What happens to stronger acids in an aqueous solution according to solvent leveling?

Stronger acids in an aqueous solution are indeed affected by solvent leveling, which is a principle stating that in a certain solvent, strong acids can only exist in their ionized form to a certain extent dictated by the autoionization of the solvent itself. In water, the strongest acids will completely dissociate into hydronium ions and their conjugate bases, which means their behavior deviates from what would be observed in non-aqueous solvents where they might remain in a more basic form.

In the case of water, any acid that is stronger than hydronium ion will behave like a weaker acid due to this leveling effect. Hence, when comparing their behavior in aqueous solutions to that in non-aqueous solvents, they are observed to be weaker than they would be under those conditions, as the predominant species tends to be the hydronium ion rather than the acid itself in a non-dissociated form. This reflects the concept of solvent leveling, where strong acids appear to be weaker due to the limitations imposed by the solvent in effectively stabilizing the dissociated species.