The variation of solubility with temperature $T$ for a gas in a liquid is shown by the following graphs. The correct representation is:

The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas. This statement is known as ...

Calculate $K_H$ when $2 \ mmol$ of $O_2$ dissolve in $540 \ mL$ of water at $27 \ ^oC$ temperature. Given $P_{O_2} = 2 \times 10^{-8} \ bar$.

The Henry's law constant for the solubility of $N_2$ gas in water at $25 \, ^oC$ is $1 \times 10^5 \, atm$. The mole fraction of $N_2$ in air is $0.8$. Calculate the number of moles of $N_2$ from air that will dissolve in $10 \, moles$ of $H_2O$ at $25 \, ^oC$ and at a total pressure of $5 \, atm$.

Which of the following salt's solubility increases appreciably with an increase in temperature?

What is the significance of Henry's Law constant $K_H$?