What relationship exists between pressure and the solubility of gases in liquids?

The solubility of gases in liquids is characterized by a direct relationship with pressure, which is described by Henry's Law. According to Henry's Law, the amount of gas that can dissolve in a liquid at a specific temperature is directly proportional to the partial pressure of that gas above the liquid. This means that as the pressure of the gas increases, the solubility of the gas in the liquid also increases.

For example, when carbonated beverages are sealed, carbon dioxide is dissolved in the liquid under high pressure. When the seal is broken, the pressure decreases, resulting in the escape of gas bubbles. This relationship highlights the importance of pressure in controlling the solubility of gases in liquids, which is vital in various applications, including chemical reactions and biological processes in aquatic systems.

Understanding this positive correlation is essential for fields such as chemistry, environmental science, and medicine, where gas exchange in liquids is a crucial factor.