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Acid Equilibrium and pH

Acid Equilibrium and pH. Søren Sørensen. 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 Lewis Acid Model

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Acid Equilibrium and pH

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  1. Acid Equilibrium and pH Søren Sørensen

  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 • Lewis Acid Model • Acids are electron pair acceptors • Bases are electron pair donors

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

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

  5. Dissociation Constants: Strong Acids

  6. 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?

  7. Dissociation Constants: Weak Acids

  8. 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

  9. 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

  10. pH and pOH Calculations

  11. The pH Scale Graphic: Wikimedia Commons user Slower

  12. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #1:Write the dissociation equation HC2H3O2 C2H3O2- + H+

  13. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #2:ICE it! HC2H3O2 C2H3O2- + H+ 0.50 0 0 +x +x - x x x 0.50 - x

  14. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #3:Set up the law of mass action HC2H3O2 C2H3O2- + H+ E 0.50 - x x x

  15. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #4:Solve for x, which is also [H+] HC2H3O2 C2H3O2- + H+ E 0.50 - x x x [H+] = 3.0 x 10-3 M

  16. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #5:Convert [H+] to pH HC2H3O2 C2H3O2- + H+ E 0.50 - x x x

  17. Text Pg. 671 Sample 16.1 and Practice • Sample 16.2 and Practice • Pg. 673 probably will not appear on AP test. • Equilibrium shifts from the stronger acid to the stronger base (table will not be available to id the strengths) • Pg. 674 and 675 Sample and practice • Pg. 677 use Kw to calculate [H+] or [OH-] • Pg. 677 16.6 and 16.7 Sample and practice

  18. Pg. 679 Indicators • Most important phenolphthalein • Pink in the presence of a base • Pg. 680 16.8 and 16.9 Sample and Practice • Pg. 683 Sample and practice

  19. Percent Ionization • Percent ionization = concentration ionized X 100 • original concentration • Percent ionization = [H+]equilibrium X 100 • [HA]initial • Pg. 684 Sample and practice • Pg. 685 Sample and practice

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