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Trichloroacetic acid is stronger. The Cls bonded to the molecule in place of the hydrogen has a greater electron-withdrawing power contributing to anion stability when it loses the proton.
Yes it is. The reasoning behind it being stronger is that the anion created from trichloroacetic is more stable than acetic acid. This is due to the Cl's delocalizing the negative charge of the oxygen and the resonance structure that is created when the H is broken off.
Yes, because the Cl's in trichloroacetic acid pulls more on the electrons in the anion than the H's in acetic acid. The resonance in trichloroacetic acid also makes it relatively strong.
The chlorine, since it has a higher electronegativity, is able to withdraw more electron density from the oxygen resulting in more delocalized electrons and a more stable resulting anion. This is why trichloroacetic acid is the stronger acid
After dissociating H+, the resulting anion for trichloroacetic acid is more stable as Cl is electronegative and withdraws the negative charge. Therefore it's more stronger than the acetic acid.
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