1. PROPERTIES OF ACIDS & BASES
CHAPTER 15
PROPERTIES OF ACIDS & BASES

2. WHAT IS AN ACID?
A compound that donates a hydrogen ion (H+) when dissociated

3. Chapter 15 Acids, continued Acids Generate Hydronium Ions, continued
Section 1 What Are Acids and Bases?
Chapter 15
Acids, continued
Acids Generate Hydronium Ions, continued

4. ACID PROPERTIES aqueous solutions have a sour taste
change the color of acid-base indicators
when reacted with an active metal, releases hydrogen gas
Zn (s) + H2SO4 (aq)  ZnSO4 (aq) + H2 (g)

5. ACID PROPERTIES when reacted with base, produces salt and water
HCl (aq) + NaOH (aq)  NaCl (s) + H2O (l)
conduct electric current
Turns litmus paper red

6. Strength and Weakness of Acids and Bases
Chapter 15
Visual Concepts
Strength and Weakness of Acids and Bases

7. STRONG VS. WEAK ACIDS Strong acids dissociate completely
Every H+ ion breaks off
Weak acids dissociate incompletely
A few H+ ions break off then reform

8. WHAT IS A BASE? A compound that accepts a hydrogen ion (H+)
contains OH- ion

9. Section 1 What Are Acids and Bases?
Chapter 15
Bases, continued

10. BASE PROPERTIES aqueous solutions of bases have a bitter taste
bases change the color of acid base indicators
dilute aqueous solutions of bases feel slippery

11. BASE PROPERTIES when reacted with acid, produces salt and water
conduct electric current
Turns litmus paper blue

12. Relationship between [H3O+] and [OH-]
Section 1 What Are Acids and Bases?
Chapter 15
DO NOW!
Copy this chart on page NB75
Relationship between [H3O+] and [OH-]

13. DIFFERENT DEFINITIONS
SHOULD BE MEMORIZED

14. Arrhenius Acids and Bases
Chapter 15
Visual Concepts
Arrhenius Acids and Bases

15. ARRHENIUS
ACID
A chemical compound that increases the concentration of H+ ions in solution
Good for calculating pH
BASE
A chemical compound that increases the concentration of OH- ions in solution
Good for calculation pOH
Limited to bases containing OH-

16. Brønsted-Lowry Classification, continued
Section 1 What Are Acids and Bases?
Chapter 15
Brønsted-Lowry Classification, continued
Brønsted-Lowry Acids Donate Protons, continued

17. Brønsted-Lowry Acids and Bases
Chapter 15
Visual Concepts
Brønsted-Lowry Acids and Bases

18. BRONSTED-LOWRY ACID A molecule or ion that is a proton (H+) donor BASE
A molecule or ion that is a proton (H+) acceptor
Includes compounds w/o OH-

19. Why don’t we like this definition?
LEWIS
ACID
Electron pair acceptor
BASE
Electron pair donator
Why don’t we like this definition?

20. Acid-Base Titrations and pH

21. pH
pH < 7 is acidic
pH = 7 is neutral
pH > 7 is basic

24. [H+] = concentration of protons
Calculating pH
pH = - log [H+]
pH = power of Hydrogen
[H+] = concentration of protons

25. Calculating pOH pOH = - log [OH-] pOH = power of Hydroxide
[OH-] = concentration in Normality
pH + pOH = 14

26. CALCULATING pH FROM CONCENTRATION

27. SAMPLE PROBLEM A
What is the pH of a 1 x 10-3 M HCl solution?

28. SAMPLE PROBLEM A What is the pH of a 1.0 x 10-3 M HCl solution?
Step 1:
Convert from M to N.
N = (1.0 x 10-3) (1)
N = 1.0 x 10-3

29. SAMPLE PROBLEM A What is the pH of a 1.0 x 10-3 M HCl solution?
Step 2:
Plug-in.
pH = - log [H+]
pH = - log (1.0 x 10-3)
pH = 3

30. SAMPLE PROBLEM B
What is the pH of a 2.5 x 10-2 M H2SO4 solution?

31. SAMPLE PROBLEM B What is the pH of a 2.5 x 10-2 M H2SO4 solution?
Step 1:
Convert from M to N.
N = (0.025) (2)
N = 0.050

32. SAMPLE PROBLEM B What is the pH of a 2.5 x 10-2 M H2SO4 solution?
Step 2:
Plug-in.
pH = - log [H+]
pH = - log (0.050)
pH = 1.3

33. SAMPLE PROBLEM C
What is the pH of a 2.5 x 10-2 M NaOH solution?

34. SAMPLE PROBLEM C What is the pH of a 2.5 x 10-2 M NaOH solution?
Step 1:
Convert from M to N.
N = (0.025) (1)
N = 0.025

35. SAMPLE PROBLEM C What is the pH of a 2.5 x 10-2 M NaOH solution?
Step 2:
Plug-in.
pOH = - log [OH-]
pOH = - log (0.025)
pOH = 1.6

