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The Henry’s law constant for O2 in water at 25°C is 1.27×10−3M/atm and the mole fraction of O2 in the atmosphere is 0.21. Calculate the solubility of O2 in water at 25°C at an atmospheric pressure of 1.00 atm. Strategy: ▪ Use Dalton’s law of partial pressures to calculate the partial pressure of oxygen. ▪ Use Henry’s law to calculate the solubility, expressed as the concentration of dissolved gas.

The Henry’s law constant for O2 in water at 25°C is 1.27×10−3M/atm and the mole fraction of O2 in the atmosphere is 0.21. Calculate the solubility of O2 in water at 25°C at an atmospheric pressure of 1.00 atm. Strategy: ▪ Use Dalton’s law of partial pressures to calculate the partial pressure of oxygen. ▪ Use Henry’s law to calculate the solubility, expressed as the concentration of dissolved gas. Correct Answer 2.7×10-4M

According to Dalton’s law, the partial pressure of O2 is proportional to the mole fraction of O2: PA=XAPt=(0.21)(1.00atm)=0.21atm From Henry’s law, the concentration of dissolved oxygen under these conditions is: CO2 = KpO2 = (1.27×10−3M/atm) (0.21atm) = 2.7×10-4 M.

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