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What is the ratio of the solubilities of \( \mathrm{N}_{2} \) and \( \mathrm{O}_{2} \) in \( \mathrm{H}_{2} \mathrm{O} \) at \( 373 \mathrm{~K} \), given that \( \mathrm{K}_{H}\left(\mathrm{~N}_{2}\right)=12.6 \times 10^{4} \) atm and \( K_{H}\left(O_{2}\right)=7.01 \times 10^{4} \mathrm{~atm} \) ? Assume that \( p\left(N_{2}\right)=0.80 \mathrm{~atm} \) and \( p\left(O_{2}\right)=0.20 \mathrm{~atm} \).

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