Solubilityis

Solubilityis is the property of a substance (the solute) to dissolve in a solvent to form a homogeneous solution at a specified temperature and pressure. In practical terms, solubility is typically expressed as the maximum amount of solute that can dissolve in a given amount of solvent to form a saturated solution, often reported as molarity (M), molality (m), or grams per liter (g/L).

Solubility depends on interactions between solute and solvent, temperature, and, for gases, pressure. For many solids in water, solubility changes with temperature, typically increasing with temperature, though there are notable exceptions. Gas solubility in liquids generally decreases with increasing temperature and increases with higher pressure, following Henry's law. Solubility can be hindered or enhanced by solvent polarity and the presence of common ions (the common-ion effect).

Chemical considerations include the solubility product constant (Ksp) for sparingly soluble salts, which defines the equilibrium between solid and dissolved ions. The dissolution rate is not the same as solubility and depends on kinetics, surface area, and agitation.

Applications span pharmaceuticals, where solubility influences bioavailability; environmental science, where the solubility of pollutants affects transport and toxicity; and materials science, where crystallization and precipitation are used in manufacturing. Measuring solubility involves equilibrating phases, constructing solubility curves, or using gravimetric, spectroscopic, or chromatographic methods.