For an example let's assume we have a weak acid HA . And we add either a strong or a weak base. Then what I want to know is whether the weak ionization of the acid HA taken place?.

Weak ionization of acid HA. ==> enter image description here

  • $\begingroup$ Yes it takes place, the reaction you wrote is correct, what exactly do you want to know ? $\endgroup$ – Ndrina Limani May 4 '15 at 9:57
  • $\begingroup$ So for a moment let's assume we add a base to this weak acid in order to reduce the H+ concentration, then what would really happen to the the concentration of this weak acid HA and the concentration of conjugate base?. $\endgroup$ – On the way to success May 4 '15 at 10:33

A weak acid does not (contrary to what you show in your equation) predominantly ionize before the base is added. But keep in mind that proton transfer reactions (at least those between oxygen and/or nitrogen atoms) occur almost instantaneously in both directions, so the equilibrium you illustrated is established immediately (for a weak acid, with the big arrow pointing left). So when (strong) base is added, H3O+ is consumed immediately, then more acid is ionized to re establish the equilibrium--and this goes on as you add more base until you have consumed almost all of the weak acid. These reactions are controlled by the relative energies of the reactants and products, and not by reaction rates.

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