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The percent dissociation for a weak acid is given by the following relationship: % Dissociation =...

The percent dissociation for a weak acid is given by the following relationship:

% Dissociation =   \frac{[A^-]}{[HA]_{0}}\cdot 100

for                                                                           HA + H2O ? H3O+ + A-

Show mathematically that doubling the initial concentration of weak acid lowers the % dissociation. Hint: Start with [HA]o and solve ICE problem for this initial condition, then do the same for [HA]o/2.

*It seems obvious to me that doubling the initial concentration would lower the % dissociation based on the% dissociation equation. I'm having trouble incorporating the ICE tables. Can anyone show me how to do that?

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