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TEP-AcidsandBases
| 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 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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