1. ACIDS AND BASES
Chapters 15 and 16

2. Acids
H (Hydronium – H3O+)
pH less than 7
Sour taste
Corrosive
Conduct electric current
Ionization
Bases
OH (Hydroxide)
pH greater than 7 (alkaline)
Bitter taste/slippery
Corrosive
Conduct electric current
Dissociation

3. COMMON ACIDS
Acetic acid – vinegar
Juices/citrus fruit
Sulfuric acid
– car batteries
Nitric acid
- fertilizer/explosive
Hydrochloric acid
- Stomach
- pool cleaner (muriatic acid)
COMMON BASES
Ammonia – NH3
KOH – soap
NaOH – drain opener
Antacids

4. Indicators
Acid Base Litmus paper red blue Phenolphthalein (phth) clear bright pink Bromothymol blue yellow blue Universal indicator red-yellow blue-purple

5. Neutralization Reactions
A reaction between an acid and a base
Produces water and a salt.

6. Arrhenius acid – Increases concentration of Hydrogen (H+) or Hydronium ions (H3O+). Arrhenius base – Increases concentration of Hydroxide ions (OH-).

7. HCl + NH3 → NH4+ + Cl- Bronsted-Lowry acid – Proton donor
Bronsted-Lowry base – Proton acceptor
HCl NH3 → NH Cl-

8. STRENGTH VS. How completely it ionizes or dissociates
STRENGTH VS. How completely it ionizes or dissociates. (will not change) Acids – ionize Bases - dissociate
CONCENTRATION Measurement of how much acid or base is in a solution. (can be changed)

9. pH is the potential of hydrogen – measures concentration of H+ in a solution [H+]
Changes by a multiple of 10
pH scale of 0-14 – Logarithms are used to simplify scale
Examples
10 versus 9
1 versus 3
6 versus 3

10. Acids **Balance charges **Do not name “Hydrogen”
Hydro _____________ic __________________ic __________________ous
“ide” like Cl
“ate” like ClO3
“ite” like ClO2