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TEP-AcidsandBases

QuestionAnswer
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 process; any process that results from 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 a 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 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 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 a compound of hydrogen, oxygen, and a third element, usually a nonmetal
BrØnsted-Lowery reaction the transfer of protons from one reactant (the acid) to another (the base)
Created by: Tessa Elise
 

 



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