- common ion effect
- effect on equilibrium when a substance with an ion in common with the dissolved species is added to the solution; causes a decrease in the solubility of an ionic species, or a decrease in the ionization of a weak acid or base
- complex ion
- ion consisting of a transition metal central atom and surrounding molecules or ions called ligands
- coordinate covalent bond
- (also, dative bond) bond formed when one atom provides both electrons in a shared pair
- dissociation constant
- (Kd) equilibrium constant for the decomposition of a complex ion into its components in solution
- formation constant
- (Kf) (also, stability constant) equilibrium constant for the formation of a complex ion from its components in solution
- Lewis acid
- any species that can accept a pair of electrons and form a coordinate covalent bond
- Lewis acid-base adduct
- compound or ion that contains a coordinate covalent bond between a Lewis acid and a Lewis base
- Lewis base
- any species that can donate a pair of electrons and form a coordinate covalent bond
- ligand
- molecule or ion that surrounds a transition metal and forms a complex ion; ligands act as Lewis bases
- molar solubility
- solubility of a compound expressed in units of moles per liter (mol/L)
- multiple equilibrium
- system characterized by more than one state of balance between a slightly soluble ionic solid and an aqueous solution of ions working simultaneously
- selective precipitation
- process in which ions are separated using differences in their solubility with a given precipitating reagent
- solubility product (Ksp)
- equilibrium constant for the dissolution of a slightly soluble electrolyte