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In 0.1 M solution, weak electrolyte, acetic acid is 1.3% dissociated. If you 100 molecules of acetic acid are placed originally in the solution, how many acid molecules remain minimized at equilibrium?
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In 0.1 M solution, weak electrolyte, acetic acid is 1.3% dissociated. ...
We start with 0.1 M CH3COOH, which we are told is 1.3% ionized. We add 100 molecules of CH3COOH to this solution. Now, now many of those 100 molecules remain unionized when the equilibrium is re-established?

Can’t be answered. We don’t know the volume of the original 0.1 M solution, so we can’t know how the 100 molecules changes the original concentration.

If we assume some significant volume, then the vanishingly tiny number of added molecules won’t change the concentration perceptibly, so the same 1.3% dissociation will still pertain, and 98 or 99 of the added molecules will remain non-ionized.

A lot of assuming here. A very weird question that doesn’t seem to carry very much pedagogic value.
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In 0.1 M solution, weak electrolyte, acetic acid is 1.3% dissociated. If you 100 molecules of acetic acid are placed originally in the solution, how many acid molecules remain minimized at equilibrium?
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