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Acid/ Base Definitions

Acid/ Base Definitions. Arrhenius Definitions. Acid – H + /H 3 O + producer Base – OH - producer Good for strong acids and bases. Bronsted-Lowry Definition. Acid – proton (H + ) donor Base – proton acceptor Accounts for some weak bases which do not have an OH -. Lewis Definition.

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Acid/ Base Definitions

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  1. Acid/ Base Definitions

  2. Arrhenius Definitions • Acid – H+/H3O+ producer • Base – OH- producer • Good for strong acids and bases

  3. Bronsted-Lowry Definition • Acid – proton (H+) donor • Base – proton acceptor • Accounts for some weak bases which do not have an OH-

  4. Lewis Definition • Acid – electron pair acceptor • Base – electron pair donor • Encompasses even more than the Bronsted-Lowry definition

  5. Identify the Lewis acid and base Ni2+ + 6NH3 Ni(NH3)62+ H+ + H2O  H3O+

  6. Conjugate Acid/Base • In every acid/base reaction, there are actually two acids and two bases • NH3 + HF → F- + NH4+ • On the reactant side, HF is an acid so it has a Ka, but on the product side F- the is a base so it has a Kb

  7. Relationship Between Ka and Kb • Ka x Kb = Kw • pK = - log K • pKa + pKb = 14.00

  8. Example • Calculate the Kb for the F- ion if the Ka for its conjugate acid is given in Appendix A5.1. • Calculate the Ka for the ammonium ion, NH4+.

  9. Example • Calculate the pH of a .30M NaF solution. The Ka for HF is 7.2x10-4.

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