Why are some acids and bases stronger then others?
Actually, the key to the answer for this question is the relative strength of conjugate bases. The more readily a pair of electrons can be shared with an H^+, the stronger the base. A strong acid has an H in it that is bonded to another atom which does not share the bonding electrons easily with the H, usually because of low charge density on the conjugate base atom due high electronegativity and large size as well as resonance. Thus, in a strong acid, it is easy for water to take the H+ away by sharing one of the electron pairs on the water’s O atom with the H+ to replace the ones in the original bond to the conjugate base. The bond that was holding the H in the acid is now an unshared pair of electrons on the atom left behind. (Often that atom is part of a larger structure such as the O^- in HSO4^- when the H is removed from H2SO4) If the pair of electrons is well stabilized, the conjugate base is weak, and the original acid was strong. If the pair of electrons is not stabilized very
