The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the solubility of $O_2$ from the air is $2\mathrm{.}67{10}^{-4}M$ at sea level and $25C,$ what is the solubility of $O_2$ at an elevation of $12,000ft$ where the atmospheric pressure is $0\mathrm{.}657$ atm? Assume the temperature is $25C,$ and that the mole fraction of $O_2$ in air is $0\mathrm{.}209$ at both $12,000ft$ and at sea level.