1. Acids
and
Bases

2. Properties of Acids  A dilute acid tastes sour.
 When a reactive metal is added to an acid it produces H2(aq)
 When an acid is tested with Litmus paper, the paper turns red.
 When phenolphthalein is added to an acid, no reaction occurs.
 Acids are electrolytes.
 When an acid and a base are added together the products are water and salt.

3. Properties of Bases  A dilute base tastes bitter.
 If a metal oxide and water are combined a base is formed.
 When a base is tested with Litmus paper, the paper turns blue.
 When phenolphthalein is added to a base, the base turns pink.
 Bases are electrolytes.
 When an acid and a base are added together the products are water and salt.

4. Arrhenius Acid An acid is anything that releases H+ in solution.
Example:
HCl(aq)  H+(aq) + Cl-(aq)
HBr, HF, HI, H2SO4, HNO3, H3PO4, H2CO3, CH3COOH

5. A base is anything that releases OH- in solution.
Arrhenius Bases
A base is anything that releases OH- in solution.
Example:
NaOH(aq)  Na+(aq) + OH-(aq)
NaOH, KOH, LiOH, Sr(OH)2

6. Neutralization
 occurs when in acid-base reactions equal quantities of an acid and base are mixed.
 the products are salt and water
 the products are neither acid nor base which makes them neutral
Example:
HCl + NaOH  NaCl + H2O

7. Titration
Titration is the process of metering a standard solution into a solution of unknown concentration.
Formula: MA x VA = MB x VB
If 50.0mL of 1M KOH is used, how much 2M HCl is needed to titrate this reaction?
2M x X = 1M x 50.0mL
X = 25.0mL

8. A Bronsted-Lowry base is anything that accepts a proton.
Bronsted-Lowry Acid
A Bronsted-Lowry acid is anything that donates a proton.
Bronsted-Lowry Base
A Bronsted-Lowry base is anything that accepts a proton.

9. Examples
HCl + NH3 --> NH4+ + Cl Acid Base Acid Base
HCl + H2O --> H3O+ + Cl- Acid Base Acid Base
NH3 + H2O --> NH4+ + OH- Base Acid Acid Base
Water can either be an acid or a base. Water is therefore an amphoteric substance.

10. Conjugate Acid-Base pairs
Conjugate acid-base pair: in an acid-base reaction, an acid transfers a proton to become a conjugate base, this acid and the newly formed base form an acid-base pair.
Example:
HCl + NH3 --> NH4+ + Cl- Acid Base Acid Base
HCl and Cl- are an acid-base pair and NH3 and NH4+ are an acid-base pair in this equation.

11. pH H2O + H2O --> H3O+ + OH- Kw = [H3O+][OH-] Kw = 1 x 10-14
pH = -log[H3O+]
7 = -log[1 x 10-7]
HCl + H2O  H3O+ + Cl-
1 x 10-3M x 10-3M
pH = 3
NaOH  Na+ + OH-
.01M 1 x 10-2
pH = 12

12. Strong Acids Strong BasesHI
HBr
HCl
HNO3
H2SO4
HClO4
LiOH
NaOH
KOH
RbOH
CsOH

13. Hydrolysis
Hydrolysis is a process by which some salts react with water to form solutions that are acidic or basic.
Examples:
NaCl + H2O  HCl + NaOH Neutral
NaF + H2O  HF + NaOH Basic
MgCl2 + H2O  HCl + Mg(OH)2 Acidic

14. THE
END