1. 1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with 100.0 mL 2.5 M B. K c = 2.0 x 10 -10

2. 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. K c = 2.0 x 10 -12

3. Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10400.0

4. Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10400.0 ([A 4 ]/[A 1 ]) a = rate 4 /rate 1 3 a = 9; thus, a = 2

5. Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10400.0 ([B 3 ]/[B 2 ]) b = rate 3 /rate 2 2 b = 8; thus b = 3

6. Exp # [A] [B] [C] Rate 1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10400.0 ([C 2 ]/[C 1 ]) c = rate 2 /rate 1 2 c = 2; thus c = 1

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

8. __N 2 +__CO 2 +__O 2  __NO 2 +__CO __NO 2  __N 2 O 4 __N 2 O 4 + __CO  __NO +__CO 2 __ NO + __ CO 2  __ N 2 O 5 + __ C __N 2 O 5 + __C  __C 2 N 2 O 5

9. __N 2 +__CO 2 +__O 2  __NO 2 +__CO __NO 2  __N 2 O 4 __N 2 O 4 + __CO  __NO +__CO 2 4 NO + 3 CO 2  2 N 2 O 5 + 3 C __N 2 O 5 + __C  __C 2 N 2 O 5

10. __N 2 +__CO 2 +__O 2  __NO 2 +__CO __NO 2  __N 2 O 4 2 N 2 O 4 + 4 CO  4 NO +4 CO 2 4 NO + 3 CO 2  2 N 2 O 5 + 3 C __N 2 O 5 + __C  __C 2 N 2 O 5

11. __N 2 +__CO 2 +__O 2  __NO 2 +__CO __NO 2  __N 2 O 4 2 N 2 O 4 + 4 CO  4 NO +4 CO 2 4 NO + 3 CO 2  2 N 2 O 5 + 3 C __N 2 O 5 + __C  __C 2 N 2 O 5

12. __N 2 +__CO 2 +__O 2  __NO 2 +__CO 4 NO 2  2 N 2 O 4 2 N 2 O 4 + 4 CO  4 NO +4 CO 2 4 NO + 3 CO 2  2 N 2 O 5 + 3 C __N 2 O 5 + __C  __C 2 N 2 O 5

13. __N 2 +__CO 2 +__O 2  __NO 2 +__CO 4 NO 2  2 N 2 O 4 2 N 2 O 4 + 4 CO  4 NO +4 CO 2 4 NO + 3 CO 2  2 N 2 O 5 + 3 C __N 2 O 5 + __C  __C 2 N 2 O 5

14. 2 N 2 + 4 CO 2 + 2 O 2  4 NO 2 + 4 CO 4 NO 2  2 N 2 O 4 2 N 2 O 4 + 4 CO  4 NO +4 CO 2 4 NO + 3 CO 2  2 N 2 O 5 + 3 C __N 2 O 5 + __C  __C 2 N 2 O 5

15. 2 N 2 + 4 CO 2 + 2 O 2  4 NO 2 + 4 CO 4 NO 2  2 N 2 O 4 2 N 2 O 4 + 4 CO  4 NO +4 CO 2 4 NO + 3 CO 2  2 N 2 O 5 + 3 C 2 N 2 + 3 CO 2 + 2 O 2  2 N 2 O 5 + 3 C __N 2 O 5 + __C  __C 2 N 2 O 5

16. 2 N 2 + 4 CO 2 + 2 O 2  4 NO 2 + 4 CO 4 NO 2  2 N 2 O 4 2 N 2 O 4 + 4 CO  4 NO +4 CO 2 4 NO + 3 CO 2  2 N 2 O 5 + 3 C 2 N 2 + 3 CO 2 + 2 O 2  2 N 2 O 5 + 3 C 2 N 2 O 5 + 4 C  2 C 2 N 2 O 5

17. 2 N 2 + 4 CO 2 + 2 O 2  4 NO 2 + 4 CO 4 NO 2  2 N 2 O 4 2 N 2 O 4 + 4 CO  4 NO +4 CO 2 4 NO + 3 CO 2  2 N 2 O 5 + 3 C 2 N 2 + 3 CO 2 + 2 O 2  2 N 2 O 5 + 3 C 2 N 2 O 5 + 1 4 C  2 C 2 N 2 O 5

19. Acid/Base

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

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

22. Arrhenius ·Acids: release H + or H 3 O + in solution ·Bases: release OH - in solution

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

24. Bronsted-Lowry ·Acid: Proton donor ·Base: Proton Acceptor

25. Bronsted-Lowry ·HA + H 2 O --> H 3 O + + A - ·HI + H 2 O --> H 3 O + + I - ·Acid Base CA CB ·NH 3 + H 2 O --> NH 4 + + OH - ·Base Acid CA CB

26. Lewis Acid/Base ·Acid: Electron Acceptor ·Base: Electron Donor

27. Lewis Acid/Base H 3 N: + BF 3 --> H 3 N-BF 3 Base Acid Neutral

28. Drill: List 3 properties each of both acids & bases

29. Common Names ·H + Hydrogen ion ·H 3 O + Hydronium ion ·H - Hydride ion ·OH - Hydroxide ion ·NH 3 Ammonia ·NH 4 + Ammonium ion

