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Chemistry 132 NT

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Chemistry 132 NT

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    1. Chemistry 132 NT Instead of having “answers” on a math test, they should just call them “ impressions”, and if you got a different “impression”, so what, can’t we all be brothers? Jack Handey

    3. Acid-Base Equilibria Chapter 16 Module 3 Sections 16.5, 16.6, and 16.7

    4. Review Calculating the concentration of a species in a weak base solution using Kb

    5. The Common Ion Effect The common-ion effect is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion common to the equilibrium.

    6. The Common Ion Effect The common-ion effect is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion common to the equilibrium.

    7. The Common Ion Effect The common-ion effect is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion common to the equilibrium.

    8. The Common Ion Effect The common-ion effect is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion common to the equilibrium.

    9. A Problem To Consider An aqueous solution is 0.025 M in formic acid, HCH2O and 0.018 M in sodium formate, NaCH2O. What is the pH of the solution. The Ka for formic acid is 1.7 x 10-4.

    10. A Problem To Consider An aqueous solution is 0.025 M in formic acid, HCH2O and 0.018 M in sodium formate, NaCH2O. What is the pH of the solution. The Ka for formic acid is 1.7 x 10-4.

    11. A Problem To Consider An aqueous solution is 0.025 M in formic acid, HCH2O and 0.018 M in sodium formate, NaCH2O. What is the pH of the solution. The Ka for formic acid is 1.7 x 10-4.

    12. A Problem To Consider An aqueous solution is 0.025 M in formic acid, HCH2O and 0.018 M in sodium formate, NaCH2O. What is the pH of the solution. The Ka for formic acid is 1.7 x 10-4.

    13. A Problem To Consider An aqueous solution is 0.025 M in formic acid, HCH2O and 0.018 M in sodium formate, NaCH2O. What is the pH of the solution. The Ka for formic acid is 1.7 x 10-4.

    14. A Problem To Consider An aqueous solution is 0.025 M in formic acid, HCH2O and 0.018 M in sodium formate, NaCH2O. What is the pH of the solution. The Ka for formic acid is 1.7 x 10-4.

    15. A Problem To Consider An aqueous solution is 0.025 M in formic acid, HCH2O and 0.018 M in sodium formate, NaCH2O. What is the pH of the solution. The Ka for formic acid is 1.7 x 10-4.

    16. A Problem To Consider An aqueous solution is 0.025 M in formic acid, HCH2O and 0.018 M in sodium formate, NaCH2O. What is the pH of the solution. The Ka for formic acid is 1.7 x 10-4.

    17. Buffers A buffer is a solution characterized by the ability to resist changes in pH when limited amounts of acid or base are added to it.

    18. Buffers A buffer is a solution characterized by the ability to resist changes in pH when limited amounts of acid or base are added to it.

    19. Buffers A buffer is a solution characterized by the ability to resist changes in pH when limited amounts of acid or base are added to it.

    20. Buffers A buffer is a solution characterized by the ability to resist changes in pH when limited amounts of acid or base are added to it.

    21. The pH of a Buffer The solution described in Example 16.10 in your text is a buffer, because it is composed of a weak acid (0.10 M acetic acid) and its conjugate base (0.20 M acetate ion).

    22. A Problem To Consider Instructions for making up a buffer say to mix 60.0 mL of 0.100 M NH3 with 40.0 mL of 0.100 M NH4Cl. What is the pH of this buffer?

    23. A Problem To Consider Instructions for making up a buffer say to mix 60.0 mL of 0.100 M NH3 with 40.0 mL of 0.100 M NH4Cl. What is the pH of this buffer?

    24. A Problem To Consider Instructions for making up a buffer say to mix 60.0 mL of 0.100 M NH3 with 40.0 mL of 0.100 M NH4Cl. What is the pH of this buffer?

    25. A Problem To Consider Instructions for making up a buffer say to mix 60.0 mL of 0.100 M NH3 with 40.0 mL of 0.100 M NH4Cl. What is the pH of this buffer?

    26. A Problem To Consider Instructions for making up a buffer say to mix 60.0 mL of 0.100 M NH3 with 40.0 mL of 0.100 M NH4Cl. What is the pH of this buffer?

    27. A Problem To Consider Instructions for making up a buffer say to mix 60.0 mL of 0.100 M NH3 with 40.0 mL of 0.100 M NH4Cl. What is the pH of this buffer?

    28. A Problem To Consider Instructions for making up a buffer say to mix 60.0 mL of 0.100 M NH3 with 40.0 mL of 0.100 M NH4Cl. What is the pH of this buffer?

    29. A Problem To Consider Instructions for making up a buffer say to mix 60.0 mL of 0.100 M NH3 with 40.0 mL of 0.100 M NH4Cl. What is the pH of this buffer?

    30. A Problem To Consider Instructions for making up a buffer say to mix 60.0 mL of 0.100 M NH3 with 40.0 mL of 0.100 M NH4Cl. What is the pH of this buffer?

