Explain the effects of the degree of dissociation of a solute on the boiling point of a solution.

The degree of dissociation of a solute refers to the extent to which the solute molecules break apart into ions when dissolved in a solvent. When a solute dissociates, it increases the number of particles in the solution, which in turn affects the boiling point of the solution.

According to Raoult's Law, the boiling point of a solution is directly proportional to the concentration of solute particles in the solution. This means that as the degree of dissociation of a solute increases, the number of particles in the solution also increases, leading to a higher boiling point.

For example, if a solute completely dissociates into ions when dissolved in a solvent, it will contribute more particles to the solution compared to a solute that only partially dissociates. As a result, the solution with the completely dissociated solute will have a higher boiling point than the solution with the partially dissociated solute.

In summary, the degree of dissociation of a solute directly affects the boiling point of a solution by increasing the number of particles in the solution, which in turn increases the boiling point of the solution.

The degree of dissociation of a solute refers to the extent to which the solute particles break down into ions or smaller molecules when dissolved in a solvent. This dissociation affects the boiling point of a solution in several ways:

1. Van't Hoff Factor:

The van't Hoff factor (i) is used to account for the effect of dissociation on colligative properties like boiling point elevation. For a solute that dissociates into n ions, the i value is:

```
i = n + 1
```

For example, if a solute dissociates into two ions (AB → A+ + B-), the van't Hoff factor would be 3.

2. Boiling Point Elevation:

The boiling point elevation of a solution (ΔTb) is directly proportional to the van't Hoff factor:

```
ΔTb = Kb - i - m
```

where:

- Kb is the boiling point elevation constant of the solvent
- i is the van't Hoff factor
- m is the molality of the solution

3. Number of Particles:

The degree of dissociation increases the number of particles in the solution. When the solute dissociates, it creates more ions or molecules, which increases the number of solute particles present.

4. Intermolecular Forces:

Dissociation reduces the intermolecular forces between solute particles, as they are now separated by solvent molecules. This weakens the attractive forces holding the particles together, making it easier for them to vaporize and contribute to the vapor pressure.

5. Vapor Pressure:

The vapor pressure of a solution is the pressure exerted by the vapor of the solvent and solute above the liquid. Dissociation increases the vapor pressure because of the increased number of particles and reduced intermolecular forces.

6. Boiling Point:

The boiling point of a liquid is the temperature at which its vapor pressure equals the external atmospheric pressure. As dissociation increases the vapor pressure, it lowers the boiling point of the solution.

Conclusion:

The degree of dissociation of a solute affects the boiling point of a solution by altering the van't Hoff factor, increasing the number of particles, reducing intermolecular forces, and increasing the vapor pressure. This results in a lower boiling point for solutions with highly dissociated solutes compared to solutions with non-dissociated solutes.