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Understanding Aqueous Equilibria: The Common Ion Effect and Buffers

This chapter explores key concepts in aqueous equilibria, focusing on the common ion effect and its implications for weak and strong electrolytes in solution. It highlights Le Chatelier’s Principle and predicts how the presence of a common ion influences ionization in weak electrolytes. A comparison between HCl, acetic acid, and buffered solutions illustrates varying H+ concentrations, alongside the demonstration of reaction rates in different cylinders. Furthermore, the fundamental characteristics of buffer solutions are discussed, emphasizing their role in resisting pH changes.

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Understanding Aqueous Equilibria: The Common Ion Effect and Buffers

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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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