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Drill: Calculate the pH of: [H + ] = 3.0 x 10 -5 M [HI] = 2.0 x 10 -4 M

Drill: Calculate the pH of: [H + ] = 3.0 x 10 -5 M [HI] = 2.0 x 10 -4 M. 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 - ] or K w = [H 3 O + ][OH - ]

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Drill: Calculate the pH of: [H + ] = 3.0 x 10 -5 M [HI] = 2.0 x 10 -4 M

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  1. Drill: Calculate the pH of: [H+] = 3.0 x 10-5 M [HI] = 2.0 x 10-4 M

  2. Acid-Base Equilibria

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

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

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

  6. 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

  7. 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

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

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

  10. Calculate [H+] of 0.050 M H2SO4

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

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

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

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

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

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

  17. Acid-Base Equilibria Problems

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

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

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

  21. The pH of a 0.79 M solution of Hnut is 3.10. Calculate its Ka

  22. Drill: Calculate [H+] & pH of 0.50 M NaOH

  23. Drill: Calculate [H+] & pH of 2.0 M C6H5NH2Kb = 3.2 x 10-5

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

  25. PolyproticAcidEquilibria

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

  27. Calculate [H2SeO3], [HSeO3-1], [SeO3-2], [H+],[OH-], & pH of 0.27 M H2SeO3Ka1 = 2.7 x 10-7Ka2 = 5.4 x 10-11

  28. 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

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

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

  31. You have 10 identical coins with 1 coin having a slight mass difference. Determine the odd coin with only 3 uses of an equal arm balance.

  32. Drill: Calculate the pH of 0.25 M HAz Ka = 2.5 x 10-3

  33. Drill: Calculate the pH of 0.25 M HAz Ka = 2.5 x 10-3

  34. Calculate the pH of0.10 M HClO Ka = 2.5 x 10-8

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

  36. Drill: Calculate the pH of 0.020 M QOH.Kb = 3.2 x 10-7

  37. TestReview

  38. Arrhenius Bronsted-Lowry Lewis

  39. Be able to name: • Acids • Bases

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

  41. Show the ionization of HClin solution

  42. Show the ionization of NH3in solution

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

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

  45. Calculate the [H+], [OH-], pH, & pOH of 2.0 M NH3Kb = 1.8 x 10-5

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

  47. Calculate the volume of 0.30 M Ba(OH)2 required to titrate 50.00 mL of 0.40 M H3PO4 to its equivalence point.

  48. Calculate [H2A], [HA-], [A-2], [H+], & pH of 0.20 M H2A Ka1 = 2.0 x 10-7Ka2 = 5.0 x 10-11

  49. Calculate the pH of a solution of 0.20 M QNH2.Kb = 2.0 x 10-3

  50. Drill: 831 mL NH3 was bubbled through 2.0 L of water at 27.0oC under 150 kPa pressure. 80.0 % of the ammonia dissolves in the water. Calculate the pH of the final solution.

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