Solubility equilibrium

Solubility equilibrium is the dynamic balance in a saturated solution between a dissolved substance and its undissolved solid, with dissolution and precipitation occurring at equal rates.

Dissolution: Dissolution is the process by which particles of a solute disperse into a solvent. It supplies dissolved particles as the solid enters solution.
Chemical equilibrium: Chemical equilibrium is a state in which forward and reverse reaction rates are equal and concentrations remain constant. Solubility equilibrium is a phase-specific instance of this general balance.
Gravimetric analysis: Gravimetric analysis determines a substance’s amount by measuring the mass of a solid formed from it. Controlled precipitation turns dissolved analytes into weighable solids.
Unsaturated solution: An unsaturated solution contains less dissolved solute than its equilibrium solubility limit under specified conditions. Unlike a saturated solution, it can dissolve more solute without precipitation.
Precipitation: Precipitation is the formation of a solid from substances dissolved in a solution. It returns dissolved particles to the solid phase.
Chemical potential: Chemical potential is the change in a system’s free energy when the amount of a substance changes. Equal chemical potentials across phases characterize equilibrium between solid and solution.
Selective precipitation: Selective precipitation separates substances by forming one insoluble compound while others remain dissolved. Differences in solubility equilibria enable separation of ions.
Supersaturated solution: A supersaturated solution contains more dissolved solute than its stable equilibrium solubility limit. It is a metastable excess, not a stable solid–solution balance.
Saturated solution: A saturated solution contains as much dissolved solute as can remain at equilibrium under specified conditions. It is the solution state in which solubility equilibrium can be established.
Activity (chemistry): Activity is an effective concentration that accounts for nonideal interactions in a chemical system. Equilibrium constants are rigorously expressed using activities rather than raw concentrations.

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