What is commonly true about the solubility of gases in relation to pressure changes?

When considering the solubility of gases, the relationship to pressure is guided by Henry's Law. This law states that the amount of gas that can be dissolved in a liquid at a given temperature is directly proportional to the partial pressure of that gas above the liquid. Therefore, as the pressure of a gas increases, the solubility of that gas in the liquid also increases. This means that under higher pressure, more gas molecules can be forced into solution.

This principle is evident in various real-world applications, such as carbonated beverages, where carbon dioxide is dissolved in the liquid under high pressure. When the bottle is opened, the pressure is released, leading to a decrease in the solubility of carbon dioxide and the gas escapes, resulting in the characteristic fizz.

Understanding this relationship helps elucidate why elevated pressure is key to enhancing gas solubility in liquids, affirming that increased pressure leads to greater solubility.