1. Warm-Up Find the Molarity of the following.
If 22.4 g of NaOH is contained in 700. mL of solution
If 600. mL of 6.0 M HCl is diluted to 1.5 L

2. Follow along in your text Chapters 14 & 15
What are Acids & Bases?
Follow along in your text Chapters 14 & 15

3. Properties ACIDS BASES electrolytes  electrolytes sour taste
bitter taste
turn litmus red
turn litmus blue
react with metals to form H2 gas
slippery feel
vinegar, milk, soda, apples, citrus fruits
ammonia, lye, antacid, baking soda
ChemASAP

4. HCl + H2O  H3O+ + Cl– Definitions – +
Arrhenius - In aqueous solution…
Acids form hydronium ions (H3O+)
HCl + H2O  H3O+ + Cl– H Cl O – +
acid

5. NH3 + H2O  NH4+ + OH- Definitions – +
Arrhenius - In aqueous solution…
Bases form hydroxide ions (OH-)
NH3 + H2O  NH4+ + OH- H N O – +
base

6. HCl + H2O  Cl– + H3O+ Definitions acid conjugate base base
Brønsted-Lowry
Acids are proton (H+) donors.
Bases are proton (H+) acceptors.
HCl + H2O  Cl– + H3O+
acid
conjugate base
base
conjugate acid

7. Definitions
H2O + HNO3  H3O+ + NO3– B A CA CB

8. Amphoteric - can be an acid or a base.
Definitions
NH3 + H2O  NH4+ + OH- B A CA CB
Amphoteric - can be an acid or a base.

9. Polyprotic - an acid with more than one H+
Definitions
Give the conjugate base for each of the following: HF
H3PO4
H3O+
F -
H2PO4-
H2O
Polyprotic - an acid with more than one H+

10. Br - HSO4- CO32- HBr H2SO4 HCO3- Definitions
Give the conjugate acid for each of the following:
Br -
HSO4-
CO32-
HBr
H2SO4
HCO3-

11. Definitions Lewis Acids are electron pair acceptors.
Bases are electron pair donors.
Lewis base
Lewis acid

12. Strength Strong Acid/Base 100% ionized in water strong electrolyte HCl- +
HCl
HNO3
H2SO4
HBr HI
HClO4
NaOH
KOH
Ca(OH)2
Ba(OH)2

13. Strength Weak Acid/Base does not ionize completely weak electrolyte HF- + HF
CH3COOH
H3PO4
H2CO3
HCN
NH3

14. Follow along in your text Chapter 15 Section2 Pages 539 -547
The pH Scale
Follow along in your text Chapter 15 Section2 Pages

15. H2O + H2O H3O+ + OH- Kw = [H3O+][OH-] = 1.0  10-14
Ionization of Water
Hydronium Ion
H2O + H2O H3O+ + OH-
Kw = [H3O+][OH-] = 1.0  10-14

16. Ionization of Water
Find the hydroxide ion concentration of 3.0  10-2 M HCl.
[H3O+][OH-] = 1.0  10-14
[3.0  10-2][OH-] = 1.0  10-14
[OH-] = 3.3  M
Acidic or basic?
Acidic
Hint: [H3O+] > [OH-]

17. pouvoir hydrogène (Fr.)
pH Scale 14 7
INCREASING
ACIDITY
INCREASING
BASICITY
NEUTRAL
pH = -log[H3O+]
pouvoir hydrogène (Fr.)
“hydrogen power”

18. pH of Common Substances
pH Scale
pH of Common Substances

19. pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14 [H3O+] = 10-pH
pH Scale
pH = -log[H3O+]
pOH = -log[OH-]
pH + pOH = 14
[H3O+] = 10-pH
[OH-] = 10-pOH

20. pH Scale What is the pH of 0.050 M HNO3? pH = -log[H3O+]
Acidic or basic?
Acidic

21. pH Scale
What is the molarity of HBr in a solution that has a pOH of 9.6?
pH + pOH = 14
pH = 14
pH = 4.4
pH = -log[H3O+]
So [H3O+] = 10-pH
[H3O+] =
[H3O+] = 4.0  10-5 M HBr
Acidic

22. ACID + BASE  SALT + WATER
Neutralization
Chemical reaction between an acid and a base.
Products are a salt (ionic compound) and water.
ACID + BASE  SALT + WATER
Neutralization does not mean pH = 7.

23. Neutralization HC2H3O2 + NaOH  NaC2H3O2 + H2O
Salts can be neutral, acidic, or basic.
HCl + NaOH  NaCl + H2O
strong
strong
neutral
HC2H3O2 + NaOH  NaC2H3O2 + H2O
weak
strong
basic

24. Titration
standard solution
unknown solution
Titration
Analytical method in which a standard solution is used to determine the concentration of an unknown solution.

25. Titration Equivalence point (endpoint)
Point at which equal amounts of H3O+ and OH- have been added.
Determined by…
indicator color change
dramatic change in pH

26. pH Indicators Indicator Type pH Range Color Changes Methyl Violet
-2 – 3
Yellow to Violet
Thymol Blue
0 – 4.5
6 – 11
Red to Yellow
Yellow to Blue
Methyl Orange
2 – 6
Methyl Red
4 – 8
Litmus
3.5 – 9.5
Red to Blue
Bromothymol Blue
4 – 8.5
Phenolphthalein
Colorless to Pink
Alizarin Yellow R
8 – 13
Yellow to Red

27. Titration

28. moles H3O+ = moles OH- MV n = MV n Titration M: Molarity V: volume
n: # of H+ ions in the acid or # of OH- ions in the base

29. Titration
42.5 mL of 1.3M KOH are required to neutralize 50.0 mL of H2SO4. Find the molarity of H2SO4.
H3O+
M = ?
V = 50.0 mL
n = 2
OH-
M = 1.3M
V = 42.5 mL
n = 1
MV# = MV#
M(50.0mL)(2)
=(1.3M)(42.5mL)(1)
M = 0.55M H2SO4