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