Solubility of a gas in a liquid increases with

Calculate the pressure of the gas if the solubility of the gas in water at $25^{\circ} C$ is $6.85 \times 10^{-4} \ mol \ dm^{-3}$. (Henry's law constant $K_H$ is $6.85 \times 10^{-4} \ mol \ dm^{-3} \ bar^{-1}$) (in $bar$)

Given the solubility curves of $KNO_3$ and $KCl$,which of the following statements is not true?

Air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportions of $20\%$ and $79\%$ by volume at $298\ K$. The water is in equilibrium with air at a pressure of $10\ atm$. At $298\ K$,if the Henry's law constants for oxygen and nitrogen are $3.30 \times 10^7\ mm$ and $6.51 \times 10^7\ mm$,respectively,the mole ratio of gases $(O_2 : N_2)$ dissolved in water is about

Solubility of $N_2$ gas in water at $25\,^{\circ}C$ and $0.78\, atm$ is $5.4 \times 10^{-4}\, M$. Calculate Henry's law constant for $N_2$ in water at $25\,^{\circ}C$.

Which of the following graphs correctly represents the plots of $K_{H}$ for gases in water versus temperature?