State where forward and reverse reactions occur at equal rates

Equilibrium constant for dissolution of a solid in water

Square brackets denote molar concentrations

Superscripts indicate stoichiometric coefficients

Determine if a precipitate will form under given conditions

Calculate the concentration of ions in a saturated solution

Solubility generally increases with temperature

Presence of an ion in common with the solid reduces solubility

Acidic or basic conditions can affect solubility of certain compounds

Determine the maximum amount of solid that can dissolve

Calculate the new solubility after adding a common ion

Key to predicting and controlling chemical reactions

Relevance in water treatment and pollution control

Used in qualitative and quantitative analysis of ions

Does not predict rate of dissolution or precipitation

Real solutions may deviate from ideal behavior due to intermolecular forces