36. SAMPLE PROBLEM C What is the pH of a 0.025 M NaOH solution? Step 3:
Solve for pH.
pH + pOH = 14
pH = 14
pH = 12.4

37. CALCULATING CONCENTRATION FROM pH

38. [H3O+] [H3O+] = 10-pH [H3O+] = concentration of acid (N)
Look for your log button.
Above it – 10x
To access it,
hit 2nd F key
Hit log key

39. The Self-Ionization of Water, continued
Chapter 15
Section 2 Acidity, Basicity, and pH
The Self-Ionization of Water, continued
The Self-Ionization Constant of Water, continued

40. [OH-] = concentration of base (N)
[OH-] = 10-pOH
[OH-] = concentration of base (N)
[H3O+] [OH-] = 1.0 x 10-14

41. SAMPLE PROBLEM D
What is the concentration of a HCl solution with pH of 5.6?

42. SAMPLE PROBLEM D
What is the concentration of a HCl solution with pH of 5.6?
Plug into equation & calculator.
[H+] =
[H+] = 2.5 x 10-6

43. SAMPLE PROBLEM E
What is the concentration of a Mg(OH)2 solution with pH of 5.6?

44. SAMPLE PROBLEM E
What is the concentration of a Mg(OH)2 solution with pH of 5.6?
Step 1:
Plug into equation & calculator.
[H+] =
[H+] = 2.5 x 10-6

45. SAMPLE PROBLEM E
What is the concentration of a Mg(OH)2 solution with pH of 5.6?
Step 2:
Convert from H to OH.
[H+] = 2.5 x 10-6
[H+] [OH-] = 1.0 x 10-14
(2.5 x 10-6) [OH-] = 1.0 x 10-14
[OH-] = 4.0 x 10-9

46. NEUTRALIZATION REACTIONS

47. Neutralization Reaction
Chapter 15
Visual Concepts
Neutralization Reaction

48. NEUTRALIZATION REACTIONS
The reaction of an acid and a base to form salt & water
H+ ions react with OH- to form water
Predict products as in a double replacement rxn (partner swap)
HCl (aq) + NaOH (aq) 
H2O (l) + NaCl (s)

49. PRACTICE REACTIONS
HCl + LiOH 
HNO3 + Ca(OH)2 
H2SO4 + Al(OH)3 

50. PRACTICE REACTIONS HCl + LiOH  H2O + LiCl
2 HNO3 + Ca(OH)2  2 H2O + Ca(NO3)2
3 H2SO Al(OH)3  6 H2O + Al2(SO4)3

51. NORMALITY
AN ACIDS/BASES UNIT

52. NORMALITY (N) N = (MOLARITY) ( # OF H’s)
What is N equal to in a monoprotic acid?
N = M
What is N equal to in a diprotic acid?
N = 2 M

53. TITRATIONS
NA VA = NB VB

54. Chapter 15
Titration
Visual Concepts

55. NORMALITY & NEUTRALIZATION REACTIONS
NA VA = NB VB
Where:
NA = normality of acid
VA = volume of acid
NB = normality of base
VB = volume of base

56. NORMALITY & NEUTRALIZATION REACTIONS
What volume of a 0.25 M HCl solution is needed to neutralize 36 mL of 0.30 Mg(OH)2 M?
Step 1: Start with what you know.
NA = (0.25 M) (1) = 0.25 N
VA = X mL
NB = (0.30 M) (2) = 0.60 N
VB = 36 mL

57. NORMALITY & NEUTRALIZATION REACTIONS
What volume of a 0.25 M HCl solution is needed to neutralize 36 mL of 0.30 Mg(OH)2 M?
Step 2: Substitute & Solve.
NA VA = NB VB
(0.25) (X) = (0.60) (36)
0.25 X = 21.6
X = 86.4 mL

58. Multiple Choice 1. Which of the following is not a characteristic of
an acid?
A. An acid changes the color of an indicator.
B. An acid has a bitter taste.
C. An acid ionizes in water.
D. An acid produces hydronium ions in water.

59. Multiple Choice 1. Which of the following is not a characteristic of
an acid?
A. An acid changes the color of an indicator.
B. An acid has a bitter taste.
C. An acid ionizes in water.
D. An acid produces hydronium ions in water.

60. Multiple Choice 2. When an acid reacts with an active metal,
A. the hydronium ion concentration increases.
B. the metal forms anions.
C. hydrogen gas is produced.
D. carbon dioxide gas is produced.

61. Multiple Choice 2. When an acid reacts with an active metal,
A. the hydronium ion concentration increases.
B. the metal forms anions.
C. hydrogen gas is produced.
D. carbon dioxide gas is produced.

