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

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

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

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

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

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

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

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

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

17. Buffer & Salt Hydrolysis Problems

18. Calculate the pH of 1.0 M HF in 0.50 M NaF. K a HF = 6.5 x 10 -4

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

20. 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

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

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

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

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

25. Strong Acids Strong Bases

26. Acid rxns Base rxns

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

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

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

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

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

32. 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

33. 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

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

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

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