How does increasing pressure affect the solubility of gases in divers' bodies?

Increasing pressure has a direct effect on the solubility of gases in liquids, such as the blood and tissues of divers. As pressure increases, the amount of gas that can dissolve in a liquid also increases. This phenomenon is explained by Henry's Law, which states that at a constant temperature, the amount of dissolved gas is proportional to the pressure of that gas above the liquid.

For divers, this increased solubility is significant during descents when they are exposed to higher ambient pressure. The body absorbs more of the breathing gases, like nitrogen, which is critical to understand in the context of avoiding issues such as decompression sickness, commonly known as "the bends." After spending time at depth, when ascending, it's important for divers to follow safe ascent procedures to allow dissolved gases to safely come out of solution and be exhaled, preventing bubbles from forming in the tissues and bloodstream.

In contrast, the other options do not align with this scientific principle. While it may seem intuitive to think that increased pressure could reduce solubility or have no effect, the opposite is true according to established gas laws. "Inerting" gases does not apply here, as increasing pressure enhances the solubility of gases, rather than rendering them