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Pressure and Gas Solubility (Henry's Law)

Here we look at pressure and solubility of a gas dissolved in liquid. This is a relationship referred to as Henry's law. In this case, the solute is a gas, and the solvent is a liquid, water. Henry's law states that there is a direct relationship between partial pressure and gas solubility. When the partial pressure of a gas on or above a liquid increases, the solubility of the gas in the liquid increases. Gases dissolve in water frequently: a good example is soda, where carbon dioxide gas dissolves in water. When the soda bottle is closed, the partial pressure above the liquid is high, and so gas solubility is high as well. When the soda bottle is opened, the partial pressure decreases, and the solubility of the gas also decreases. Bubbles form, because much of the gas cannot dissolve any more. Henry's law is also important in Scuba diving. As the diver goes deeper under the water, there is more and more pressure, and so more and more gas can dissolve in their blood. If the scuba diver comes to the surface too quickly, gas will bubble out of their blood, causing decompression sickness or the bends. This can be treated using a decompression chamber, which increases the pressure on the scuba diver, and so it adjusts the gas pressure and the gas solubility.