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Drill: Calculate the pH of 2.0 x 10 -4 M HI

Drill: Calculate the pH of 2.0 x 10 -4 M HI. Calculate the pH of 3.3 x 10 -8 M HI. Acid-Base Equilibria. Ionization of Water. H 2 O (l)  H + (aq) + OH - (aq) 2 H 2 O (l)  H 3 O + (aq) + OH - (aq). Water Ionization Constant. K w = [H + ][OH - ] K w = [H 3 O + ][OH - ]

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Drill: Calculate the pH of 2.0 x 10 -4 M HI

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  1. Drill: Calculate the pH of 2.0 x 10-4 M HI

  2. Calculate the pH of 3.3 x 10-8 M HI

  3. Acid-Base Equilibria

  4. Ionization of Water H2O(l) H+(aq)+ OH-(aq) 2 H2O(l) H3O+(aq) + OH-(aq)

  5. Water Ionization Constant Kw = [H+][OH-] Kw = [H3O+][OH-] Kw = 1.00 x 10-14 Memorize this

  6. Kw Calculations In pure water [H+] = [OH-] Kw =[H+][OH-] = 1.0 x 10-14 Let [H+] = x = [OH-]

  7. Kw Calculations Kw =[H+][OH-] = x2 Kw = x2 =1.0 x 10-14 Thus x = 1.0 x 10-7 M [H+] = x = 1.0 x 10-7 M

  8. pH of Pure Water [H+] = 1.0 x 10-7 M pH = -log[H+] pH = -log[1.0 x 10-7] pH = 7 -log 1 Thus pH = 7.00

  9. Calculate [H+],[OH-], pH, & pOH of 0.020 M HCl

  10. Calculate [H+] of 0.050 M H2SO4

  11. AP CHM HW • Problems: 9 • Page: 395

  12. CHM II HW • Problems: 27 • Page: 787

  13. Drill: Calculate [H+],[OH-], pH, & pOH of 0.025 M KOH

  14. Weak Acid Ionization HA(aq) H+(aq) + A-(aq) HA(aq) + H2O(l) H3O+(aq) + A-(aq)

  15. Acid Dissociation Constant HA(aq)H+(aq) + A-(aq) • [H+][A-] • [HA] Ka =

  16. Weak Base Ionization NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)

  17. Base Dissociation Constant NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) • [NH4+][OH-] • [NH3] Kb =

  18. Acid-Base Equilibria Problems

  19. Calculate [H+], [OH-], pH, & pOH of 2.0 M HC2H3O2 (HAc)Ka = 1.8 x 10-5

  20. Drill: Calculate [H+], [OH-], pH, & pOH of0.50 M NH3Kb = 1.8 x 10-5

  21. Calculate [H+],[OH-], pH, & pOH of 0.010 M HC7H5O2 (HBz)Ka = 6.4 x 10-5

  22. AP CHM HW • Problems: 37 • Page: 396

  23. CHM II HW • Problems: 43 • Page: 788

  24. Drill: Calculate [H+], [OH-], pH, & pOH of 0.50 M C6H5NH2Kb = 3.2 x 10-5

  25. Calculate the Ka of 0.10 M Hquack when it ionized 5.0 % in an aqueous solution.

  26. Drill: The pH of a 0.79 M solution of Hnut is 3.10. Calculate its Ka

  27. Calculate the pH of a solution of 0.00050 M HBS : Ka = 5.0 x 10-12

  28. Drill: Calculate the pH of0.025 M HF:Ka = 6.4 x 10-4

  29. AP CHM HW • Problems: 39 • Page: 397

  30. CHM II HW • Problems: 45 • Page: 788

  31. Drill: Calculatethe pH of 0.025 M QOH:Kb = 2.0 x 10-4

  32. Calculate [H2CO3], [HCO3-], [CO3-2], [H+],[OH-], & pH of 0.44 M H2CO3Ka1 = 4.4 x 10-7Ka2 = 4.7 x 10-11

  33. AP CHM Test covering A/B & A/B Equilibria will be on Thursday

  34. CHM II Test covering A/B & A/B Equilibria will be on Thursday

  35. Calculate [H2SeO3], [HSeO3-], [SeO3-2], [H+],[OH-], & pH of 0.27 M H2SeO3Ka1 = 2.7 x 10-7Ka2 = 5.4 x 10-11

  36. AP CHM HW • Problem 39 on page 396

  37. Calculate the pH, & pOH of 0.10 M HClO Ka = 2.5 x 10-8

  38. Drill: Calculate the pH of 2.5 M HAz Ka = 2.5 x 10-14

  39. Calculate [H3A],[H2A-], [HA-2],[A-3],[H+], &pH of 0.30 M H3A Ka1 = 3.0 x 10-7Ka2 = 5.0 x 10-11Ka3 = 4.0 x 10-15

  40. AP CHM HW • Work problem 55 on page 397 • Test Thursday

  41. CHM II HW • Work problem 53 on page 788 • Test Thursday

  42. Review

  43. Arrhenius Bronsted-Lowry Lewis

  44. Be able to name: • Acids • Bases

  45. Be able to describe & Identify: • Strong Acids • Strong Bases

  46. Show the ionization of HClO4 in solution

  47. Show the ionization of NH3 in solution

  48. Calculate the [H+], [OH-], pH, & pOHof 0.1 M HNO3

  49. Calculate the [H+], [OH-], pH, & pOHof 0.02 M NaOH

  50. Drill: Calculate the pH, & pOH of 0.10 M HNO2Ka = 6.0 x 10-4

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