1. Acids Lesson 22 Subtle Items

2. 1.Weak bases neutralize a strong acid as well as a strong base would.

3. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would. HCl +NaOH

4. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would. HCl +NaOH→NaCl +HOH

5. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would. HCl +NaOH→NaCl +HOH HCl +HCO 3 -

6. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would. HCl +NaOH→NaCl +HOH HCl +HCO 3 - →H 2 CO 3 +Cl -

7. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would. HCl +NaOH→NaCl +HOH HCl +HCO 3 - →H 2 CO 3 +Cl - Both reactions go to completion because of the strong acid.

8. 2.H 3 BO 3

9. 2.H 3 BO 3 triprotic

10. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 -

11. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3

12. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic

13. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 -

14. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HCl

15. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HClmonoprotic

16. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HClmonoprotic HCl → H + + Cl -

17. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HClmonoprotic HCl → H + + Cl - Only lose one proton when in water! However,

18. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HClmonoprotic HCl → H + + Cl - Only lose one proton when in water! However, H 3 BO 3 + NaOH

19. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HClmonoprotic HCl → H + + Cl - Only lose one proton when in water! However, loses all three because of the strong base! H 3 BO 3 + 3NaOH→ Na 3 BO 3 +3HOH

20. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HClmonoprotic HCl → H + + Cl - Only lose one proton when in water! However, loses all three because of the strong base! H 3 BO 3 + 3NaOH→ Na 3 BO 3 +3HOH HCl + NaOH→

21. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HClmonoprotic HCl → H + + Cl - Only lose one proton when in water! However, loses all three because of the strong base! H 3 BO 3 + 3NaOH→ Na 3 BO 3 +3HOH HCl + NaOH→ NaCl +HOH

22. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HClmonoprotic HCl → H + + Cl - Only lose one proton when in water! However, loses all three because of the strong base! H 3 BO 3 + 3NaOH→ Na 3 BO 3 +3HOH HCl + NaOH→ NaCl +HOH Which neutralizes more NaOH, H 3 BO 3 or HCl?

23. 2.H 3 BO 3 triprotic H 3 BO 3 ⇌ H + + H 2 BO 3 - H 2 CO 3 diprotic H 2 CO 3 ⇌ H + + HCO 3 - HClmonoprotic HCl → H + + Cl - Only lose one proton when in water! However, loses all three because of the strong base! H 3 BO 3 + 3NaOH→ Na 3 BO 3 +3HOH HCl + 1NaOH→ NaCl +HOH Which neutralizes more NaOH? H 3 BO 3 or HCl?

24. 3.Which determines acid strength? Molarity pH = Ka

25. 3.Which determines acid strength? Molarity is concentration. pH = Ka

26. 3.Which determines acid strength? Molarity is concentration. pH = -Log[H + ] Ka

27. 3.Which determines acid strength? Molarity is concentration. pH = -Log[H + ] Ka is strength as indicated in the acid chart

28. 4.Which determines the pH. Ka Molarity Temperature

29. 4.Which determines the pH = -Log[H + ] Ka Molarity Temperature

30. 4.Which determines the pH = -Log[H + ] Ka determines the [H + ] and the pH Molarity Temperature

31. 4.Which determines the pH = -Log[H + ] Ka determines the [H + ] and the pH Molarity determines the [H + ] and the pH Temperature

32. 4.Which determines the pH = -Log[H + ] Ka determines the [H + ] and the pH Molarity determines the [H + ] and the pH Temperature determines the [H + ] and the pH

33. 5.Pick the best conductor. 1 MNaOH0.1 M HCl0.01 M KOH

34. 5.Pick the best conductor. 1 MNaOH0.1 M HCl0.01 M KOH All strong- highest Molarity!

35. 6.Pick the worst conductor. NaOHHClNaCNNH 3

36. 6.Pick the worst conductor. NaOHHClNaCNNH 3

37. 6.Pick the worst conductor. NaOHHClNaCNNH 3 Good Conductors are….. Strong acids Strong Bases Soluble Salts

38. 7.1 mole H 2 CO 3 and 1mole NaHCO 3 are dissolved in 0.5 L of water. What kind of solution results in the above mixture? Buffer Write an equation for the equilibrium. H 2 CO 3 ⇋ H + +HCO 3 - Label each chemical species with a concentration. 2 MLow2 M What limits the ability to buffer against acid? [HCO 3 - ] What limits the ability to buffer against base? [H 2 CO 3 ]

39. 8.AcidBase HF

40. 8.AcidBase HFF -

41. 8.AcidBase HFF - H 2 BO 3 -

42. 8.AcidBase HFF - H 3 BO 3 H 2 BO 3 -

43. 8.AcidBase HFF - H 3 BO 3 H 2 BO 3 - HCN

44. 8.AcidBase HFF - H 3 BO 3 H 2 BO 3 - HCNCN -

45. 8.AcidBase HFF - H 3 BO 3 H 2 BO 3 - HCNCN - Put an asterisk next to the strongest acid and base

46. 8.AcidBase *HFF - H 3 BO 3 H 2 BO 3 - HCNCN - Put an asterisk next to the strongest acid and base

47. 8.AcidBase *HFF - H 3 BO 3 H 2 BO 3 - HCNCN - * Put an asterisk next to the strongest acid and base

48. 8.AcidBase *HFF - H 3 BO 3 H 2 BO 3 - HCNCN - * Put an asterisk next to the strongest acid and base What is the relationship between acid strength and strength of conjugate base?

