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Chapter 24: Problem 53

Pure acetic acid is a viscous liquid, with high melting and boiling points \(\left(16.7^{\circ} \mathrm{C}\right.\) and $\left.118^{\circ} \mathrm{C}\right)$ compared to compounds of similar molecular weight. Suggest an explanation.

Short Answer

Expert verified
The high melting and boiling points of pure acetic acid compared to compounds of similar molecular weight can be attributed to its strong intermolecular forces, including both dipole-dipole interactions and hydrogen bonding. The presence of these strong forces means that more energy is required to overcome them, thus resulting in elevated melting and boiling points. Comparatively, compounds like ethyl ether, with weaker intermolecular forces, exhibit lower boiling points.

Step by step solution

01

Identify the molecular structure of acetic acid

Acetic acid has the molecular formula CH3COOH. The structure of acetic acid includes a carboxyl group (-COOH) bonded to a methyl group (CH3). In the carboxyl group, there's an oxygen atom double bonded to a carbon atom, and a hydroxyl group (-OH) bonded to the same carbon atom. This structure plays an important role in the intermolecular forces it exhibits.
02

Identify the intermolecular forces acting in acetic acid

Intermolecular forces are the forces between molecules that hold them together. There are three main types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding. Due to the presence of polar bonds (C=O and O-H) in the acetic acid molecule, it exhibits dipole-dipole interactions. Also, the presence of a hydroxyl group (-OH) allows for strong hydrogen bonding interactions.
03

Explain the effect of intermolecular forces on physical properties

Substances with strong intermolecular forces require more energy to overcome these forces, leading to higher melting and boiling points. In the case of acetic acid, both dipole-dipole and hydrogen bonding interactions contribute to the strength of the intermolecular forces, leading to high melting and boiling points.
04

Compare acetic acid with compounds of similar molecular weight

Let's compare acetic acid to a compound with a similar molecular weight that doesn't have strong intermolecular forces, such as ethyl ether (C2H5OCH2CH3). Ethyl ether has a lower boiling point of 34.6°C due to weaker London dispersion forces and minor dipole-dipole interactions. There is no hydrogen bonding present in ethyl ether, making its intermolecular forces weaker than those in acetic acid.
05

Conclusion

The high melting and boiling points of pure acetic acid compared to compounds of similar molecular weight can be explained by the presence of strong intermolecular forces in acetic acid, particularly hydrogen bonding, which require more energy to overcome.

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