Liquid Solution

\(\mathrm{K}_{\mathrm{H}}\) for \(\mathrm{O}_2\) at \(293 \mathrm{~K}\) is \(34.86 \mathrm{~kbar}\). What should be the partial pressure of \(\mathrm{O}_2\) gas so that it has a solubility of \(0.08 \mathrm{~g} / \mathrm{L}\) in water at \(293 \mathrm{~K}\) ? (Density of solution \(=1 \mathrm{~g} / \mathrm{ml}\))