic mixture, are close to each other. Their separation is best carried out by:

The value of Henry's law constant of $\mathrm{Ar}, {\mathrm{CO}}_2, {\mathrm{CH}}_4,$ and ${\mathrm{O}}_2$ in water at $25°\mathrm{C}$ are $40.30,1.67,0.41$ and $34.86 \mathrm{kbar},$respectively. The order of their solubility in water at the same temperature and pressure is:

Upon mixing equal volumes of aqueous solutions of $0.1 \mathrm{M} \mathrm{HCl}$ and $0.2 \mathrm{M} {\mathrm{H}}_2{\mathrm{SO}}_4,$ the concentration of ${\mathrm{H}}^{+}$ in the resulting solution is:

The variation of solubility of four different gases ($\mathrm{G}1,\mathrm{G}2$ etc.,) in a given solvent with pressure at a constant temperature is shown in the plot.

The gas with the highest value of Henry's law constant is

At $300 \mathrm{K}$ the vapour pressure of two pure liquids, $\mathrm{A}$ and $\mathrm{B}$ are $100$ and $500 \mathrm{mmHg}$, respectively. If in a mixture of $\mathrm{A}$ and $\mathrm{B}$, the vapour pressure is $300 \mathrm{mmHg}$, the mole fractions of $\mathrm{A}$ in the liquid and in the vapour phase, respectively, are

At $298 \mathrm{K}$, the ratio of osmotic pressures of two solutions of a substance with concentrations of $0.01 \mathrm{M}$ and $0.001 \mathrm{M}$, respectively, is: