Acid dissociation constant
Acid dissociation constant (also known as Ka) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions.
Definition[edit | edit source]
The acid dissociation constant is defined by the following equation:
- Ka = [A-][H3O+] / [HA]
where [A-] is the concentration of the acid anion, [H3O+] is the concentration of the hydronium ion, and [HA] is the concentration of the acid. The larger the Ka, the more the acid dissociates and the stronger the acid.
Determination[edit | edit source]
The acid dissociation constant can be determined experimentally by measuring the pH of a solution containing the acid and using the Henderson-Hasselbalch equation. It can also be calculated from the standard Gibbs free energy change for the dissociation reaction.
Applications[edit | edit source]
The acid dissociation constant is used in many areas of chemistry, including analytical chemistry, environmental chemistry, and biochemistry. It is particularly important in the field of acid-base chemistry, where it is used to predict the outcome of reactions and to calculate the pH of solutions.
See also[edit | edit source]
References[edit | edit source]
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