1. Acids
and
Bases

2. Definitions Acids – produce H+ Bases - produce OH- Acids – donate H+
Bases – accept H+
Arrehenius
Bronsted-Lowry

3. Examples HCl Lemon Juice Soda NaOH Bleach Soap H2SO4 Acid Rain Vinegar
Acids
HCl
Lemon Juice
Soda
NaOH
Bleach
Soap
H2SO4
Acid Rain
Vinegar
KOH
Ammonia
M.O.M
Bases

4. Properties of Acids pH < 7.0 Taste Sour React with metals
Turn litmus paper red

5. Properties of Bases pH > 7.0 Taste Bitter Slippery, soapy feeling
Turn litmus paper blue

6. Acids & Bases
Conduct electricity (electrolytes)
React with indicators

7. Indicators Universal Indicator
Chemicals which change colors when they are put into acids or bases.

8. Acid + Base  Water + Ionic Compound
Acid/Base Reactions
(Neutralization Reactions)
Acid + Base  Water + Ionic Compound
HCl KOH 
HOH
+ KCl
H2SO KOH 
2H2O
+ K2SO4

9. What is pH?
measures the concentration of H+ ions (How acidic or basic a solution is)
pH = -log[H+]
If [H+] = 1 x 10-4, then pH = 4
If [H+] = 1 x 10-13, then pH = 13
If [H+] = 1 x 10-7, then pH = 7

10. pH Scale Acid Neutral Base H+ OH- 1 2 3 4 5 6 7 8 9 10 11 12 13 141 2 3 4 5 6 7 8 9 10 11 12 13 14
Urine
Blood
Saliva
Bleach
Ammonia
Sea Water
Pure Water
Baking Soda
Gastric Juice
Tomato Juice
Black Coffee
Milk of Magnesia
Battery Acid, HCl
Orange Juice, Soda
Lemon Juice, Vinegar
Liquid Draino, NaOH

11. pH and pOH [H+][OH-] = 10-14 pH + pOH = 14
If [OH-] = 10-8 M, what is the pH?
the pOH = 8, so the pH must be 14 – 8
So the pH = 6