49. 8.AcidBase *HFF - H 3 BO 3 H 2 BO 3 - HCNCN - * Put an asterisk next to the strongest acid and base What is the relationship between acid strength and strength of conjugate base?Inverse

50. 9.What ions are in H 2 SO 4 solution? H 2 SO 4

51. 9.What ions are in H 2 SO 4 solution? H 2 SO 4 →H + +HSO 4 -

52. 9.What ions are in H 2 SO 4 solution? H 2 SO 4 →H + +HSO 4 - HSO 4 -

53. 9.What ions are in H 2 SO 4 solution? H 2 SO 4 →H + +HSO 4 - HSO 4 - ⇌ H + +SO 4 2-

54. 9.What ions are in H 2 SO 4 solution? H 2 SO 4 →H + +HSO 4 - HSO 4 - ⇌ H + +SO 4 2-

55. 9.What ions are in H 2 SO 4 solution? H 2 SO 4 →H + +HSO 4 - HSO 4 - ⇌ H + +SO 4 2-

56. 9.What ions are in H 2 SO 4 solution? H 2 SO 4 →H + +HSO 4 - HSO 4 - ⇌ H + +SO 4 2-

57. 9.What ions are in H 2 SO 4 solution? H 2 SO 4 →H + +HSO 4 - HSO 4 - ⇌ H + +SO 4 2- [ OH - ]

58. 9.What ions are in H 2 SO 4 solution? H 2 SO 4 →H + +HSO 4 - HSO 4 - ⇌ H + +SO 4 2- [ OH - ] because it is in water!

59. 9.What ions are in H 2 SO 4 solution? H 2 SO 4 →H + +HSO 4 - HSO 4 - ⇌ H + +SO 4 2-

60. 10. Which titration will have the equivalence point with lowest conductivity? HCl+ NaOH H 2 SO 4 + Ba(OH) 2

61. 10. Which titration will have the equivalence point with lowest conductivity? HCl+ NaOH → NaCl +HOH H 2 SO 4 + Ba(OH) 2 →

62. 10. Which titration will have the equivalence point with lowest conductivity? HCl+ NaOH → NaCl +HOH H 2 SO 4 + Ba(OH) 2 → High Solubility

63. 10. Which titration will have the equivalence point with lowest conductivity? HCl+ NaOH → NaCl +HOH H 2 SO 4 + Ba(OH) 2 → BaSO 4 +2HOH High Solubility

64. 10. Which titration will have the equivalence point with lowest conductivity? HCl+ NaOH → NaCl +HOH H 2 SO 4 + Ba(OH) 2 → BaSO 4 +2HOH High Solubility Low Solubility Lowest Conductivity

65. 11.What is the best acid for titrating 0.10 M NH 3 ? 0.10 M NaOH0.10 M HF 6.0 M HCl0.10 M HCl

66. 11.What is the best acid for titrating 0.10 M NH 3 ? 0.10 M NaOH0.10 M HF 6.0 M HCl0.10 M HCl

67. 11.What is the best acid for titrating 0.10 M NH 3 ? 0.10 M NaOH0.10 M HF 6.0 M HCl0.10 M HCl Must be strong and about the same molarity!

68. 12.HClMolaritypH 1 M

69. 12.HClMolaritypH 1 M0

70. 12.HClMolaritypH 1 M0 0.1M

71. 12.HClMolaritypH 1 M0 0.1M1

72. 12.HClMolaritypH 1 M0 0.1M1 0.01M

73. 12.HClMolaritypH 1 M0 0.1M1 0.01M2

74. 12.HClMolaritypH 1 M0 0.1M1 0.01M2 0.001M

75. 12.HClMolaritypH 1 M0 0.1M1 0.01M2 0.001M3

76. 12.HClMolaritypH 1 M0 0.1M1 0.01M2 0.001M3 0.0001M

77. 12.HClMolaritypH 1 M0 0.1M1 0.01M2 0.001M3 0.0001M4

78. 12.HClMolaritypH 10 M 1 M0 0.1M1 0.01M2 0.001M3 0.0001M4

79. 12.HClMolaritypH 10 M-1 1 M0 0.1M1 0.01M2 0.001M3 0.0001M4

80. 13.A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak?

81. Strong

82. 13.A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak? Strong as pH = -Log[0.00010] = 4.0

83. 13.A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak? Strong as pH = -Log[0.00010] = 4.0 The pH is not 0 because the acid is 0.00010 M!

84. 14.Describe the buffer present in human blood. H 2 CO 3 NaHCO 3 15.What is stomach acid? HCl 16.What is battery acid? H 2 SO 4