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Solubility changes with temperature and pressure in gases and solids, where temperature increases decrease gas solubility but typically increase solid solubility. Henry's law explains gas solubility under varying pressures.
The solubility of most substances depends strongly on the temperature and, in the case of gases, on the pressure. When it comes to solubility changes, for gases, as temperature increases, the solubility decreases due to the increased kinetic energy of the gas molecules, causing them to escape the attraction of the solvent molecules.
Henry's law describes the relationship between the pressure and the solubility of a gas, providing a mathematical expression for gas solubility in liquids under different pressures.
In contrast, for solids, the majority exhibit increased solubility with higher temperatures, although this effect can vary depending on the specific solute, as depicted in solubility curves.
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