Carboxylic acids have higher boiling points than aldehydes, ketones and even alcohols of comparable molecular mass. It is due to their

Question

The number of \(\pi\)-bonds present in benzoic acid is:

Answer 1

The question at hand is regarding the boiling points of carboxylic acids compared to aldehydes, ketones, and alcohols of similar molecular mass. Here's a step-by-step explanation:

Boiling points are influenced by intermolecular forces. The stronger these forces, the higher the boiling point.
Carboxylic acids are known to form strong intermolecular hydrogen bonds. This bonding occurs between the hydrogen atom of the hydroxyl group (-OH) of one carboxylic acid molecule and the oxygen atom of the carbonyl group (C=O) of another molecule.
This type of bonding results in the formation of dimers in the liquid phase, which effectively doubles the molecular size and significantly increases the boiling point.
Compared to aldehydes and ketones, which do not form such strong hydrogen bonds, and alcohols, which form weaker hydrogen bonds, the intermolecular hydrogen bonds in carboxylic acids are much stronger.

Given these points, the correct answer is due to the formation of intermolecular H-bonding.

Let's rule out the incorrect options:
Formation of intramolecular H-bonding: This is more typical in certain specific structural arrangements and doesn't significantly contribute to higher boiling points.
More extensive association via van der Waal's forces: While van der Waal's forces do exist, they are weaker than hydrogen bonds and are not the primary reason for the high boiling points.
Formation of carboxylate ion: This occurs during ionization, not in the context of boiling points.

In summary, the high boiling points of carboxylic acids relative to other similar molecules are primarily due to the formation of intermolecular hydrogen bonds.

Answer 2

The question at hand is regarding the boiling points of carboxylic acids compared to aldehydes, ketones, and alcohols of similar molecular mass. Here's a step-by-step explanation:

Boiling points are influenced by intermolecular forces. The stronger these forces, the higher the boiling point.
Carboxylic acids are known to form strong intermolecular hydrogen bonds. This bonding occurs between the hydrogen atom of the hydroxyl group (-OH) of one carboxylic acid molecule and the oxygen atom of the carbonyl group (C=O) of another molecule.
This type of bonding results in the formation of dimers in the liquid phase, which effectively doubles the molecular size and significantly increases the boiling point.
Compared to aldehydes and ketones, which do not form such strong hydrogen bonds, and alcohols, which form weaker hydrogen bonds, the intermolecular hydrogen bonds in carboxylic acids are much stronger.

Given these points, the correct answer is due to the formation of intermolecular H-bonding.

Let's rule out the incorrect options:
Formation of intramolecular H-bonding: This is more typical in certain specific structural arrangements and doesn't significantly contribute to higher boiling points.
More extensive association via van der Waal's forces: While van der Waal's forces do exist, they are weaker than hydrogen bonds and are not the primary reason for the high boiling points.
Formation of carboxylate ion: This occurs during ionization, not in the context of boiling points.

In summary, the high boiling points of carboxylic acids relative to other similar molecules are primarily due to the formation of intermolecular hydrogen bonds.

Carboxylic acids have higher boiling points than aldehydes, ketones and even alcohols of comparable molecular mass. It is due to their

The Correct Option is A

Solution and Explanation

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