Equilibrium Constant Definition

The equilibrium constant is a ratio based on equilibrium concentrations.
The equilibrium constant is a ratio based on equilibrium concentrations. Rafe Swan, Getty Images
By
Anne Marie Helmenstine, Ph.D.
Chemistry Expert
  • Ph.D., Biomedical Sciences, University of Tennessee at Knoxville
  • B.A., Physics and Mathematics, Hastings College
Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. She has taught science courses at the high school, college, and graduate levels.
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Anne Marie Helmenstine, Ph.D.
Updated March 08, 2019

The equilibrium constant is the ratio of the equilibrium concentrations of the products raised to the power of their stoichiometric coefficients to the equilibrium concentrations of the reactants raised to the power of their stoichiometric coefficients.
For a reversible reaction:
aA + bB → cC + dD
The equilibrium constant, K, is equal to:
K = [C]c·[D]d/[A]a·[B]b
where
[A] = equilibrium concentration of A
[B] = equilibrium concentration of B
[C] = equilibrium concentration of C
[D] = equilibrium concentration of D

There are several different types of equilibrium constants. These including binding constants, association constants, dissocation constants, stability constants, and formation constants.

Factors that may affect the equilibrium constant include temperature, ionic strength, and choice of solvent.

Source

  • Denbigh, K. (1981). "Chapter 4". The Principles of Chemical Equilibrium (4th ed.). Cambridge: Cambridge University Press. ISBN 978-0-521-28150-8.