62. Multiple Choice 3. Which of the following is a Brønsted-Lowry base?
A. an electron pair donor
B. an electron pair acceptor
C. a proton donor
D. a proton acceptor

63. Multiple Choice 3. Which of the following is a Brønsted-Lowry base?
A. an electron pair donor
B. an electron pair acceptor
C. a proton donor
D. a proton acceptor

64. Multiple Choice 4. What is the formula for acetic acid? A. CH3COOH
B. HNO3
C. HClO4
D. HCN

65. Multiple Choice 4. What is the formula for acetic acid? A. CH3COOH
B. HNO3
C. HClO4
D. HCN

66. Multiple Choice
5. Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.
A. calcium sulfate
B. calcium hydroxide
C. calcium oxide
D. calcium phosphate

67. Multiple Choice
5. Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.
A. calcium sulfate
B. calcium hydroxide
C. calcium oxide
D. calcium phosphate

68. Short Answer
6. How does a strong acid differ from a weak acid? Give one example of each.

69. Short Answer
6. How does a strong acid differ from a weak acid? Give one example of each.
Answer: A strong acid is 100% ionized; a weak acid is less than 100% ionized. Possible strong acids are HCl, HI, HBr, HNO3, H2SO4, HClO4, and HClO3. With very few exceptions, any other acid will be a weak acid.

70. Multiple Choice 1. Distilled water contains A. H2O. B. H3O+. C. OH.
D. All of the above

71. Multiple Choice 1. Distilled water contains A. H2O. B. H3O+. C. OH.
D. All of the above

72. Multiple Choice 2. What is the pH of a 0.0010 M HNO3? A. 1.0 B. 3.0
D. 5.0

73. Multiple Choice 2. What is the pH of a 0.0010 M HNO3? A. 1.0 B. 3.0
D. 5.0

74. Multiple Choice
3. Which of the following solutions would have a pH value greater than 7?
A. [OH] = 2.4  102 M
B. [H3O+] = 1.53  102 M
C M HCl
D. [OH] = 4.4  109 M

75. Multiple Choice
3. Which of the following solutions would have a pH value greater than 7?
A. [OH] = 2.4  102 M
B. [H3O+] = 1.53  102 M
C M HCl
D. [OH] = 4.4  109 M

76. Multiple Choice 4. If the pH of a solution of the strong base NaOH
is known, which property of the solution can be
calculated?
A. molar concentration
B. [OH]
C. [H3O+]
D. All of the above

77. Multiple Choice 4. If the pH of a solution of the strong base NaOH
is known, which property of the solution can be
calculated?
A. molar concentration
B. [OH]
C. [H3O+]
D. All of the above

78. Multiple Choice 5. A neutral aqueous solution
A. has a 7.0 M H3O+ concentration.
B. contains neither hydronium ions nor hydroxide
ions.
C. has an equal number of hydronium ions and
hydroxide ions.
D. None of the above

79. Multiple Choice 5. A neutral aqueous solution
A. has a 7.0 M H3O+ concentration.
B. contains neither hydronium ions nor hydroxide
ions.
C. has an equal number of hydronium ions and
hydroxide ions.
D. None of the above

80. Multiple Choice
6. Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.
A. calcium sulfate
B. calcium hydroxide
C. calcium oxide
D. calcium phosphate

81. Multiple Choice
6. Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.
A. calcium sulfate
B. calcium hydroxide
C. calcium oxide
D. calcium phosphate

82. Multiple Choice 7. The pH of a solution is 6.32. What is the pOH?
B. 4.8  107
C. 7.68
D. 2.1  108

83. Multiple Choice 7. The pH of a solution is 6.32. What is the pOH?
B. 4.8  107
C. 7.68
D. 2.1  108

84. Multiple Choice
8. Which of the pH levels listed below is the most acidic?
A. pH = 1
B. pH = 5
C. pH = 9
D. pH = 13

85. Multiple Choice
8. Which of the pH levels listed below is the most acidic?
A. pH = 1
B. pH = 5
C. pH = 9
D. pH = 13

86. Short Answer
9. A solution has a pH of What is the hydronium ion concentration? Is the solution acidic or basic?

87. Short Answer
9. A solution has a pH of What is the hydronium ion concentration? Is the solution acidic or basic?
Answer: [H3O+] = 1.8  105 M; acidic

88. Extended Response
10. The hydroxide ion concentration in a solution is 1.6  1011 M. What are the [H3O+], the pH, and the pOH of the solution?

89. Extended Response
10. The hydroxide ion concentration in a solution is 1.6  1011 M. What are the [H3O+], the pH, and the pOH of the solution?
Answer: [H3O+] = 6.3  104 M
pH = 3.20
pOH = 10.80

90. Extended Response
11. Write the balanced equation that represent the reaction that takes place when milk of magnesia (magnesium hydroxide) reacts with hydrochloric acid in your stomach.

91. Extended Response
Write the balanced equation that represent the reaction that takes place when milk of magnesia (magnesium hydroxide) reacts with hydrochloric acid in your stomach.
Answer: