Asked by bill
How will the presence of hydrobromic acid affect the percent ionization of acetic acid?
Answers
Answered by
DrBob222
Acetic acid is CH3COOH. Let's save some typing by calling acetic acid HAc (The H from the COOH part and Ac for the CH3COO^- part).
HAc ==> H^+ + Ac^-
HBr ==> H^+ + Br^-
You know HBr is a strong acid; i.e., it is 100% ionized. Therefore, you are adding excess H^+ to the acetic acid (that is a common ion) and it will do what you think it will do; i.e., by LeChatelier's principle, the ionization of HAc will shift to the left which means less ionization and a smaller percent ionization.
HAc ==> H^+ + Ac^-
HBr ==> H^+ + Br^-
You know HBr is a strong acid; i.e., it is 100% ionized. Therefore, you are adding excess H^+ to the acetic acid (that is a common ion) and it will do what you think it will do; i.e., by LeChatelier's principle, the ionization of HAc will shift to the left which means less ionization and a smaller percent ionization.
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