12.1 Introduction to Acids and Bases
| ARRHENIUS | BRONSTED-LOWRY | PROPERTIES | |
|---|---|---|---|
| ACID | H+ donor in H2O (increases [H3O+]) | H+ donor | Turn litmus red, sour |
| BASE | OH- donor in H2O (increases [OH-]) | H+ acceptor | Turn litmus blue, bitter, slippery |
Acid-Base Neutralization Reactions
Bronsted-Lowry acids and bases may or may not form water. (Identify conjugate acid/base pairs.)
Amphiprotic – a substance that can act as either a Bronsted-Lowry acid or base (ex. HSO4-, H2O, HCO3-)
Identify the conjugate acid of HCO3-.
Identify the conjugate base of HCO3-.
| STRONG ACIDS | STRONG BASES |
|---|---|
| HI HBr HCl H2SO4 HNO3 HClO4 HClO3 | LiOH NaOH KOH RbOH CsOH Ba(OH)2 Sr(OH)2 Ca(OH)2 Mg(OH)2 |
Strong acids and bases dissociate/ionize/hydrolyze completely in water. Any acid that is not strong is weak by default (ex. HF, HNO2, HCN, etc.). Weak bases include NH3.