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| 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
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| complex ion | ion consisting of a transition metal central atom and surrounding molecules or ions called ligands
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| coordinate covalent bond | (also, dative bond) bond formed when one atom provides both electrons in a shared pair
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| dissociation constant (Kd) | equilibrium constant for the decomposition of a complex ion into its components in solution
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| formation constant (Kf) | (also, stability constant) equilibrium constant for the formation of a complex ion from its components in solution
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| Lewis acid | any species that can accept a pair of electrons and form a coordinate covalent bond
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| Lewis acid-base adduct | compound or ion that contains a coordinate covalent bond between a Lewis acid and a Lewis base
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| Lewis base | any species that can donate a pair of electrons and form a coordinate covalent bond
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| ligand | molecule or ion that surrounds a transition metal and forms a complex ion; ligands act as Lewis bases
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| molar solubility | solubility of a compound expressed in units of moles per liter (mol/L)
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| 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
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| selective precipitation | process in which ions are separated using differences in their solubility with a given precipitating reagent
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| solubility product (Ksp) | equilibrium constant for the dissolution of a slightly soluble electrolyte
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