A monoprotic weak acid, HA , is ionized according to the reaction
HA(aq)+H2O(l)↽−−⇀A−(aq)+H3O+(aq)
pKa=4.10
where A− is the conjugate base to HA.
For this weak monoprotic acid, the predominant species present at pH 2.94 is:
charged
neutral
unknown
for which I assumed, as the pH is less than pKa, there would be a higher [H3O+] than at equilibrium; the solution, however, is "neutral" rather than "charged". Why is this so?