Unit 7 · Equilibrium

Chapter 7.6

Solubility Equilibria and the Common-Ion Effect

Silver chloride barely dissolves in water, and it dissolves even less in salt water. The salt supplies chloride, and an equilibrium that already has product has nowhere to go.

in preparation · lesson 34 of 45

By the end

  1. 01Write K_sp for a sparingly soluble salt and relate it to molar solubility
  2. 02Compute K_sp from a measured solubility and solubility from K_sp
  3. 03Compare the solubilities of salts from their K_sp values
  4. 04Compute or explain the reduced solubility of a salt when a common ion is present

In unit 7

  1. 7.1Dynamic Equilibrium: When Nothing Seems to Change
  2. 7.2The Reaction Quotient and the Equilibrium Constant
  3. 7.3What the Size of K Tells You, and How K Values Combine
  4. 7.4Equilibrium Calculations and Particle Pictures
  5. 7.5Le Châtelier's Principle and the Reaction Quotient
  6. 7.6Solubility Equilibria and the Common-Ion Effect
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