What effect does pressure generally have on the solubility of gases in liquids?

The solubility of gases in liquids generally increases with pressure due to Henry's Law, which states that at constant temperature, the amount of a gas that dissolves in a liquid is directly proportional to the partial pressure of that gas above the liquid. When the pressure over the liquid is increased, more gas molecules are forced into the liquid phase, leading to higher solubility. This principle is commonly observed in carbonated beverages, where increased pressure allows a greater amount of carbon dioxide to dissolve in the liquid, which is then released as bubbles when the pressure is reduced (such as when you open a bottle).

In contrast, reduced pressure decreases the solubility of gases and may lead to gas escaping from the solution. It is also important to note that solubility is not impacted by pressure in the same way for solid or liquid solutes, which are typically unaffected by changes in atmospheric pressure.