Boiling points of `CH_3COOH` (mol.wt=60) is higher than that of `CH_3CH_2CH_2OH` (mol.wt=60). It is due to

Options

A. Intramolecular H-bonding between two carboxylic acid molecules at two point which is at one points only in alcohol
B. strong van der Waals’ forces
C. intramolecular H-bonding
D. None of the above

Answer

To determine why the boiling point of acetic acid (CH₃COOH) is higher than that of propanol (CH₃CH₂CH₂OH), we can analyze the intermolecular forces at play, particularly hydrogen bonding.

### Step-by-Step Solution:

1. **Identify the Compounds**:
- Acetic acid (CH₃COOH) and propanol (CH₃CH₂CH₂OH) both have the same molecular weight (60 g/mol).

2. **Understand Hydrogen Bonding**:
- Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (like oxygen) and is attracted to another electronegative atom in a different molecule.
- Acetic acid has a carboxylic acid functional group (-COOH) which can form two hydrogen bonds: one from the hydrogen of the -OH group and one from the carbonyl oxygen (C=O).

3. **Compare Hydrogen Bonding in Both Compounds**:
- In acetic acid, each molecule can form two hydrogen bonds with neighboring acetic acid molecules.
- In propanol, each molecule can form only one hydrogen bond (from the -OH group).

4. **Intermolecular Forces**:
- The stronger the intermolecular forces, the higher the boiling point. Since acetic acid can form more hydrogen bonds compared to propanol, it has stronger intermolecular forces.

5. **Conclusion**:
- The higher boiling point of acetic acid compared to propanol is due to the greater number of hydrogen bonds formed between acetic acid molecules, resulting in stronger intermolecular forces.

### Final Answer:
The boiling point of CH₃COOH is higher than that of CH₃CH₂CH₂OH due to the presence of stronger hydrogen bonding in acetic acid, which allows it to form more hydrogen bonds compared to propanol.