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Smaller concentrations of weak acid dissociate more, why?
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Topic: Smaller concentrations of weak acid dissociate more, why? (Read 1414 times)
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user11
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Smaller concentrations of weak acid dissociate more, why?
«
on:
February 20, 2014, 11:07:43 AM »
Hi, how can you explain on a molecular level why a higher % of a weak acid dissociates at really small concentrations?
I can't really visualize which driving forces would push the equilibrium to the right, thus forming a higher % of H+ and would appreciate some help
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ncehlesnon
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Re: Smaller concentrations of weak acid dissociate more, why?
«
Reply #1 on:
February 21, 2014, 12:59:59 AM »
I think we can see it in this way:the process of dissociating is HAc+H2O==Ac
-
+H3O
+
, so the more existence of water makes the balance moves to the right.
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Smaller concentrations of weak acid dissociate more, why?