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Ch.16. Acids and Bases (the fundamentals)

Ch.16. Acids and Bases (the fundamentals). Contents. 16-1 The Arrhenius Theory: A Brief Review 16-2 Br ønsted-Lowry Theory of Acids and Bases 16-3 The Self-Ionization of Water and the pH Scale 16-4 Strong Acids and Strong Bases 16-5 Weak Acids and Weak Bases 16-6 Polyprotic Acids

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Ch.16. Acids and Bases (the fundamentals)

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  1. Ch.16. Acids and Bases (the fundamentals)

  2. Contents 16-1 The Arrhenius Theory: A Brief Review 16-2 Brønsted-Lowry Theory of Acids and Bases 16-3 The Self-Ionization of Water and the pH Scale 16-4 Strong Acids and Strong Bases 16-5 Weak Acids and Weak Bases 16-6 Polyprotic Acids 16-7 Ions as Acids and Bases 16-8Molecular Structure Acid-Base Behavior

  3. H2O NaOH(s) → Na+(aq) + OH-(aq) 16-1 The Arrhenius Theory: A Brief Review H2O HCl(g) → H+(aq) + Cl-(aq) Na+(aq) + OH-(aq)+ H+(aq) + Cl-(aq) → H2O(l) + Na+(aq) + Cl-(aq) H+(aq)+ OH-(aq) → H2O(l) Arrhenius theory did not handle non OH- bases such as ammonia very well.

  4. 16-2 Brønsted-Lowry Theory of Acids and Bases • An acid is a proton donor. • A base is a proton acceptor. conjugate acid conjugate base base acid NH3 + H2O NH4+ + OH- NH4+ + OH- NH3 + H2O ?? ?? acid base

  5. The Solvated Proton

  6. [NH4+][OH-] Kc= [NH3][H2O] [NH4+][OH-] Kb= Kc[H2O] = = 1.810-5 [NH3] Base Ionization Constant conjugate base conjugate acid base acid NH3 + H2O NH4+ + OH-

  7. [CH3CO2-][H3O+] Kc= [CH3CO2H][H2O] [CH3CO2-][H3O+] Ka= Kc[H2O] = = 1.810-5 [CH3CO2H] Acid Ionization Constant conjugate base conjugate acid acid base CH3CO2H+ H2O CH3CO2- + H3O+

  8. A Weak Base

  9. A Weak Acid

  10. A Strong Acid

  11. Worked Examples Follow:

  12. CRS Questions Follow:

  13. - - + + In the reaction depicted below, which species are acids?

  14. - - + + In the reaction depicted below, which species are acids?

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