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Common Ion Effect

The content delves into the common ion effect, explaining its significance in altering the solubility of compounds, with a focus on its application in advanced problem-solving scenarios such as the MCAT. It covers the theoretical underpinnings through Le Chatelier's Principle, mathematical calculations using ICE tables, and practical applications including complex ion formation and pH's impact on solubility.
  • The common ion effect decreases a salt's solubility when one of its ions is already present in the solution, demonstrated through Le Chatelier's Principle.
  • ICE tables are introduced as a method to calculate changes in solubility, highlighting the initial, change, and equilibrium stages of a reaction.
  • Complex ion formation can increase the solubility of a compound by removing one of the ions from the solution, significantly altering the equilibrium.
  • The role of pH in changing solubility is explored, showing how the presence of weak acids or bases can affect the solubility of certain compounds.
  • Practical examples, including the impact of fluoride on dental health and the selection of compounds to precipitate fluoride ions, illustrate the common ion effect's relevance in healthcare.
Understanding the Common Ion Effect
Calculating Solubility Changes
Complex Ion Formation and Solubility
The Impact of pH on Solubility
Applying the Common Ion Effect in Healthcare