1. Chapter 19
Acids and Bases

2. TEKS
(G) define acids and bases and distinguish between Arrhenius and Bronsted-Lowry definitions and predict products in acid base reactions that form water;
(H) understand and differentiate among acid-base reactions, precipitation reactions, and oxidation-reduction reactions;
(I) define pH and use the hydrogen or hydroxide ion concentrations to calculate the pH of a solution; and

3. Properties of Acids and Bases
Tastes sour
reacts with metals to produce hydrogen gas
Reacts with carbonates to produce carbon dioxide
conducts electricity so are good electrolytes
Turns blue litmus red
Has a pH between 0-6
Reacts with a base to produce salt and water
Tastes bitter
Slippery
conducts electricity
Turns red litmus blue
Reacts with an acid to produce salt and water
Has a pH above 7

4. Ions in Solution contains more H+ ions than OH- ions H+ > OH-
Acidic Solution
Neutral solutions
Basic Solution
contains more H+ ions than OH- ions
H+ > OH-
neither acidic or basic
equal # of H+ and OH- ions
H+ = OH-
contains more OH- ions than H+ ions
H+ < OH-

5. Arrhenius vs Bronstead-Lowry
an acid is a substance that ionizes to produce hydrogen ions in aqueous solution
States that an acid is a hydrogen-ion donor
a base dissociates to produce a hydroxide ion in aqueous solution
a base is a hydrogen-ion acceptor

6. Amphoteric Substances
Amphoteric- a substance that can act as both acids and bases
Ex: Water
When HF dissolves in water, water acts as base
When NH3 dissolves in water, water acts as acid

7. Strong Acids vs Weak Acids

8. 19.2 Strengths of Acids Strong Acids Weak Acids
acid that ionizes completely
acid that ionizes only partially in dilute aqueous solutions
Ex: HC2H3O2, H2CO3
Good conductors of electricity, makes great electrolytes
Ex: HCl, HNO3, H2SO4
Poor conductors of electricity
Reactions shown with 
Reactions shown with >

9. Strong Base vs Weak Base

10. 19.2 Strengths of Bases Strong Base Weak Base
dissociate completely into metal ions and hydroxide ions
Ex: NaOH, Ca(OH)2
ionizes only partially in dilute aqueous solutions to form conjugate acid of the base and hydroxide ion
Ex: CH3NH2

11. 19.3 What is pH? Pure water contains equal numbers of H+ and OH- ions
Kw = [H+] [OH-]
Use 1.0x10-14 M for Kw

12. Ion Product Constant of Water
Ion Product Constant of Water- Kw- the value of the equilibrium constant for water
At 298 K, Kw is 1.0 x 10-14
Kw = [H+] [OH-]

13. pH pH- the negative logarithm of the hydrogen ion concentration
pH = -log [H+]

14. Math Calculations pH + pOH = 14 pH= -log(H+)
pH when given pOH = 14- (-log OH)

15. pH Scale
pH below 7 is an acid
pH above 7 is a base
pH = 7 is neutral

16. pH of Common Substances
Timberlake, Chemistry 7th Edition, page 335

18. pH Scale

19. 19.4 Neutralization
Neutralization Reaction- acid & base react to produce a salt & water
a Double-Replacement Reaction
Salt- an ionic compound formed from the cation of a base & anion of an acid

20. Acid-Base Indicator- a compound that changes color as it is placed in either an acid or base

22. Titration
The process in which an acid-base neutralization reaction is used to determine the concentration of a solution of unknown concentration.

23. End Point
The point at which an indicator used in a titration changes color

24. Buffers
A solution that resists changes in pH when limited amounts of acids and bases are added.