What happens to stronger acids concerning their conjugate bases?

Stronger acids are characterized by their ability to donate protons (H⁺) more readily compared to weaker acids. When a strong acid donates a proton, it forms its conjugate base. The strength of an acid is inversely related to the strength of its conjugate base; this means that the stronger the acid, the weaker its conjugate base will be.

This relationship can be understood through the concept of acidity and basicity within the context of the acid-base theory. A strong acid fully dissociates in solution, resulting in a high concentration of H⁺ ions. The conjugate base of a strong acid, therefore, has a lower tendency to re-accept a proton, making it a weak base. This is why stronger acids correspond to weak conjugate bases.

Ultimately, this fundamental principle of acid-base chemistry highlights the connection between the strength of acids and the corresponding weak nature of their conjugate bases, validating that stronger acids indeed have weaker conjugate bases.