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7.7 Calculating Equilibrium Concentrations

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Calculating Q and K

In order to calculate the final concentrations in a reaction that achieve the equilibrium constant value, one way we can do this is through an ICE Table. ICE stands for initial, change, and equilibrium, which combines values from the equilibrium constant with the stoichiometry of the reaction to calculate the final concentration of the reactants and products when equilibrium is reached. Let’s do an example with the reaction involving the dissolution of hydrocyanic acid, shown below.

HCN⇆H++CN−HCN \leftrightarrows H^+ + CN^-

In this unit

12 lessons

  1. 7.1Introduction to EquilibriumPreview lesson
  2. 7.2Direction of Reversible ReactionsPreview lesson
  3. 7.3Reaction Quotient and Equilibrium ConstantPreview lesson
  4. 7.4Calculating the Equilibrium ConstantPreview lesson
  5. 7.5Magnitude of the Equilibrium ConstantPreview lesson
  6. 7.6Properties of the Equilibrium ConstantPreview lesson
  7. 7.7Calculating Equilibrium ConcentrationsThis lesson
  8. 7.8Representations of EquilibriumPreview lesson
  9. 7.9Introduction to Le Châtelier’s PrinciplePreview lesson
  10. 7.10Reaction Quotient and Le Châtelier’s PrinciplePreview lesson
  11. 7.11Introduction to Solubility EquilibriaPreview lesson
  12. 7.12Common-Ion EffectPreview lesson

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