What does an increase in pressure do to the solubility of gases?

An increase in pressure affects the solubility of gases by increasing the amount of gas that can dissolve in a liquid. This phenomenon is largely explained by Henry's Law, which states that the amount of a gas that can dissolve in a liquid at a given temperature is directly proportional to the partial pressure of that gas in equilibrium with the liquid.

When the pressure of a gas above a liquid increases, the gas molecules are forced into the liquid more effectively, which leads to a higher concentration of the gas dissolved in the liquid. This relationship is particularly noticeable in systems involving gases and is utilized in various applications, such as carbonated beverages, where carbon dioxide is dissolved in solutions under high pressure. When the bottle is opened, the pressure is released, and the gas escapes, which is why we see bubbles forming.

By understanding this principle, it's clear why an increase in pressure improves the solubility of gases in liquids.