1. I. Introduction to Acids & Bases
Ch. 19 – Acids & Bases
I. Introduction to Acids & Bases

2. Review – Acid Nomenclature

3. Review – Acid Nomenclature

4. Review – Naming Acids HCl Hydrochloric acid H2S Hydrosulfuric acid
H2SO4
H2SO3
HNO3
HNO2
HBr
Hydrochloric acid
Hydrosulfuric acid
Sulfuric acid
Sulfurous acid
Nitric acid
Nitrous acid
Hydrobromic acid

5. A. 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

6. HF H3PO4 H2SO4 B. Definitions monoprotic triprotic diprotic polyprotic
Monoprotic – an acid with one H+
Polyprotic – an acid with more than one H+
Diprotic – an acid with 2 H+
Triprotic – an acid with 3 H+ HF
H3PO4
H2SO4
monoprotic
triprotic
diprotic
polyprotic

7. HCl + H2O  H3O+ + Cl– B. Definitions – + Arrhenius
Acids contain hydrogen
Acids form hydronium ions (H3O+) in aqueous solution
HCl + H2O  H3O+ + Cl– H Cl O – +
acid

8. NaOH  Na+ + OH- B. Definitions Arrhenius
Bases contain a hydroxide group
Bases form hydroxide ions (OH-) in aqueous solution
H2O
NaOH  Na+ + OH-
base

9. HCl + H2O  Cl– + H3O+ B. 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

10. HBr + NaOH  NaBr + H2O B. Definitions acid conjugate base base
Brønsted-Lowry
Conjugate Acids are the result after a base accepts a hydrogen ion
Conjugate Bases are the result after an acid donates a hydrogen ion
HBr + NaOH  NaBr + H2O
acid
conjugate base
base
conjugate acid

11. Amphoteric – can be an acid or a base
B. Definitions
H2O + HNO3  H3O+ + NO3– B A CA CB
H2O + NH3  NH4+ + OH- A B CA CB
Amphoteric – can be an acid or a base

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

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

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

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

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

17. Ch. 19 – Acids & Bases
II. pH (p. 644 – 658)

18. pH water equilibrium
Pure water ionizes to a small extent to produce hydrogen ions and hydroxide ions
According to LeChatlier’s principle if an acid is dissolved in water the equilibrium will shift to the left decreasing the hydroxide ion concentration.
If a base is dissolved in water this decreases the hydrogen ion concentration.

19. Self-Ionization of Water
A. Ionization of Water
H2O (l)+ H2O (l) H3O+(aq)+ OH- (aq)
Self-Ionization of Water

20. Kw = [H3O+][OH-] = 1.0  10-14 A. Ionization of Water
Ion Product Constant for Water
The ion production of water, Kw = [H3O+][OH–]
Pure water contains equal concentrations of H+ and OH– ions, so [H3O+] = [OH–]
For all aqueous solutions, the product of the hydrogen-ion concentration and the hydroxide-ion concentration equals 1.0 x 10-14

21. A. Ionization of Water
Find the hydroxide ion concentration of 3.0  10-2 M HCl.
HCl → H Cl-
3.0  10-2M  10-2M
[H3O+][OH-] = 1.0  10-14
[3.0  10-2][OH-] = 1.0  10-14
[OH-] = 3.3  M

22. A. Ionization of Water
Find the hydronium ion concentration of 1.4  10-3 M Ca(OH)2.
Ca(OH)2 → Ca OH-
1.4  10-3M  10-3M
[H3O+][OH-] = 1.0  10-14
[H3O+][2.8  10-3] = 1.0  10-14
[H3O+] = 3.6  M

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

24. pH of Common Substances
B. pH Scale
pH of Common Substances

25. pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14
B. pH Scale
pH = -log[H3O+]
pOH = -log[OH-]
pH + pOH = 14

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

27. B. pH Scale What is the pH of 0.050 M Ba(OH)2? [OH-] = 0.100 M
pOH = -log[OH-]
pOH = -log[0.100]
pOH = 1.00
pH = 13.00
Acidic or basic?
Basic

28. B. pH Scale
What is the molarity of HBr in a solution that has a pOH of 9.60?
pH + pOH = 14
pH = 14
pH = 4.40
pH = -log[H3O+]
4.40 = -log[H3O+]
-4.40 = log[H3O+]
[H3O+] = 4.0  10-5 M HBr
Acidic