16.1 Introduction to Acids and Bases
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PRE-HEALTH PREP
PRE-HEALTH PREP
Table of Contents
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| ARRHENIUS | BRONSTED-LOWRY | LEWIS | |
|---|---|---|---|
| ACID | ↑ [H3O+] in H2O | H+ donor | Electron acceptor |
| BASE | ↑ [OH-] in H2O | H+ acceptor | Electron donor |
Conjugate Acid/Base Pairs
Determine the missing conjugate acids or bases in the following table.
| CONJUGATE ACID | CONJUGATE BASE |
|---|---|
| HCl | |
| NH3 | |
| HCO3- | |
| HCO3- | |
| OH- | |
| OH- |
Amphiprotic – describes a chemical species that can act as a Bronsted-Lowry acid or base
Strong Acids and Strong Bases
Strong acids and bases dissociate/ionize/hydrolyze completely in water.
| STRONG ACIDS | STRONG BASES |
|---|---|
| HClO4 | LiOH |
| H2SO4 | NaOH Mg(OH)2 |
| Hl | KOH Ca(OH)2 |
| HBr | RbOH Sr(OH)2 |
| HCl | CsOH Ba(OH)2 |
| HNO3 | |
| HClO3 |