acid/base vocabulary
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| Dissociation | the separation of ions that occurs when an ionic compound dissolves
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| Hydronium ion | the H3O+ ion
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| Ionization | the formation of ions from solute molecules by the action of the solvent; any process that results in the formation of an ion
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| Strong electrolyte | any compound of which all or almost all of the dissolved compound exists as ions in aqueous solution
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| Weak electrolyte | a compound of which relatively small amount of dissolved compound exists as ions in an aqueous sulition
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| pH | the negative of the common logarithm of the hydronium ion concentration of a solution
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| pOH | the negative of the common logarithm of the hydroxide ion concentration of a solution
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| Acid base indicator | a compound whose color is sensitive to pH
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| Titration | the controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration
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| End point | the point in a titration at which an indicator changes color
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| Equivalence point | the point at which the two solutions used in a titration are present in chemically equivalent amounts
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| Alkaline | a solution in which a base has completely dissociated in water to yield aqueous OH- ions
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| Arrhenius Acids | a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solution
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| Arrhenius Base | a substance that increases the concentration of hydroxide ions, OH-, in aqueous solution
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| Binary acid | an acid that contains only two different elements: hydrogen and one of the more-electronegative elements
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| Strong acid | an acid that ionizes completely in aqueous solution
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| Weak acid | an acid that is a weak electrolyte
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| Amphoteric | any species that can react as either an acid or a base
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| BrØnsted-Lowery base | a molecule or ion that is a proton acceptor
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| BrØnsted-Lowery acid | a molecule or ion that is a proton donor
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| Lewis acid-base reaction | the transfer of protons from one reactant (the acid) to another (the base)
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| Lewis acid | an atom, ion, or molecule that accepts an electron pair to form a covalent bond
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| Lewis base | an atom, ion, or molecule that donates an electron pair to form a covalent bond
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| Diprotic acid | an acid that can donate two protons per molecule
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| Monoprotic acid | an acid that can donate only one proton (hydrogen ion) per molecule
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| Polyprotic acid | an acid that can donate more than one proton per molecule
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| Triprotic acid | an acid able to donate three protons per molecule
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| Conjugate acid | the species that is formed when a BrØnsted-Lowry base gains a proton
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| Conjugate base | the species that remains after a BrØnsted-Lowry acid has given up a proton
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| Neutralization | the reaction of hydronium ions and hydroxide ions to form water molecules
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| Salt | an ionic compound composed of a cation and the anion from an acid; an ionic compound composed of a cation from a base and an anion from an acid
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| Oxyacid | an acid that is compound of hydrogen, oxygen, and a third element, usually a non-metal
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| BrØnsted-Lowery reaction | the transfer of protons from one reactant (the acid) to another (the base)
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