1. 1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with mL 2.5 M B. Kc = 2.0 x 10-10

2. Drill:
1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when a solution is made with 1.0 M A &
1.0 M B. Kc = 2.0 x 10-12

3. Exp # [A] [B] [C] Rate
1) 27 C
2) 27 C
3) 27 C
4) 27 C
5)127 C

4. ([A4]/[A1])a = rate4/rate1
Exp # [A] [B] [C] Rate
1) 27 C
2) 27 C
3) 27 C
4) 27 C
5)127 C
([A4]/[A1])a = rate4/rate1
3a = 9; thus, a = 2

5. ([B3]/[B2])b = rate3/rate2
Exp # [A] [B] [C] Rate
1) 27 C
2) 27 C
3) 27 C
4) 27 C
5)127 C
([B3]/[B2])b = rate3/rate2
2b = 8; thus b = 3

6. ([C2]/[C1])c = rate2/rate1
Exp # [A] [B] [C] Rate
1) 27 C
2) 27 C
3) 27 C
4) 27 C
5)127 C
([C2]/[C1])c = rate2/rate1
2c = 2; thus c = 1

7. Rate = k[A]2[B]3[C]
k =
Rate [A]2[B]3[C]

8. 1 P2 + 2 SO2 + 1 O2  2 PO2 + 2 SO
2 PO2  1 P2O4
1 P2O SO  2 PO + 2 SO2
4 PO SO2  2 P2O5 + 3 S
3 P2O S  1 P6S6O15

9. 1 P2 + 2 SO2 + 1 O2  2 PO2 + 2 SO
2 PO2  1 P2O4
1 P2O SO  2 PO + 2 SO2
4 PO SO2  2 P2O5 + 3 S
3 P2O S  1 P6S6O15

10. 1 P2 + 2 SO2 + 1 O2  2 PO2 + 2 SO
2 PO2  1 P2O4
2 P2O SO  4 PO + 4 SO2
4 PO SO2  2 P2O5 + 3 S
3 P2O S  1 P6S6O15

11. 1 P2 + 2 SO2 + 1 O2  2 PO2 + 2 SO
4 PO2  2 P2O4
2 P2O SO  4 PO + 4 SO2
4 PO SO2  2 P2O5 + 3 S
3 P2O S  1 P6S6O15

12. 2 P2 + 4 SO2 + 2 O2  4 PO2 + 4 SO
4 PO2  2 P2O4
2 P2O SO  4 PO + 4 SO2
4 PO SO2  2 P2O5 + 3 S
3 P2O S  1 P6S6O15

13. 2 P2 + 4 SO2 + 2 O2  4 PO2 + 4 SO
4 PO2  2 P2O4
2 P2O SO  4 PO + 4 SO2
4 PO SO2  2 P2O5 + 3 S
3 P2O S  1 P6S6O15

14. 2 P2 + 4 SO2 + 2 O2  4 PO2 + 4 SO
4 PO2  2 P2O4
2 P2O SO  4 PO + 4 SO2
4 PO SO2  2 P2O5 + 3 S
2 P2 + 3 SO2 + 2 O2  2 P2O5 + 3 S

15. 2 P2 + 3 SO2 + 2 O2  2 P2O5 + 3 S
Rate = k[P2 ]2[SO2]3[O2]2

16. __N2 +__CO2 +__O2  __NO2 +__CO
__NO2  __N2O4
__N2O __CO  __NO +__CO2
__ NO __ CO2  __ N2O5 + __ C
__N2O __C  __C2N2O5