30. Amphoterism ·Can act like an acid or a base ·Can donate or accept protons

31. Define acids & bases by each of the three methods

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

33. Naming Bases ·Almost all bases are metal hydroxides ·Name by normal method ·Ammonia (NH 3 ) as well as many amines are bases

34. Drill: Name each of the following: NaOHHI Ba(OH) 2 H 2 SO 4 HMnO 4 H 3 PO 3

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

36. Strong Acids ·HClO 4 Perchloric acid ·H 2 SO 4 Sulfuric acid ·HNO 3 Nitric acid ·HClHydrochloric acid ·HBrHydrobromic acid ·HIHydroiodic acid

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

38. Binary Acids ·Acids containing only 2 elements ·HClHydrochloric acid ·H 2 SHydrosulfuric acid

39. Ternary Acids ·Acids containing 3 elements ·H 2 SO 4 Sulfuric acid ·H 2 SO 3 Sulfurous acid ·HNO 3 Nitric acid

40. Drill: Name & give the formula for at least 4 each of strong acids & strong bases

41. Strong Acid/Base Ionizes 100 % (1 M) HAH + + A - 1 M – all1 1

42. Monoprotic Acids ·Acids containing only one ionizable hydrogen ·HBr Hydrobromic acid ·HCNHydrocyanic acid ·HC 2 H 3 O 2 Acetic acid

43. Diprotic Acids ·Acids containing 2 ionizable hydrogens ·H 2 SO 4 Sulfuric acid ·H 2 SO 3 Sulfurous acid ·H 2 CO 3 Carbonic acid

44. Triprotic Acids ·Acids containing 3 ionizable hydrogens ·H 3 PO 4 Phosphoric acid ·H 3 PO 3 Phosphorus acid ·H 3 AsO 4 Arsenic acid

45. Polyprotic Acids ·Acids containing more than one ionizable hydrogens ·H 2 SO 4 Sulfuric acid ·H 4 SiO 4 Silicic acid ·H 2 CO 2 Carbonous acid

46. Monohydroxic Base ·A base containing only one ionizable hydroxide ·NaOHSodium hydroxide ·KOHPotassium hydro. ·LiOHLithium hydroxide

47. AP CHM HW Read: Chapter 13 Problems: 1 - 3 Page: 395

48. CHM II HW Read: Chapter 18 Problems: 3 & 5 Page: 787

49. Neutralization Rxn ·A reaction between an acid & a base making salt & H 2 O ·HA (aq) + MOH (aq)  MA (aq) + H 2 O (l)

50. Neutralization Rxn HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O (l)

51. Drill: Identify: acid, base, CA, & CB HCO 3 - + H 2 O H 2 CO 3 + OH -

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

53. Calculate the pH of each of the following: 1) [H + ] = 0.040 M 2) [HCl] = 0.0025 M 3) [HBr] = 0.080 M

54. Calculate the pOH of each of the following: 1) [OH - ] = 0.030 M 2) [KOH] = 0.0025 M 3) [NaOH] = 4.0 x 10 -12 M

55. AP CHM HW Read Chapter 13 Work problems 17 & 19 on page 395

56. Standard Solution ·A solution with known concentration

57. Titration ·A method of determining the concentration of one solution by reacting it with a standard solution ·M A V A = M B V B for monoprotics

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

59. Equivalence Point ·The point where the H + concentration is equal to the OH - concentration

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

61. Indicator ·An organic dye that changes color when the pH changes

62. Drill: ·Calculate the molarity of 25.0 mL HCl when it’s titrated to its equivalence point with 50.0 mL 0.200 M NaOH

63. Dilution Formula M 1 V 1 = M 2 V 2

64. ·Calculate the mL of 16.0 M HNO 3 it takes to make 4.0 L of 0.100 M HNO 3

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

66. Molarity ·Moles of solute per liter of solution (M)

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

68. Titration Formula ·N A V A = N B V B ·Elliott’s Rule: ·# H M A V A = # OH M B V B

69. Make Calculations ·Calculate the molarity of 30.0 mL H 2 CO 3 when it’s titrated to its equivalence point with 75.0 mL 0.200 M NaOH

70. Make Calculations ·Calculate the molarity of 40.0 mL H 3 PO 4 when it’s titrated to its equivalence point with 30.0 mL 0.20 M Ba(OH) 2

71. Calculate the volume of 0.250 M HCl needed to titrate 50.00 mL 0.200 M NaOH to its equivalence point

72. Calculate the molarity 25.0 mL H 3 PO 4 that neutralizes 50.00 mL 0.200 M Ca(OH) 2 to its equivalence point

73. Drill: Calculate the volume of 0.10 M H 3 PO 4 that neutralizes 50.00 mL 0.200 M Ca(OH) 2 to its equivalence point

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

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

76. Drill: Calculate the molarity of 25.00 mL of H 3 PO 4 that was titrated to its equivalence point with 75.00 mL of 0.125 M Ba(OH) 2.

77. Drill: 3.2 g HI is dissolved in a 125 mL aqueous solution. Calculate its pH.

78. Titration Curve: Strong acid vs strong base

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

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