At $T(K)$,the partial pressure of dissolved oxygen in $1 \ L$ water is $1 \ bar$. The concentration of oxygen in $ppm$ is ($K_{H}$ of $O_2$ at $T(K)$ is $50 \ kbar$)

$A$ gas $X$ is dissolved in water at $2 \ bar$ pressure. Its mole fraction in the solution is $0.02$. Find the mole fraction of water in the solution when the pressure of the gas is doubled at the same temperature.

At $298 \ K$,Henry's law constant for $CO_2$ in water is $1.67 \times 10^8 \ Pa$. At $298 \ K$,the quantity of $CO_2$ in $1000 \ mL$ of soda water when packed at $1.67 \times 10^2 \ kPa$ $CO_2$ pressure in $mol \ L^{-1}$ is: (water density $= 1.0 \ g \ cm^{-3}$)

Which one of the following statements regarding Henry's law is not correct?

What is the solubility of a gas in water at $25^{\circ} C$ if the partial pressure is $0.346 \ bar$ (Henry's law constant is $0.159 \ mol \ dm^{-3} \ bar^{-1}$)?

As temperature increases,the value of $K_H$ increases,thus the value of solubility of a gaseous solute will $ . . . . . . $.