Because it is very very important. Here is why:
There are two principal why gas solubility is important for divers:
Narcosis. The lipid solubility of gas determines the narcotic effect at depth. For most divers, this is not really noticeable until they reach about 100 feet in depth, when they start to suffer to a greater or lesser degree from narcosis (often misleadingly called "Nitrogen narcosis", or "rapture of the deep"). Technical divers who go to greater depths often use helium gas mixes - due to the very low lipid solubility of helium, it has very little narcotic affect, leaving the diver clear headed.
Decompression sickness. Breathing gases under pressure causes the body to also absorb those gases. If a diver stays at depth for a long time, her tissues can absorb a great deal of gas, and if she ascends too quickly, bubbles can form in her bloodstream, which leads to decompression sickness (also called "the bends" or "caisson's disease"). Divers can avoid DCS by either breathing oxygen rich mixtures like nitrox (the body metabolises oxygen, so it doesn't get absorbed) or limiting their depth or bottom teams to avoid excessive gas absorbtion. Divers who stay too deep or too long need to make decompression stops at shallow depths before surfacing, to allow the gas to diffuse out of their tissues safely.
Solubility can increase and decrease with temperature variations and changes, Pressure can increase and decrease solubility with difference pressure variations, the nature of the gas and the nature of the solvent as well chance the solubility of the gas.
If the pressure of the gas increase, the solubility in a liquid increase.
Increasing temperature decreases gas solubility in water due to reduced gas solubility at higher temperatures. In contrast, increasing pressure increases gas solubility in water according to Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid.
When the pressure increase the solubility increase.
Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. This means that as the pressure of the gas increases, its solubility in the liquid also increases, and vice versa.
Divers need to understand solubility because it plays a critical role in how gases behave under pressure while underwater. As divers descend, the increased pressure causes more gas (like nitrogen) to dissolve in their blood and tissues. If a diver ascends too quickly, the rapid decrease in pressure can lead to gas bubbles forming, resulting in decompression sickness, or "the bends." Therefore, it’s crucial for divers to follow proper ascent rates and safety stops to allow gases to safely off-gas.
If you are talking about the solubility of gasses in a liquid then lowering the temperature will increase the solubility of the gas
Pressure can affect the solubility but the effect is not important.
Solubility can increase and decrease with temperature variations and changes, Pressure can increase and decrease solubility with difference pressure variations, the nature of the gas and the nature of the solvent as well chance the solubility of the gas.
Increasing the temperature of a solvent decreases the solubility of a gas Generally, increasing solvent temperature decreases the solubility of gases.
solubility of a gas or solid?
Increasing temperature decreases the solubility of a gas solute in a liquid solvent. This is because higher temperatures increase the kinetic energy of molecules, leading to weaker gas-liquid interactions and reduced solubility.
The word solubility is inadequate here; gases form mixtures.
If the pressure of the gas increase, the solubility in a liquid increase.
More gas dissolves into the liquid.
Increasing temperature decreases gas solubility in water due to reduced gas solubility at higher temperatures. In contrast, increasing pressure increases gas solubility in water according to Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid.
Solubility is direct proportional to pressure