1. Descriptions & Reactions
Acids & Bases
Descriptions & Reactions

2. HCl + H2O  H3O+ + Cl– Descriptions – +
Arrhenius - In aqueous solution…
Acids form hydrogen ions (H+) or hydronium ions (H3O+)
HCl + H2O  H3O+ + Cl– H Cl O – +
acid

3. NH3 + H2O  NH4+ + OH- Descriptions – +
Arrhenius - In aqueous solution…
Bases form hydroxide ions (OH-)
NH3 + H2O  NH4+ + OH- H N O – +
base

4. Another common way to refer to hydrogen ions is to call them “protons”
Descriptions
Another common way to refer to hydrogen ions is to call them “protons”
Brønsted-Lowry
Acids are proton (H+) donors.
Bases are proton (H+) acceptors.
HCl + H2O  Cl– + H3O+
acid
conjugate base
base
conjugate acid
Conjugate acid – particle formed when a base gains a H+
Conjugate base – particle that remains when an acid has donated a H+

5. Descriptions Lewis Lewis base Lewis acid
Acids are electron pair acceptors.
Bases are electron pair donors.
Lewis base
Lewis acid

6. Descriptions Strong Acid/Base Ionize completely in water- +
Strong Acid/Base
Ionize completely in water
strong electrolyte
HCl
HNO3
H2SO4
HBr HI
HClO4
NaOH
KOH
Ca(OH)2
Ba(OH)2

7. Descriptions Weak Acid/Base ionize partially in water weak electrolyte- +
Weak Acid/Base
ionize partially in water
weak electrolyte HF
CH3COOH
H3PO4
H2CO3
HCN
NH3

8. Neutralization Chemical reaction between an acid and a base.
Products are a salt (ionic compound) and water.

9. ACID + BASE  SALT + WATER
Neutralization
ACID + BASE  SALT + WATER
HCl + NaOH  NaCl + H2O
strong
strong
neutral
HC2H3O2 + NaOH  NaC2H3O2 + H2O
weak
strong
basic