In the titration of a weak acid with a strong base, the point where half of the acid has reacted with the base is noteworthy because the ph equals: the pKa.
In layman's terms, pKa is a measurement of an acid's strength. A strong acid will have a pKa value that is lower than 0. To be more specific, pKa is the Ka value's negative log base ten value (acid dissociation constant). It gauges an acid's potency by determining how firmly a proton is retained by a Bronsted acid.
The strength of the acid and its capacity to donate protons increase with decreasing pKa values.
Acid dissociation constant, Ka, gauges how well an acid separates from its water-soluble constituents. Since acid generally dissociates into its ions, the stronger the acid, the higher the value of Ka.
The following equation describes the connection between pKa and Ka:
pKa = –log[Ka]
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