What is the effect of increasing pressure on the solubility of a gas in a liquid?

When pressure is increased in a system containing a gas dissolved in a liquid, the solubility of that gas in the liquid typically increases. This phenomenon can be explained by Henry's Law, which states that the amount of gas that dissolves in a liquid at a constant temperature is directly proportional to the pressure of that gas above the liquid.

As the pressure above the liquid increases, it forces more gas molecules into the liquid, enhancing the interaction between the gas and the liquid particles. This results in a higher concentration of the dissolved gas in the liquid. For example, carbonated beverages are a practical illustration of this principle; when the pressure inside the can is released (by opening it), the solubility of carbon dioxide decreases, leading to the formation of bubbles as the gas escapes from the liquid.

In summary, increasing the pressure directly impacts gas solubility by promoting a higher amount of gas to be dissolved in the liquid, thus affirming that the correct response is that the solubility increases.