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Acids and Bases intro

Learn about acids and bases, their definitions, dissociation reactions, and the self-ionization of water. Explore the Arrhenius and Bronsted-Lowry models, strong and weak acids, pH calculations, and the relationship between H3O+ and OH- ions.

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Acids and Bases intro

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  1. Acids and Bases intro

  2. Acid/Base Definitions • Arrhenius Model • Acids produce hydrogen ions in aqueous solutions • Bases produce hydroxide ions in aqueous solutions • Bronsted-Lowry Model • Acids are proton donors • Bases are proton acceptors

  3. Acid Dissociation HA  H+ + A- AcidProtonConjugate base Alternately, H+ may be written in its hydrated form, H3O+ (hydronium ion)

  4. for example… HCl  H+ + Cl- AcidProtonConjugate base

  5. Dissociation of Strong Acids Strong acids are assumed to dissociate completely in solution. Large Ka or small Ka? Reactant favored or product favored?

  6. Dissociation Constants: Strong Acids

  7. Dissociation of Weak Acids Weak acids are assumed to dissociate only slightly (less than 5%) in solution. Large Ka or small Ka? Reactant favored or product favored?

  8. Dissociation Constants: Weak Acids

  9. Self-Ionization of Water H2O + H2O  H3O+ + OH- At 25, [H3O+] = [OH-] = 1 x 10-7 Kw is a constant at 25 C: Kw = [H3O+][OH-] Kw = (1 x 10-7)(1 x 10-7) = 1 x 10-14

  10. Calculating pH, pOH pH = -log10(H3O+) pOH = -log10(OH-) Relationship between pH and pOH pH + pOH = 14 Finding [H3O+], [OH-] from pH, pOH [H3O+] = 10-pH [OH-] = 10-pOH

  11. pH and pOH Calculations

  12. pH Scale

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