| A | B |
|---|
| Acid | a compound that produces hydrogen ions in solution, is a hydrogen-ion donor, or an electron-pair acceptor |
| Base | a compound that produces hydroxide ions in solution, is a hydrogen-ion acceptor, or an electron-pair donor |
| Hydroxide Ion | (OH-) the negative ion formed when a water molecule loses a hydrogen ion |
| Hydronium Ion | (H3O+) the positive ion formed when a water molecule gains a hydrogen ion; all hydrogen ions in aqueous solution are this |
| Neutral Solution | an aqueous solution in which the concentrations of hydrogen and hydroxide ions are equal, that is, 1.0 x 10^-7 mol/L; it has a pH of 7 |
| Acidic Solution | any solution in which the hydrogen ion concentration is greater than the hydroxide ion concentration |
| Basic Solution | any solution in which the hydroxide ion concentration is greater than the hydrogen ion concentration |
| Alkaline Solutions | a basic solution |
| pH | a number used to denote the hydrogen ion concentration, or acidity, of a solution; it is the negative logarithm of the hydrogen ion concentration of a solution |
| Monoprotic Acids | any acid that contains one ionizable proton (hydrogen ion); nitric acid (HNO3) |
| Diprotic Acids | any acid that contains 2 ionizable protons (hydrogen ions); sulfuric acid (H2SO4) |
| Hydrogen-Ion Donor | an acid, according to the Bronsted-Lowry theory |
| Amphoteric | a substance that can act as both an acid and a base; water is an example of this |
| Strong Acids | an acid that is completely (or almost completely) ionized in aqueous solution |
| Weak Acids | an acid that is only slightly ionized in aqueous solution |
| Strong Bases | a base that completely dissociates into metal ions and hydroxide ions in aqueous solution |
| Weak Bases | a base that does not dissociate completely in aqueous solution |
