A solution with oxygen dissolved in water containing $0.5 \mathrm{mg} \mathrm{\textrm {O } _ { 2 }} / 100 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$ is brought in contact with a large volume of atmospheric air at $283 \mathrm{~K}$ and a total pressure of $1 \mathrm{~atm}$. The Henry's law constant for the oxygen-water system at $283 \mathrm{~K}$ equals $32,700 \mathrm{~atm} / \mathrm{mol}$ fraction.

(a) Will the solution gain or lose oxygen?

(b) What will be the concentration of oxygen in the equilibrium solution?