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Ka, the acid ionization constant, is the equilibrium constant for chemical reactions involving weak acids in aqueous solution. The numerical value of Ka is used to predict the extent of acid dissociation.
There is a simple relationship between the magnitude of Ka for an acid and Kb for its conjugate base. Consider, for example, the ionization of hydrocyanic acid (HCN) in water to produce an acidic solution, and the reaction of CN − with water to produce a basic solution: HCN (aq) ⇌ H + (aq) + CN − (aq) CN − (aq) + H2O (l) ⇌ OH − (aq) + HCN (aq)
What is K a in Chemistry? The acid dissociation constant (Ka) is used to differentiate between strong and weak acids. The acid dissociates more as the Ka increases. Strong acids must therefore dissociate more in water. A weak acid, on the other hand, is less likely to ionise and release a hydrogen ion, leading to a less acidic solution.
Revision notes on 5.5.2 pH, Ka, pKa & Kw Calculations for the CIE A Level Chemistry syllabus, written by the Chemistry experts at Save My Exams.
For an aqueous solution of a weak acid, the dissociation constant is called the acid ionization constant (Ka). Similarly, the equilibrium constant for the reaction of a weak base with water is the base ionization constant (Kb).
Read this tutorial for information on Ka, the acid dissociation constant. You will learn how to use this value to calculate pKa and pH!
Every acid has a characteristic dissociation constant (K a), which is a measure of its ability to donate hydrogen ions in solution. In other words, K a provides a way to gauge the strength of an acid. Larger values signify stronger acids.