Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: AFT on December 04, 2008, 05:39:53 PM
-
I solved an assignment problem and I came to the conclusion that the % ionization of a strong acid decreases as the initial concentration of the ionized acid is increased.
I don't fully understand why this is..?
Any clarification would be greatly appreciated!
Thanks in advance!!
-
We can think of this phenomenon at molecular level.
Let's consider the acid HA, which consists of H+ and A-.
At low initial concentration, more water molecules are available for hydration of the H-A molecules, resulting in increasing ionization of the acid. But as we use more concentrated acid, the ionic interaction between the H+ and A- dominates (due to number) over the possible hydration provided by water, henceforth, the ionization decreases.
Hope my explanation helps