Chemists use equilibrium constants, or Keq values, to express whether a reversible chemical reactions favours the formation of products or reactants. Acetic acid, or CH3COOH, for example, undergoes a partial reaction with water according to CH3COOH + H2O <---> CH3COO- + H3O+. An equilibrium constant greater than one would indicate that most of the acetic acid molecules convert to CH3COO-. An equilibrium constant less than one would indicate that most of the acetic acid molecules remain intact. When specifically applied to acids, chemists refer to equilibrium constants as acid-dissociation constants, or Ka values. These numbers are typically very small. The value for acetic acid, for example, is 0.000018, or 1.8 x 10^-5. Consequently, chemists sometimes express these quantities as pKa values, where pKa = -log Ka. In this case, the pKa of acetic acid becomes pKa = -log (0.000018) = 4.74.
Refer to a table of pKa values and locate the pKa of the compound under investigation. For example, the pKa of benzoic acid, a common food preservative, is about 4.20.
Multiply the pKa value by negative one to invert its sign. In the case of benzoic acid, 4.20 x (-1) = -4.20.
Calculate the Ka or Keq value by using a calculator to raise 10 to the power of the negative pKa. Continuing the previous example, if benzoic acid exhibits a pKa of 4.20, then its Ka = 10^(-4.20) = 6.31 x 10^-5, or 0.0000631. And because benzoic acid is acidic, its Keq and Ka values are numerically identical.
- Worcester Polytechnic Institute, Department of Chemistry: Chapter 12: Principles of Chemical Equilibrium
- Foothill College: Acid-Base Equilibrium Constants, Ka and Kb
- Purdue University, Department of Chemistry: Weak Acids and Equilibrium
- University of California, Los Angeles, Department of Chemistry: Acids and Bases: Use of the pKa Table
- Mathematically, raising 10 to an exponential power is referred to as the "antilog" and the button for this operation is usually marked "10^x" on most scientific calculators.
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