If the solubility of $H_2S$ in water at $STP$ is $0.195 \, m$,what is the value of $K_H$ in $bar$?

The 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 total pressure of $10 \ atm$. At $298 \ K$,if the Henry's law constants for oxygen and nitrogen are $3.30 \times 10^{7} \ mm \ Hg$ and $6.51 \times 10^{7} \ mm \ Hg$ respectively,calculate the mole fractions of these gases in water.

Henry's law constant for the molality of methane in benzene at $298 \, K$ is $4.27 \times 10^{5} \, mm \, Hg$. Calculate the solubility of methane in benzene at $298 \, K$ under $760 \, mm \, Hg$.

What is the solubility of a gas in water at $25^{\circ} C$ if the partial pressure is $0.18 \ atm$? $(K_{H} = 0.16 \ mol \ dm^{-3} \ atm^{-1})$

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

For the solution of the gases $w$,$x$,$y$ and $z$ in water at $298 \ K$,the Henry's law constants $(K_H)$ are $0.5$,$2$,$35$ and $40 \ kbar$,respectively. The correct plot for the given data is