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Due to double bond carbonyl oxygen is less hindered as compare to hydoxyl oxygen, therefore its electron pairs are easily available for proton.

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Q: Explain why the carbonyl oxygen in the acid-base protonation reaction of acetic acid preferentially gets protonated over the hydroxyl group in the acetic acid?
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When protonation occurs with carboxylic acid why does the H plus cation go to the carbonyl oxygen?

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