1 / 55

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 - ]

anila
Télécharger la présentation

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

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related