Question

Hydrogen bonding increases the intermolecular forces of attraction and hence increased hydrogen bonding increases the solubility in a liquid. For example, Methyl alcohol which is organic in nature is miscible with water due to hydrogen bonding. For the same reason acetic acid is soluble in water due to hydrogen bonding. Acetic acid (CH3COOH) has got only one carbon atom and steric hindrance of the methy group is low which permits water (solvent) to get attached to solute. Can you elaborate more on hydrogen bonding as it relates to disolving a solute in a liquid? Please use more than 150 words.

Answer 1

Intermolecular forces:

Intermolecular forces are the forces that act between one molecule to other molecules as attraction. These are mainly three types:

1. Dipole-dipole interaction
2. Hydrogen bond
3. London dispersion force.

London dispersion force:

1. London dispersion force is an intermolecular force which occurs between an atoms or molecules which are polar or non-polar and another atom or molecule which are polar or non-polar.
2. It occurs between all molecules or atom.
3. London dispersion forces are the result of temporary dipoles in the atoms or molecules.

Dipole-dipole interaction:

1. This type of interaction forces is found between polar molecules.
2. The strength of this force is increasing with increasing polarity of molecules.

Hydrogen bond:

1. Generally hydrogen bond is found in those molecules which have covalently hydrogen atom bonded with high electronegative atoms like oxygen, nitrogen and fluorine.

Hydrogen bond found in polar molecules containing unpaired electrons along with a hydrogen atom bonded with oxygen, nitrogen or fluorine atom

Solubility of substance depends on the following three relatives’ strengths:

1. Solute –solute
2. Solvent-solvent
3. Solute –solvent