17. __N2 +__CO2 +__O2  __NO2 +__CO
__NO2  __N2O4
__N2O __CO  __NO +__CO2
4 NO CO2  2 N2O5 + 3 C
__N2O __C  __C2N2O5

18. __N2 +__CO2 +__O2  __NO2 +__CO
__NO2  __N2O4
2 N2O CO  4 NO +4 CO2
4 NO CO2  2 N2O5 + 3 C
__N2O __C  __C2N2O5

19. __N2 +__CO2 +__O2  __NO2 +__CO
__NO2  __N2O4
2 N2O CO  4 NO +4 CO2
4 NO CO2  2 N2O5 + 3 C
__N2O __C  __C2N2O5

20. __N2 +__CO2 +__O2  __NO2 +__CO
4 NO2  2 N2O4
2 N2O CO  4 NO +4 CO2
4 NO CO2  2 N2O5 + 3 C
__N2O __C  __C2N2O5

21. __N2 +__CO2 +__O2  __NO2 +__CO
4 NO2  2 N2O4
2 N2O CO  4 NO +4 CO2
4 NO CO2  2 N2O5 + 3 C
__N2O __C  __C2N2O5

22. 2 N2 + 4 CO2 + 2 O2  4 NO2 + 4 CO
4 NO2  2 N2O4
2 N2O CO  4 NO +4 CO2
4 NO CO2  2 N2O5 + 3 C
__N2O __C  __C2N2O5

23. 2 N2 + 4 CO2 + 2 O2  4 NO2 + 4 CO
4 NO2  2 N2O4
2 N2O CO  4 NO +4 CO2
4 NO CO2  2 N2O5 + 3 C
2 N2 + 3 CO2 + 2 O2  2 N2O5 + 3 C
__N2O __C  __C2N2O5

24. 2 N2 + 4 CO2 + 2 O2  4 NO2 + 4 CO
4 NO2  2 N2O4
2 N2O CO  4 NO +4 CO2
4 NO CO2  2 N2O5 + 3 C
2 N2 + 3 CO2 + 2 O2  2 N2O5 + 3 C
2 N2O C  2 C2N2O5

25. 2 N2 + 4 CO2 + 2 O2  4 NO2 + 4 CO
4 NO2  2 N2O4
2 N2O CO  4 NO +4 CO2
4 NO CO2  2 N2O5 + 3 C
2 N2 + 3 CO2 + 2 O2  2 N2O5 + 3 C
2 N2O C  2 C2N2O5

27. Acid/Base

28. Properties of Acids
Sour taste, Change color of dyes, Conduct electricity in solution, React with many metals, React with bases to form salts

29. Properties of Bases
Bitter taste, Feel slippery, Change color of dyes, Conduct electricity in solution, React with acids to form salts

30. Arrhenius Acids: release H+ or H3O+ in solution
Bases: release OH- in solution

31. Arrhenius Acid: HA --> H+ + A- HCl --> H+ + Cl-
Base: MOH --> M+ + OH-
NaOH -->Na+ + OH-

32. Bronsted-Lowry
Acid: Proton donor
Base:
Proton Acceptor

33. Bronsted-Lowry HA + H2O --> H3O+ + A- HI + H2O --> H3O+ + I-
Acid Base CA CB
NH3 + H2O --> NH4+ + OH-
Base Acid CA CB

34. Lewis Acid/Base
Acid: Electron
Acceptor
Base: Electron Donor

35. Lewis Acid/Base
H3N: + BF3 --> H3N-BF3
Base Acid Neutral

36. Common Names H+ Hydrogen ion H3O+ Hydronium ion H- Hydride ion
OH- Hydroxide ion
NH3 Ammonia
NH4+ Ammonium ion

37. Amphiprotism Can act like an acid or a base
Can donate or accept protons

38. Naming Acids All acids are H-anion If the anion is:
-ides  hydro___ic acids
-ates  ___ic acids
-ites  ___ous acids

39. Naming Bases Almost all bases are metal hydroxides
Name by normal method
Ammonia (NH3) as well as many amines are bases

40. Strong Acids or Bases Strong acids or bases ionize 100 % in solution
Weak acids or bases ionize <100 % in solution

41. Drill: Name each of the following: KOH HBr Al(OH)3 H2CO3 HClO4 NH3

42. Review Drill & Check HW

43. CHM II HW
Review PP-21
Complete the attached assignment & turn it in tomorrow.

44. Strong Acids or Bases Strong acids or bases ionize 100 % in solution
Weak acids or bases ionize <100 % in solution

45. Strong Acids HClO4 Perchloric acid H2SO4 Sulfuric acid
HNO3 Nitric acid
HCl Hydrochloric acid
HBr Hydrobromic acid
HI Hydroiodic acid

46. Strong Bases All column I hydroxides Ca(OH)2 Calcium hydroxide
Sr(OH)2 Strontium hydroxide
Ba(OH)2 Barium hydroxide

47. Strong Acid/Base
Ionizes 100 % (1 M)
HA H+ + A-
1 M – all

48. Binary Acids Acids containing only 2 elements HCl Hydrochloric acid
H2S Hydrosulfuric acid

49. Ternary Acids H2SO4 Sulfuric acid HNO3 Nitric acid
Acids containing 3 elements
H2SO4 Sulfuric acid
HNO3 Nitric acid

50. Monoprotic Acids Acids containing only one ionizable hydrogen
HBr Hydrobromic acid
HC2H3O2 Acetic acid

51. Diprotic Acids Acids containing 2 ionizable hydrogens
H2SO4 Sulfuric acid
H2CO3 Carbonic acid

52. Triprotic Acids Acids containing 3 ionizable hydrogens
H3PO4 Phosphoric acid
H3AsO4 Arsenic acid

53. Polyprotic Acids H4SiO4 Silicic acid H2CO2 Carbonous acid
Acids containing more than one ionizable hydrogens
H4SiO4 Silicic acid
H2CO2 Carbonous acid

