1. Salts

2. Salt Solutions The salts of weak acids can recombine with water producing basic solutions

3. Salt Solutions The salts of weak bases can recombine with water producing acidic solutions

4. Salt Solutions A - + H 2 O HA + OH - B + + H 2 O H + + BOH

5. Salt or Hydrolysis Problems

6. Salt Problem Calculate the pH of a 0.20 M solution of NaBz K a = 6.4 x 10 -5

7. Salt Problem Calculate the pH of a 0.10 M solution of R-NH 3 Cl K b = 2.5 x 10 -5

8. Drill: Calculate the pH of a 0.18 M solution of KC 2 H 3 O 2 K a = 1.8 x 10 -5

9. Drill: Calculate the pH of a 0.16 M solution of KC 7 H 5 O 2 K a = 6.4 x 10 -5

10. Salt Applications Salts of strong acids & weak bases make acidic solutions

11. Salt Applications Salts of strong bases & weak acids make basic solutions

12. Salt Applications Salts of strong acids & strong bases make neutral solutions

13. Predict Relative pH NaAcBaCl 2 KNO 3 NH 4 Br KHSO 4 NH 4 Ac

14. Predict Relative pH KAcNaCl KClO 2 NH 4 Cl K 2 SO 4 NaI

15. Anhydrides Compounds without water; that when added to water, form other compounds

16. Acid Anhydrides Non-metal oxides that form acids when added to water

17. Basic Anhydrides Metal oxides that form bases when added to water

18. Predict Relative pH Na 2 OSO 2 NO 2 CO 2 CaOAl 2 O 3

19. A/B eq, Buffer & Salt Hydrolysis Problems

20. Calculate the pH of 0.10 M HF. K a HF = 6.5 x 10 -4

21. 7.4 g of Ca(OH) 2 was added to 2.0 L of 0.075 M H 2 CO 3. Calculate the molarity of all ions present in the solution. K a1 = 4.4 x 10 -7 K a2 = 4.7 x 10 -11

22. Calculate the pH of 0.10 M HF in 0.20 M NaF. K a HF = 6.5 x 10 -4

23. Calculate the pH of 5.0 M KCN. K aHCN = 5.0 x 10 -10

24. Calculate [H 3 PO 4 ], [H 2 PO 4 -1 ], [HPO 4 -2 ], [PO 4 -3 ], [K + ], [H + ], & pH of 1.0 M KH 2 PO 4 in 0.50 M K 2 HPO 4. K a1 = 7.5 x 10 -3 K a2 = 6.2 x 10 -8 K a3 = 4.2 x 10 -13

25. Calculate pH of: 0.50 M MOH in 0.20 M MCl K b = 5.0 x 10 -5

26. Calculate pH of: 0.20 M MCl K b = 5.0 x 10 -5

27. Review of Acid/Base descriptions and Acid/Base, Buffer, & Salt Equilibria

28. Arhenius, Bronsted- Lowry, & Lewis Acids & Bases

29. Strong Acids Strong Bases

30. Acid rxns Base rxns

31. A/B Equilibrium Constants K W, K A, K B, & pH

32. Calculate pH of: 0.025 M HNO 3 0.020 M KOH

33. Calculate pH of: 2.0 M HNO 2 K a = 2.0 x 10 -4

34. Calculate pH of: 3.0 M HZ in 2.0 M KZ K a HZ = 3.0 x 10 -5

35. Calculate pH of: 0.20 M KQ K a HQ = 2.0 x 10 -5

36. 150 mL of 0.10 M KOH was added to 100.0 mL of 0.10 M H 2 CO 3. Calculate [H 2 CO 3 ], [HCO 3 - ], [CO 3 -2 ], [H + ], [OH - ], & pH of the solution. K a1 = 4.4 x 10 -7 K a2 = 4.7 x 10 -11

37. Calculate [H 3 A], [H 2 A -1 ], [HA -2 ], [A -3 ], [K + ], [H + ], [OH - ], & pH of 2.0 M KH 2 A. K a1 = 4.0 x 10 -3 K a2 = 5.0 x 10 -8 K a3 = 2.5 x 10 -13

38. Calculate pH of: 2.0 M HQ K a = 2.0 x 10 -6

39. Calculate pH of: 6.0 M HZ in 4.0 M KZ K a HZ = 3.0 x 10 -5

40. Calculate pH of: 0.20 M KQ K a HQ = 2.0 x 10 -7