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Acid Base Chemistry
| Term | Definition |
|---|---|
| Arrhenius Base | Hydroxide ion producer |
| Arrhenius Acid | Hydrogen ion producer |
| Lewis Acid | electron acceptor |
| Lewis Base | electron donor |
| Bronsted Lowery Acid | H+ donor |
| Bronsted Lowery Base | H+ acceptor |
| Strong acid or base | equilibrium lies far to the right (completely dissociates) |
| Weak acid or base | equilibrium lies far to the left (mostly stays intact) |
| pH of an acid | 0-6.9 |
| pH of a base | 7.1-14 |
| neutral pH | 7 |
| carboxylic acids are typically (strong or weak) | weak |
| H+ concentration of a strong acid | [H+]=[HA] |
| increase of H+ causes pH to | decrease |
| Ka of a strong acid is (large or small) | large |
| Ka of a weak acid is (large or small) | small |
| amphoteric | a substance that can be an acid or a base |
| Kw | the dissociation constant for water |
| value of Kw for pure water at 25oC | 1.0 x 10^-14 |