54. Monohydroxic Base A base containing only one ionizable hydroxide
NaOH Sodium hydroxide
LiOH Lithium hydroxide

55. Neutralization Rxn HA(aq) + MOH(aq)  MA(aq) + H2O(l)
A reaction between an acid & a base making salt & H2O
HA(aq) + MOH(aq)
 MA(aq) + H2O(l)

56. Neutralization Rxn
HCl(aq) + NaOH(aq) 
NaCl(aq) + H2O(l)

57. pH The negative log of the hydrogen or hydronium ion concentration
pH = -log[H+]
pOH = -log[OH-]

58. Calculate the pH of each of the following: 1) [H+] = 0
Calculate the pH of each of the following: 1) [H+] = M 2) [HCl] = M 3) [HBr] = M

59. Calculate the pOH of each of the following:
1) [OH-] = M 2) [KOH] = M 3) [NaOH] = 4.0 x 10-7 M

60. A solution with known concentration
Standard Solution
A solution with known concentration

61. Drill: Identify: acid, base, CA, & CB
HCO3- + H2O
H2CO3 + OH-

62. Review Drill & Check HW

63. CHM II HW
Review PP-21
Complete the attached assignment & turn it in tomorrow.

64. Titration
A method of determining the concentration of one solution by reacting it with a standard solution

65. Titration Formula for monoprotic solutions
MAVA = MBVB

66. Equivalence Point
The point where the concentrations of the two solutions in the titration are equal

67. Titration Fact When titrating acids against bases, the end
point of the titration is
at the equivalence point

68. Acid/Base Equivalence Point
The point where the H+
concentration is equal to
the OH- concentration

69. Titration Fact
No changes will be observed when titrating acids against bases; thus, one must use an indicator to see changes

70. Indicator
An organic dye that changes color when the pH changes

71. Drill:
Calculate the molarity of 25.0 mL HCl when it’s titrated to its equivalence point with 50.0 mL M NaOH

72. Titration Formula for monoprotic solutions
MAVA = MBVB

73. Dilution Formula
M1V1 = M2V2

74. Calculate the mL of 16.0 M HNO3 it takes to make 4.0 L of 0.100 M HNO3

75. Calculate the mL of 12.5 M HCl required to make 2.5 L of 0.200 M HCl
Make Calculations
Calculate the mL of 12.5 M HCl required to make 2.5 L of M HCl

76. Moles of solute per liter of solution (M)
Molarity
Moles of solute per liter of solution (M)

77. Normality
Number of moles of hydrogen or hydroxide ions per liter of solution (N)

78. Titration Formula for Acid/Base
NAVA = NBVB
Elliott’s Rule:
#HMAVA = #OHMBVB

79. Make Calculations
Calculate the molarity of 30.0 mL H2CO3 when it’s titrated to its equivalence point with 75.0 mL M NaOH

80. Make Calculations
Calculate the molarity of 40.0 mL H3PO4 when it’s titrated to its equivalence point with 30.0 mL 0.20 M Ba(OH)2

81. Calculate the volume of 0. 250 M HCl needed to titrate 50. 00 mL 0
Calculate the volume of M HCl needed to titrate mL M NaOH to its equivalence point

82. Calculate the molarity 25. 0 mL H3PO4 that neutralizes 50. 00 mL 0
Calculate the molarity 25.0 mL H3PO4 that neutralizes mL M Ca(OH)2 to its equivalence point

83. Titration Curve: Strong acid vs strong base

85. Titration Curve: Strong acid vs strong base; then weak acid vs strong base

88. Titration Curve: Strong base vs strong acid; then weak base vs strong acid

90. 3.2 g HI is dissolved in a 1250 mL aqueous solution. Calculate its pH.

91. Calculate the volume of 0. 10 M H3PO4 that neutralizes 50. 00 mL 0
Calculate the volume of 0.10 M H3PO4 that neutralizes mL M Ca(OH)2 to its equivalence point

92. AP CHM HW
Read: Chapter 13
Problems: 7 & 9
Page: 395

93. CHM II HW
Read: Chapter 18
Problems: 27
Page: 787

94. Drill: Calculate the molarity of 25
Drill: Calculate the molarity of mL of H3PO4 that was titrated to its equivalence point with mL of M Ba(OH)2.