    31. Adding Acid or Base to a Buffer Example 16.10 in your text describes a buffer composed of acetic acid and sodium acetate. This buffer controls the equilibrium below.

    32. Adding Acid or Base to a Buffer Example 16.10 in your text describes a buffer composed of acetic acid and sodium acetate. This buffer controls the equilibrium below.

    33. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    34. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    35. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    36. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    37. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    38. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    39. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    40. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    41. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    42. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    43. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    44. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    45. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    46. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    47. A Problem To Consider Calculate the pH of 75 mL of the buffer described in Example 16.10 (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 9.5 mL of 0.10 M HCl is added.

    48. The Henderson-Hasselbalch Equation How do you prepare a buffer of given pH?

    49. The Henderson-Hasselbalch Equation How do you prepare a buffer of given pH?

    50. The Henderson-Hasselbalch Equation How do you prepare a buffer of given pH?

    51. The Henderson-Hasselbalch Equation How do you prepare a buffer of given pH?

    52. A Problem To Consider A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of this buffer? (The Ka for HF is 6.8 x 10-4)

    53. A Problem To Consider A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of this buffer? (The Ka for HF is 6.8 x 10-4)

    54. A Problem To Consider A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of this buffer? (The Ka for HF is 6.8 x 10-4)

    55. A Problem To Consider A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of this buffer? (The Ka for HF is 6.8 x 10-4)

    56. A Problem To Consider A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of this buffer? (The Ka for HF is 6.8 x 10-4)

    57. The Henderson-Hasselbalch Equation How do you prepare a buffer of given pH?

    58. Acid-Ionization Titration Curves An acid-base titration curve is a plot of the pH of a solution of acid (or base) against the volume of added base (or acid).

    59. Titration of a Strong Acid by a Strong Base Figure 16.11 shows a curve for the titration of HCl with NaOH.

    60. Figure 16.11

    61. Titration of a Strong Acid by a Strong Base Figure 16.11 shows a curve for the titration of HCl with NaOH.

    62. Titration of a Strong Acid by a Strong Base Figure 16.11 shows a curve for the titration of HCl with NaOH.

    63. A Problem To Consider Calculate the pH of a solution in which 10.0 mL of 0.100 M NaOH is added to 25.0 mL of 0.100 M HCl.

    64. A Problem To Consider Calculate the pH of a solution in which 10.0 mL of 0.100 M NaOH is added to 25.0 mL of 0.100 M HCl.

    65. A Problem To Consider Calculate the pH of a solution in which 10.0 mL of 0.100 M NaOH is added to 25.0 mL of 0.100 M HCl.

    66. A Problem To Consider Calculate the pH of a solution in which 10.0 mL of 0.100 M NaOH is added to 25.0 mL of 0.100 M HCl.

    67. A Problem To Consider Calculate the pH of a solution in which 10.0 mL of 0.100 M NaOH is added to 25.0 mL of 0.100 M HCl.

    68. Titration of a Weak Acid by a Strong Base The titration of a weak acid by a strong base gives a somewhat different curve.

    69. Titration of a Weak Acid by a Strong Base The titration of a weak acid by a strong base gives a somewhat different curve.

    70. Figure 16.12

    71. A Problem To Consider Calculate the pH of the solution at the equivalence point when 25.0 mL of 0.10 M acetic acid is titrated with 0.10 M sodium hydroxide. The Ka for acetic acid is 1.7 x 10-5.

    72. A Problem To Consider Calculate the pH of the solution at the equivalence point when 25.0 mL of 0.10 M acetic acid is titrated with 0.10 M sodium hydroxide. The Ka for acetic acid is 1.7 x 10-5.

    73. A Problem To Consider Calculate the pH of the solution at the equivalence point when 25.0 mL of 0.10 M acetic acid is titrated with 0.10 M sodium hydroxide. The Ka for acetic acid is 1.7 x 10-5.

    74. A Problem To Consider Calculate the pH of the solution at the equivalence point when 25.0 mL of 0.10 M acetic acid is titrated with 0.10 M sodium hydroxide. The Ka for acetic acid is 1.7 x 10-5.

    75. A Problem To Consider Calculate the pH of the solution at the equivalence point when 25.0 mL of 0.10 M acetic acid is titrated with 0.10 M sodium hydroxide. The Ka for acetic acid is 1.7 x 10-5.

    76. Titration of a Weak Base by a Strong Acid The titration of a weak base with a strong acid is a reflection of our previous example.

    77. Figure 16.13

    78. A Little “Trick” At the “half-way” point in the titration of a weak acid with a weak base, we can make a significant simplification.

    79. A Little “Trick” At the “half-way” point in the titration of a weak acid with a weak base, we can make a significant simplification.

    80. Operational Skills Calculating the common-ion effect on acid ionization

    81. Homework Chapter 16 Homework: collected at the first exam. Review Questions: none. Problems: 37, 41, 45, 49.

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