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

2. Drill: Calculate [H 2 Q], [HQ - ], [Q -2 ], [H + ], & pH of 0.20 M KHQ. Ka 1 = 2.0 x 10 -4 Ka 2 = 8.0 x 10 -9

3. Solubility

4. The amount of one substance that will dissolve in another

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

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

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

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

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

13. Write the equation & equilibrium expression for: Al 2 (SO 4 ) 3

14. Solubility Calculations

15. Calculate the solubility of BaSO 4(s) Ksp = 1.2 x 10 -10

16. Solubility Product BaSO 4(s) Ba +2 (aq) + SO 4 -2 (aq) Ksp =[Ba +2 ][SO 4 -2 ]

17. Calculate the solubility of SrCr 2 O 7(s) Ksp = 2.5 x 10 -13

18. Calculate the solubility of PbI 2(s) K sp = 8.0 x 10 -9

19. Calculate the solubility of Mn 2 S 3(s) K sp = 1 x 10 -98

20. Drill: Write the reaction & equilibrium expression when solid Fe 2 (SO 4 ) 3 is added to water.

21. Drill: Calculate the solubility of M 3 X 4 K sp for M 3 X 4 = 6.9 x 10 -207

22. Solubility Concepts AgI (s) Ag + + I - K sp = [Ag + ][I - ] at Eq. Q sp = [Ag + ][I - ] init.

23. Solubility Concepts If Q sp > K sp a precipitate will form If Q sp < K sp no precipitate will form

24. 150 mL 0.0010 M KI is added to 100 mL 0.050 M Pb(NO 3 ) 2. K sp for PbI 2 = 8.0 x 10 -9 Will a ppt form?

25. Calculate the solubility of AgI (s) K sp = 1.5 x 10 -16

26. Common Ion Solubility Calculations

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

28. Calculate the solubility of AgI (s) in 0.10 M NaI K sp = 1.5 x 10 -16

29. Calculate the solubility of MZ 2(s) in 0.20 M M(NO 3 ) 2 K sp = 2.0 x 10 -15

30. Drill: 10.0 mL 0.050 M KCl is added to 15 mL 0.075 M Pb(NO 3 ) 2. K sp PbCl 2 = 1.7 x 10 -5 Will a ppt form?

31. Calculate the solubility of M 2 Z 3(s) in 0.20 M M(NO 3 ) 3 K sp = 2.0 x 10 -16

32. Drill: Calculate the solubility of CaCO 3 in water. K sp = 4.9 x 10 -15

33. Calculate the solubility of PbI 2(s) in 0.010 M NaI K sp = 3.2 x 10 -8

34. The Really Bad Solubility Problems

35. Aqueous NaI is added (dropwise) to a solution of 0.10 M AgNO 3(s) & 0.10 M CuNO 3 AgI K sp = 1.0 x 10 -16 CuI K sp = 5.1 x 10 -12

36. Aqueous KCl is added (dropwise) to a solution of 0.10 M AgNO 3 & 0.10 M Cu(NO 3 ) 2 AgCl K sp = 1.8 x 10 -10 Cu Cl 2 K sp = 5.1 x 10 -12

37. Drill: Calculate the solubility of PbS (s) K sp = 1.0 x 10 -28

38. Review

39. Calculate the solubility of PbCl 2(s) K sp = 1.6 x 10 -5

40. Calculate the solubility of Sc(OH) 3(s) K sp = 2.7 x 10 -31

41. Calculate the solubility of Ca(OH) 2. K sp = 4.0 x 10 -6

42. Calculate the pH of Li 2 CO 3 K sp = 8.2 x 10 -4 K a1 = 4.4 x 10 -7 K a2 = 4.7 x 10 -11

43. Calculate the solubility of AgI (s) in 0.20 M NaI K sp = 1.5 x 10 -16

44. The solubility of MX 2(s) is 2.0 x 10 -5 M. Calculate its K sp

45. Aqueous MgCl 2 is added (dropwise) to a solution of 0.20 M KOH & 0.10 M K 2 SO 4 Mg(OH) 2 K sp = 5.0 x 10 -6 Mg SO 4 K sp = 5.6 x 10 -5

46. 10.0 mL 0.050 M KCl is added to 15 mL 0.060 M Pb(NO 3 ) 2. K sp PbCl 2 = 1.7 x 10 -5 Will a ppt form?

47. Drill: The solubility of YF 3 is 2.0 x 10 -8. Calculate the value of K sp.