solubilitylimit

Solubility limit refers to the maximum concentration of a solute that can be dissolved in a solvent at a given temperature (and pressure, if relevant) to form a saturated solution. At or above this limit, additional solute will not dissolve and will precipitate or remain as a separate phase, assuming equilibrium conditions. The concept applies to liquids as well as to solid solutions, where it describes the maximum amount of one component that can be dissolved in another within the solid lattice.

In binary phase diagrams, the solubility limit is represented by the solubility curves that bound the region of complete solid solution. Within this region, the two components form a continuous solid solution; outside, the system separates into distinct phases. For liquids, solubility limits depend strongly on temperature; for gases dissolved in liquids, Henry's law governs the apparent limit.

In metals and ceramic systems, solubility limits influence alloy design, precipitation hardening, and phase stability. They can be affected by factors such as temperature, pressure, solvent properties, and the presence of other ions or impurities (common-ion effect).

Measurement and reporting: solubility is usually given as a maximum concentration, often in units such as g solute per 100 g solvent, molarity, or weight percent. The term is closely related to solubility products (Ksp) for sparingly soluble compounds in aqueous solutions, and to phase equilibria in materials science.