1. Acids and Bases
Chapter 19

2. Characteristics of Acids
Sour tasting – vinegar, lemons
React with metals and produce H2 (g)
React with metal carbonates to produce CO2
Blue Litmus Paper  Red
Conductive
H+ ions > OH- ions
pH < 7

3. Characteristics of Bases
Bitter tasting (soap)
Slippery
Red Litmus Paper  Blue
Conductive
OH- ions > H+ ions
pH > 7

4. Pure Water is Neutral

5. Arrhenius Acid
Donates a H+ ion in an aqueous solution

6. Model doesn’t explain why ammonia is a base.
Arrhenius Base
Donates a OH- in an aqueous solution
Model doesn’t explain why ammonia is a base.

7. Bronsted-Lowry Model
Acid – donates a H+
Base –accepts a H+

8. Forms when the base accepts a H+ ion
Forms when the acid donates a H+ ion to a base

9. Conjugate Acid? Conjugate Base?
Which is the acid? Base?
Conjugate Acid? Conjugate Base?

10. Bronsted-Lowry Expands the range of acids and bases.
Amphoteric – acts as an acid and a base (water)

11. Monoprotic and Polyprotic Acids
Mono – donates only one H+
HCl, HNO3, CH3COOH
Not covalently bonded, ionizable
Poly – donates more than one H+
Diprotic – H2SO4
Triprotic – H3PO4

12. Phosphoric Acid is triprotic

13. Acid Strength Strong acids completely ionize
Weak acids do not completely ionize

15. Base Strength
Strong Bases dissociate into metal ions and hydroxide ions
Weak base partially ionizes in dilute aqueous solutions

16. Strong Base
Weak Acid

17. What is pH?