Drill:

1. Drill: • Determine the KQ/HQ ratio to make a buffer solution with a pH of 4.70 • Ka for HQ = 3.0 x 10-5

2. Drill: Calculate [H2Q], [HQ-], [Q-2], [H+], & pH of 0.20 M KHQ.Ka1 = 2.0 x 10-4Ka2 = 8.0 x 10-9

3. Review Drill & Test

4. CHM II HW • Review PP-25 • Complete the attached assignment & turn it in tomorrow

5. Solubility

6. Solubility • The amount of one substance that will dissolve in another

7. Precipitation • When dissolved particles join together forming a new phase and exit the solution

8. Precipitate (ppt) • The new phase that forms and leaves the solution

9. Ppt Examples • Water vapor combining to form rain • Dissolved ions combining to form a solid

10. Saturated Solution • When the maximum amount of one substance is dissolved in another

11. Precipitation • When more than the maximum amount of solute is added to a solution, a ppt will form

12. Write the equilibrium expression for AgCl(s) Ag+ + Cl-

13. Solubility Product MX(s) M+(aq) + X-(aq) Ksp =[M+][X-]

14. Solubility Product MX2(s) M+2(aq) + 2 X-(aq) Ksp =[M+2][X-]2

15. Write the equation & equilibrium expression for: Al2(SO4)3

16. Solubility Calculations

17. Calculate the solubility of BaSO4(s) • Ksp = 1.2 x 10-10

18. Solubility Product BaSO4(s) Ba+2(aq) + SO4-2(aq) Ksp =[Ba+2][SO4-2]

19. Calculate the solubility of SrCr2O7(s) • Ksp = 2.5 x 10-13

20. Calculate the solubility of PbI2(s) • Ksp = 8.0 x 10-9

21. Drill: Write the reaction & equilibrium expression when solid Fe2(SO4)3 is added to water.

22. Drill: Calculate the solubility of M3X4Ksp for M3X4= 6.9 x 10-207

23. Solubility Concepts AgI(s) Ag+ + I- Ksp = [Ag+][I-] at Eq. Qsp = [Ag+][I-] init.

24. Solubility Concepts • If Qsp > Ksp a precipitate will form • If Qsp < Ksp no precipitate will form

25. 150 mL 0.010 M KI is added to 100 mL 0.010 M Pb(NO3)2. Ksp for PbI2 = 8.0 x 10-9 • Will a ppt form?

26. AP CHM HW • Read: Chapter 16 • Problem: 13 • Page: 463

27. CHM II HW • Read: Chapter 20 • Problem: 17 • Page: 843

28. Drill: • 10.0 mL 0.050 M KCl is added to 15 mL 0.075 M Pb(NO3)2. Ksp = 1.7 x 10-5 • Will a ppt form?

29. Drill: Calculate the solubility of AgI(s) • Ksp = 1.5 x 10-16

30. Review Drill&Check HW

31. CHM II HW • Review PP-25 • Complete the attached assignment & turn it in tomorrow.

32. Calculate the solubility of Mn2S3(s) • Ksp = 1 x 10-98

33. Common Ion Solubility Calculations

34. Common Ion Effect • Solubility of a solid is reduced when one of its ions is already in solution

35. Calculate the solubility of AgI(s) in 0.10 M NaI • Ksp = 1.5 x 10-16

36. Calculate the solubility of MZ2(s) in • 0.20 M M(NO3)2 Ksp = 2.0 x 10-15

37. Calculate the solubility of M2Z3(s) in • 0.20 M M(NO3)3 Ksp = 2.0 x 10-16

38. AP CHM HW • Read: Chapter 16 • Problems: 18 • Page: 463

39. CHM II HW • Read: Chapter 20 • Problems: 19 • Page: 844

40. Drill: Calculate the solubility of CaCO3 in water. Ksp = 4.9 x 10-15

41. Calculate the solubility of PbI2(s) in 0.010 M NaI • Ksp = 3.2 x 10-8

42. Aqueous NaI is added (dropwise) to a solution of 0.10 M AgNO3(s) & 0.10 M CuNO3 AgI Ksp = 1.0 x 10-16 CuI Ksp = 5.1 x 10-12

43. Aqueous KCl is added (dropwise) to a solution of 0.10 M AgNO3 & 0.10 M Cu(NO3)2 • AgCl Ksp = 1.8 x 10-10 • CuCl2 Ksp = 5.1 x 10-12

44. Test on Thursday or Friday

45. Drill: Calculate the solubility of PbS(s) Ksp = 1.0 x 10-28

46. Review

47. Calculate the solubility of PbCl2(s) • Ksp = 1.6 x 10-5

48. Calculate the solubility of Sc(OH)3(s) • Ksp = 2.7 x 10-31

49. Calculate the pH of Ca(OH)2 in solution. • Ksp = 4.0 x 10-6

50. Calculate the pH of LiCO3 in soln Ksp = 8.2 x 10-4 Ka1 = 4.4 x 10-7 Ka2 = 4.7 x 10-11