| A | B |
|---|
| Amphoteric | A substance the can act as an acid or a base. |
| Arrhenius Acid/Base Definition | Acid: produces H+ in solution, Base: produces OH- in solution |
| Bronsted-Lowry Acid/Base Definition | Acid: H+ donor, Base: H+ acceptor. |
| Lewis Acid/Base Definition - | Acid: electron pair acceptor, Base: electron pair donor. |
| conjugate | a subspecies of a substance |
| Dissociation | Ionic compound becoming ions in solution |
| Ionization | A covalent compound becoming ions in solution. |
| Alkaline | Having properties of a base. |
| Ion-Product Constant | Expresses the degree of dissociation for a compound. |
| Neutral | A solution where the [H+] = [OH-] |
| Auto-Ionization | The "breaking" into H+ and OH- that occurs in water by the action of itself. |
| pH | A measure of H+ concentration. (pH = -log[H+]) |
| Molarity | molessolute /liter of solution |
| Normality | moles eqivalents/liter of solution |
| Molality | moles solute/kg solvent |
| Equivalence Point | When [H+] = [OH-] |
| Neutralization | A double replacement reaction between an acid and a base. |
| Standard | A solution of known concentration. |
| Titration | An method that uses the relative concentrations and amounts to analyze and unkown. |
| Buffer | A substance that resists change. |
| Salt | The combination of the cation from a base and the anion form a acid. |
