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Salts

Salts. Salt Solutions. The salts of weak acids can recombine with water producing basic solutions. Salt Solutions. The salts of weak bases can recombine with water producing acidic solutions. Salt Solutions. A - + H 2 O HA + OH - B + + H 2 O H + + BOH.

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Salts

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  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- + H2O HA + OH- • B+ + H2O H+ + BOH

  5. Salt or Hydrolysis Problems

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

  7. Salt Problem • Calculate the pH of a 0.10 M solution of R-NH3Cl • Kb = 2.5 x 10-5

  8. Drill: Calculate the pH of a 0.18 M solution of KC2H3O2 • Ka = 1.8 x 10-5

  9. Drill: Calculate the pH of a 0.16 M solution of KC7H5O2 • Ka = 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 • NaAc BaCl2 • KNO3 NH4Br • KHSO4 NH4Ac

  14. Predict Relative pH • KAc NaCl • KClO2 NH4Cl • K2SO4 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 • Na2O SO2 • NO2 CO2 • CaO Al2O3

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

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

  21. 7.4 g of Ca(OH)2 was added to 2.0 L of 0.075 M H2CO3. Calculate the molarity of all ions present in the solution.Ka1 = 4.4 x 10-7Ka2 = 4.7 x 10-11

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

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

  24. Calculate [H3PO4], [H2PO4-1], [HPO4-2], [PO4-3], [K+], [H+], & pH of 1.0 M KH2PO4 in 0.50 M K2HPO4. Ka1 = 7.5 x 10-3Ka2 = 6.2 x 10-8Ka3 = 4.2 x 10-13

  25. Calculate pH of: 0.50 M MOHin 0.20 M MCl Kb = 5.0 x 10-5

  26. Calculate pH of: 0.20 M MCl Kb = 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 KW, KA, KB, & pH

  32. Calculate pH of: • 0.025 M HNO3 • 0.020 M KOH

  33. Calculate pH of: • 2.0 M HNO2 • Ka = 2.0 x 10-4

  34. Calculate pH of: • 3.0 M HZin • 2.0 M KZ • Ka HZ = 3.0 x 10-5

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

  36. 150 mL of 0.10 M KOH was added to 100.0 mL of 0.10 M H2CO3. Calculate [H2CO3], [HCO3-], [CO3-2], [H+], [OH-], & pH of the solution.Ka1 = 4.4 x 10-7Ka2 = 4.7 x 10-11

  37. Calculate [H3A], [H2A-1], [HA-2], [A-3], [K+], [H+],[OH-], & pH of 2.0 M KH2A. Ka1 = 4.0 x 10-3Ka2 = 5.0 x 10-8Ka3 = 2.5 x 10-13

  38. Calculate pH of: • 2.0 M HQ • Ka = 2.0 x 10-6

  39. Calculate pH of: • 6.0 M HZin • 4.0 M KZ • Ka HZ = 3.0 x 10-5

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

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