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Acids and Bases
Vocabulary for Chemistry
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 a relatively small amount of the dissolved compound exists as ions in an aqueous solution. |
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 an aqueous solution. |
Arrhenius Base | A substance that increases th 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 formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor. |
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 Bronsted-Lowry base gains a proton. |
Conjugate base | The species that remains after a Bronsted-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 o 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 a 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). |