[miaou5]

According to my prof, for strong acids, there is technically no half equivalence point, since the half equivalence point is when the concentration of weak base to weak acid is 1 ([weak base]/[weak acid] = 1). Since the conjugate base of a strong acid is actually not basic at all, strong acids do not have a half equivalence point and cannot act as buffers.

^ Is it true that strong acids have no half-equivalence point? And does this mean that the Henderson-Hasselbalch equation doesn't apply to strong acids? In other words, I wouldn't be able to use pH to find Ka of a strong acid during a titration, even if [HCl] happened to be equal to [Cl-]?

Big thanks!!

[Hunter2]

Yes correct. Strong acids dont have buffer behaviour, so HH-equation doesnt work. A mixture of sodium chloride and hydrochloric acid works like the pure hydrochloric acid. The amount of chloride ions is unimportant.