Henry's Law Calculations Practice Problems

The solubility of O₂ in water at a partial pressure of 1.00 atm is 1.10 × 10^–3 mol/L. The partial pressure of O₂ in arterial blood is 100. mmHg while the partial pressure of O₂ in venous blood is 35.0 mmHg. What percentage of O₂ originally dissolved in arterial blood remains in venous blood? Assume the total volume of blood in the body is 5.00 L and the solubility of O₂ in blood is similar to that of water.

At a CO₂ partial pressure of 1.00 atm and 25°C, the solubility of CO₂ in water is 3.42 × 10^–2 mol/L. Calculate the solubility of CO₂ (in g/mL) at 25°C if the partial pressure of CO₂ is 850 mmHg.

At a temperature of 15°C, the partial pressure of NO is 675.0 mmHg. Determine the solubility (in g/mL) of NO in water, given that Henry's law constant for NO at 15°C is 2.31 × 10^–3 M/atm.

At a Ne partial pressure of 1.0 atm, the solubility of Ne in water is 4.83 × 10^–4 M at 15 °C and 4.42 × 10^–4 M at 30 °C. Suppose that Ne is dissolved in 2.0 L water at 15 °C. Calculate the mass of Ne lost if the temperature is increased to 30 °C.

A 0.80 g of gas sample is soluble in 1 L of water at 2°C and 2.00 atm. Calculate the amount of the gas sample soluble in 1L of water at 2°C and 5.00 atm.