1 / 75

Titrations of acids and bases

Titrations of acids and bases. Titrations of acids and bases. HA + H 2 O H 3 O + + A -. Titrations of acids and bases. HA + H 2 O H 3 O + + A -. B + H 2 O OH - + HB +. Titrations of acids and bases. HA + H 2 O H 3 O + + A -.

scott
Download Presentation

Titrations of acids and bases

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. Titrations of acids and bases

  2. Titrations of acids and bases HA + H2O H3O+ + A-

  3. Titrations of acids and bases HA + H2O H3O+ + A- B + H2O OH- + HB+

  4. Titrations of acids and bases HA + H2O H3O+ + A- B + H2O OH- + HB+ H3O+ + OH- 2 H2O

  5. H3O+ + OH- 2 H2O At equivalence point [H3O+] = [OH-] For strong acid – strong base

  6. H3O+ + OH- 2 H2O At equivalence point [H3O+] = [OH-] Kw = [H3O+] = [OH-] = 10-14

  7. H3O+ + OH- 2 H2O At equivalence point [H3O+] = [OH-] Kw = [H3O+] = [OH-] = 10-14 pH = 7

  8. Titrations of acids and bases HA + H2O H3O+ + A- B + H2O OH- + HB+ H3O+ + OH- 2 H2O

  9. Start with acid solution 7 pH Volume of base added

  10. 10 pH 4

  11. 100 ml 0.1 M HCl

  12. 100 ml 0.1 M HCl Titrate with 0.1 M NaOH

  13. 100 ml 0.1 M HCl Titrate with 0.1 M NaOH H3O+ + OH- 2 H2O

  14. 100 ml 0.1 M HCl Titrate with 0.1 M NaOH H3O+ + OH- 2 H2O Every part of a mole of NaOH added reduces the moles of H3O+ by an equal amount.

  15. 100 ml 0.1 M HCl Titrate with 0.1 M NaOH H3O+ + OH- 2 H2O As NaOH solution is added, the overall volume increases. This further decreases [H3O+].

  16. 100 ml 0.1 M HCl Titrate with 0.1 M NaOH Neutralization and dilution; both increase the pH of the solution.

  17. 100 ml 0.1 M HCl Titrate with 0.1 M NaOH Add 50 ml of NaOH solution.

  18. 100 ml 0.1 M HCl Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. Start with 0.1 L x 0.1 M H3O+

  19. 100 ml 0.1 M HCl Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. Start with 0.1 L x 0.1 M H3O+ 0.01 moles H3O+

  20. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. Add 0.05 L x 0.1 M OH-

  21. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. Add 0.05 L x 0.1 M OH- 0.005 moles OH-

  22. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. 0.005 moles OH- H3O+ is neutralized by OH- 1:1 ratio

  23. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. 0.005 moles OH- Remaining H3O+ = 0.01 moles – 0.005 moles

  24. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. 0.005 moles OH- Remaining H3O+ = 0.005 moles Total volume = 150 ml = 0.15 L

  25. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. 0.005 moles OH- [H3O+]= 0.005 moles 0.15 L

  26. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. 0.005 moles OH- [H3O+]= 0.005 moles = 0.033 M 0.15 L

  27. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 50 ml of NaOH solution. 0.005 moles OH- [H3O+]= 0.005 moles = 0.033 M 0.15 L pH = 1.48

  28. 100 ml 0.1 M HCl Titrate with 0.1 M NaOH Add 99.9 ml of NaOH solution.

  29. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 99.9 ml of NaOH solution.

  30. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 99.9 ml of NaOH solution. 0.0999 L x 0.1 M = 0.00999 moles OH-

  31. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 99.9 ml of NaOH solution. 0.0999 L x 0.1 M = 0.00999 moles OH- Moles H3O+ = 0.01 – 0.00999 = 1 x 10-5

  32. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 99.9 ml of NaOH solution. 0.0999 L x 0.1 M = 0.00999 moles OH- Moles H3O+ = 0.01 – 0.00999 = 1 x 10-5 Total volume = 0.1 L + 0.0999 L = 0.1999 L

  33. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 99.9 ml of NaOH solution. 0.0999 L x 0.1 M = 0.00999 moles OH- [H3O+]= 1 x 10-5 moles 0.1999 L

  34. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 99.9 ml of NaOH solution. 0.0999 L x 0.1 M = 0.00999 moles OH- [H3O+]= 1 x 10-5 moles = 5 x 10-5 0.1999 L

  35. 100 ml 0.1 M HCl 0.01 moles H3O+ Titrate with 0.1 M NaOH Add 99.9 ml of NaOH solution. 0.0999 L x 0.1 M = 0.00999 moles OH- [H3O+]= 1 x 10-5 moles = 5 x 10-5 0.1999 L pH = 4.3

  36. 4.3

  37. + 0.1 ml will give pH = 7 4.3

  38. If more 0.1 M NaOH solution is added after the equivalence point, there is no H3O+ to neutralize it.

  39. At pH = 7 the volume is 0.2 L

  40. At pH = 7 the volume is 0.2 L Add 0.1 mL 0.1 M NaOH

  41. At pH = 7 the volume is 0.2 L Add 0.1 mL 0.1 M NaOH Add 0.0001 L x 0.1 M = 10-5 moles OH- [OH-] = 1 x 10-5 moles = 5 x 10-5 M 0.201 L

  42. At pH = 7 the volume is 0.2 L Add 0.1 mL 0.1 M NaOH Add 0.0001 L x 0.1 M = 10-5 moles OH- [OH-] = 1 x 10-5 moles = 5 x 10-5 M 0.2001 L pOH = 4.3 pH = 9.7

  43. pH = 9.7 V = 200.1 ml V = 200 ml pH = 7 4.3 V = 199.9 ml

  44. Titrating a weak acid with a strong base

  45. Titrating a weak acid with a strong base Ka < 1 HA + H2O H3O+ + A-

  46. Titrating a weak acid with a strong base Ka < 1 HA + H2O H3O+ + A- Much less than 100% dissociation.

More Related