What is the relationship between gas pressure and solubility at varying depths?

The relationship between gas pressure and solubility is fundamentally governed by Henry's Law, which states that the amount of gas that dissolves in a liquid is directly proportional to the pressure of that gas above the liquid. As the pressure increases at greater depths in a body of water, the solubility of gases, such as oxygen and nitrogen, also increases. This means that more gas can be held in solution at higher pressures, allowing for a greater concentration of dissolved gases in the water.

At greater depths, the increase in pressure enhances the capacity of water to dissolve gases, making option C the correct choice. This principle is particularly important for divers to understand, as the increase in solubility at depth can influence the behavior of gases during ascent and descent, including the formation of bubbles during decompression.

In contrast, the other choices contradict established principles. The idea that solubility decreases with increasing pressure is inaccurate, as it overlooks the direct relationship established by Henry's Law. Suggesting that solubility is unaffected by depth ignores the significant effects pressure has on gas solubility. Lastly, while gas bubbles can indeed form during changes in pressure, stating this in relation to pressure increasing does not accurately reflect the concept of solubility at