Table A-11 (page 872) reports KH=4.01x10+4 atm for O2 at 20C. These KH values use gas phase partial pressure in atmospheres and aqueous phase concentration in mole fraction (which is dimensionless) and are often indicated with the symbol K. Convert this K to KH in M/atm. Assume the concentration of O2 in water is dilute, meaning the number of moles of O2 in a sample is small compared to the number of moles of water and that the density is negligibly different from the density of water (1.00 kg/L). What saturation O2 concentration is predicted in mg/L? How does this compare to the value in Table A-2 at 20C? Use molar masses 32.00 and 18.02 for O2 and H2O.

TABLE A-11 H2 H2S CH4 Henry's Law Constants for Common Gases Soluble in H2O KH x 10-* (atm) Temperature (C) Air N2 02 CO2 0 4.32 5.29 2.55 0.073 3.52 10 5.49 6.68 3.27 0.104 4.42 6.64 8.04 4.01 0.142 5.36 30 7.71 9.24 4.75 0.186 6.20 40 8.70 10.4 5.35 0.233 6.96 5.79 6.36 0.027 0.037 2.24 2.97 20 0.048 3.76 6.83 7.29 0.061 0.075 4.49 5.20 7.51 TABLE A-11 H2 H2S CH4 Henry's Law Constants for Common Gases Soluble in H2O KH x 10-* (atm) Temperature (C) Air N2 02 CO2 0 4.32 5.29 2.55 0.073 3.52 10 5.49 6.68 3.27 0.104 4.42 6.64 8.04 4.01 0.142 5.36 30 7.71 9.24 4.75 0.186 6.20 40 8.70 10.4 5.35 0.233 6.96 5.79 6.36 0.027 0.037 2.24 2.97 20 0.048 3.76 6.83 7.29 0.061 0.075 4.49 5.20 7.51