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With the question attached, I just want clarity on why wouldn't increasing the amount of acetic acid influence percent dissociation if the amount protons are increased according to Le Chatelier's Principle?
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Increasing the amount of acetic acid will increase the raw amount of protons in solution (read: hydronium ions), but it will not increase the proportion that dissociate. In fact, it will decrease it as I add more and more acetic acid - the reaction environment becomes more acidic, making it harder, not easier, for newly added acetic acid molecules to lose their proton.
Ok so does this scenario relate to the common ion effect where basically since I already have the acetic acid in solution; adding more of it will introduce a common ion making it less likely to ionize/dissociate?
Pretty much. The more acid I add, the less likely future acids are to dissociate.