Chapter 15 Key Terms

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 central atom surrounding molecules or ions called ligands via coordinate covalent bonds

coordinate covalent bond

(also, dative bond) covalent bond in which both electrons originated from the same atom

coupled equilibria

system characterized the simultaneous establishment of two or more equilibrium reactions sharing one or more reactant or product

dissociation constant (K_d)

equilibrium constant for the decomposition of a complex ion into its components

formation constant (K_f)

(also, stability constant) equilibrium constant for the formation of a complex ion from its components

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 acid-base chemistry

reactions involving the formation of coordinate covalent bonds

Lewis base

any species that can donate a pair of electrons and form a coordinate covalent bond

ligand

molecule or ion acting as a Lewis base in complex ion formation; bonds to the central atom of the complex

molar solubility

solubility of a compound expressed in units of moles per liter (mol/L)

selective precipitation

process in which ions are separated using differences in their solubility with a given precipitating reagent

solubility product constant (K_sp)

equilibrium constant for the dissolution of an ionic compound