| A | B |
|---|
| electrolyte | any substance that ionizes to conduct electricity |
| neutralization reaction | a reaction between an acid and a base that produces a salt and water |
| Arrhenius acid | a substance that releases H+ |
| Arrhenius base | a substance that releases OH- |
| Bronsted-Lowry acid | proton donator |
| Bronsted-Lowry base | proton acceptor |
| deprotonation | the process of losing a proton |
| protonation | the process of gaining a proton |
| conjugate pair | two particles that differ from each other by only a hydrogen ion |
| conjugate acid | the structure formed when a base is protonated |
| conjugate base | the structure formed when an acid has donated a proton |
| Lewis acid | electron pair acceptor |
| Lewis base | electron pair donor |
| self-ionization of water | the process by which one water molecule donates a proton to another water molecule |
| ionization constant of water | Kw = [H3O+][OH-] = 1x10^-7 |
| pH | -log[H3O+] |
| acidic solution | a solution with pH<7 |
| basic solution | a solution with pH>7 |
| neutral solution | a solution with pH=7 |
| pOH | -log[OH-] |
| strong acid | a substance that gives up protons easily and ionizes completely |
| weak acid | a substance that does not give up protons easily and does not ionize completely |
| strong base | a substance that readily accepts protons |
| acid-ionization constant | Ka = [H3O+][A-]/[HA] |
| base-ionization constant | Kb = [OH-][HB+]/[B] |
| amphoteric | able to act as both a Bronsted-Lowry acid and a Bronsted-Lowry base |
| monoprotic | able to donate one proton |
| polyprotic | able to donate more than one proton |
| diprotic | able to donate two protons |
| triprotic | able to donate three protons |
| indicator | a substance whose color is sensitive to pH |
| transition interval | the pH range over which an indicator changes color |
| salt | a substance formed from the anion of an acid and the cation of a base |
| titration | a controlled neutralization reaction in which an unknown concentration is determined |
| titration curve | a graph that shows how pH changes as an acid or base is added to a solution |
| equivalence point | the point in a titration at which [OH-]=[H3O+] |
| end point | the point at which a change is detected in a titration |
| buffer | a solution that resists changes to pH |
| irreversible reaction | a reaction that proceeds in only one direction |
| reversible reaction | a reaction in which the products can change back into the reactants |
| chemical equilibrium | the state of balance attained in a reversible reaction in which the forward and reverse reactions proceed at the same rate |
| equilibrium constant | a numerical expression of the ratio of the products to the reactants at equilibrium |
| homogeneous equilibrium | a chemical system in which all of the reactants and products are at equilibrium and are in the same state |
| heterogeneous equilibrium | a chemical system at equilibrium in which two or more states are represented |
| LeChatelier's principle | When a reversible process is disturbed, it will proceed in the direction that relieves the stress |
| Haber process | the industrial preparation of ammonia from hydrogen and nitrogen gases at high temperatures and pressures with a catalyst |
| common-ion effect | an equilibrium phenomenon in which two or more substances dissolve and release a common ions, thereby decreasing the ionization of the weaker electrolyte |
