Why do carboxylic acids generally have higher melting and boiling points than alcohols, ketones, and aldehydes?

carboxylic acids with the presence of -COOH groups are capable of hydrogen bonding between molecules and more energy is necessary to overcome this additional intermolecular bonding, hence, the melting and boiling points for carboxylic acids are generally higher.

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Carboxylic Acid Melting Point

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Why do carboxylic acids generally have higher melting and boiling points than alcohols, ketones, and aldehydes?

Why do carboxylic acids generally have higher melting and boiling points than alcohols, ketones, and aldehydes of comparable mass?

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The acid group is stabilized through resonance. The double bond can lie on either of the oxygens, and that stabilizes the molecule. More stable molecules have higher boiling points (and melting points). Alcohols, ketones, and aldehydes to not have resonance to stabilize them, so their boiling points are much lower.

this is so because the above mentioned carboxylic acids have stronger bonds/ van der walls forces between them thus it takes a much higher amount of heat to break the forces thus the higher melting and boiling points

because more energy is require to break the o-h bonds in carboxylic acids