Final answer:
Henry's law describes the direct proportionality between the pressure and solubility of a gas in a liquid. Applications include the release of gas from carbonated beverages upon opening and avoiding 'the bends' in scuba diving by ascending slowly. Deviations occur when the solute reacts chemically with the solvent.
Step-by-step explanation:
Henry's law explains how the solubility of a gas in a liquid is affected by pressure. Specifically, Henry’s law states that the concentration of gas in a liquid is directly proportional to the solubility and the partial pressure of that gas. For instance, when you open a carbonated beverage, the pressure of CO₂ above the liquid drops, leading to the escape of gas as bubbles, which is a direct application of Henry's law. On the other hand, scuba divers must ascend slowly to avoid 'the bends', a condition caused by a rapid decrease in pressure that results in nitrogen bubbles forming in the blood. This is because, under higher pressures, more nitrogen dissolves in the body fluids according to Henry's law.
It is important to note that deviations from Henry's law occur when the solute gas chemically reacts with the solvent. An example of this is the increased solubility of ammonia in water due to the formation of ammonium and hydroxide ions, which cannot be accurately predicted by Henry's law alone.