text: For condensed phases (solids and liquids), the pressure dependence of solubility is typically weak and usually neglected in practice. Assuming an ideal solution, the dependence can be quantified as:
  where  is the mole fraction of the -th component in the solution,  is the pressure,  is the absolute temperature,  is the partial molar volume of the th component in the solution,  is the partial molar volume of the th component in the dissolving solid, and  is the universal gas constant.
  The pressure dependence of solubility does occasionally have practical significance. For example, precipitation fouling of oil fields and wells by calcium sulfate (which decreases its solubility with decreasing pressure) can result in decreased productivity with time.