A scuba diver is breathing compressed air that is 21% (by volume) oxygen at a depth of 66 ft. beneath the surface. The total pressure at this depth is 3.0 atm. The Henry's law constant (k) for O2 in water at a normal body temperature (37 °C ) is 1.93 * 10-3 mol>(L atm). What is the solubility of O2 in the blood of the diver at 66 ft. beneath the surface? (LO 13.9) (a) 1.22 * 10-3 M (b) 2.76 * 10-2 M (c) 1.22 * 10-1 M (d) 2.76 * 10-1 M

Henry's Law states that the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of that gas above the liquid. This relationship can be expressed mathematically as C = kP, where C is the concentration of the gas in the liquid, k is the Henry's law constant, and P is the partial pressure of the gas. Understanding this law is crucial for calculating the solubility of gases in liquids, such as oxygen in blood.

Partial pressure is the pressure exerted by a single component of a gas mixture. In the context of the scuba diver, the total pressure at a depth of 66 ft is 3.0 atm, and the partial pressure of oxygen can be calculated by multiplying the total pressure by the fraction of oxygen in the air (21%). This concept is essential for determining how much oxygen is available for dissolution in the diver's blood.

The solubility of gases in blood is influenced by factors such as temperature, pressure, and the specific gas involved. For oxygen, its solubility can be calculated using Henry's Law, taking into account the partial pressure of oxygen and the Henry's law constant for oxygen in blood. This concept is vital for understanding how oxygen is transported in the body, especially under varying pressure conditions experienced by divers.