Different intermolecular attractions accessible to solvent molecules cause various solvent effects, in part.
Certain solvents form hydrogen bonds. A fairly typical example is water, as well as alcohols like methanol. Others don't donate hydrogen bonds; they can only accept them.
Some solvents may more effectively stabilize the anions that result from the deprotonation of Bronsted acids. As a result, when measured in various solvents, pKa values may vary.
<h3>What is pKa value?</h3>
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).
How tightly a proton is retained by a Bronsted acid is how the strength of an acid is measured.
