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Chapter 17

Chapter 17. Additional aspects of aqueous equilibria. Common Ion Effect. Whenever a weak electrolyte and a strong electrolyte contain a common ion, the weak electrolyte ionizes less than it would if it were alone in solution LeChatlier’s Principle

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Chapter 17

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  1. Chapter 17 Additional aspects of aqueous equilibria

  2. Common Ion Effect • Whenever a weak electrolyte and a strong electrolyte contain a common ion, the weak electrolyte ionizes less than it would if it were alone in solution • LeChatlier’s Principle • Which one of these solutions would you expect would have the least H+? 2 M HCl 2 M Acetic Acid (HC2H3O2) or Solution with 2M Acetic acid and 2M sodium acetate?

  3. Demonstration For the reaction CaCO3 + 2H+ CO2 + H2O + Ca2+ Rate = k[H+]2 Predict which cylinder will react fastest Cylinder #1 100mL of 2M HCl Cylinder #2 100mL of 2M Acetic acid Cylinder #3 100mL of 2M Acetic acid/ sodium acetate

  4. Buffered solutions • Buffer is something which resists changes in pH. It does this because it contains significant amounts of an acid & its conjugate base or a base and its conjugate acid • The acid can neutralize excess base and the base can neutralize excess acid

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