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An ideal solution is one that has features that are similar to those of an ideal gas mixture. In ideal gases, therefore, there have been no interactions amongst gas molecules. However, we cannot apply the same logic to solutions since, in order to be termed a liquid, molecules in solutions would have to have intermolecular interactions amongst them. As a result of molecular engineering, optimal solutions differ from ideal gases. Non-ideal solutions are the ones that exist in the real world. However, certain solutions behave in a similar way to a perfect solution.The major difference between an ideal solution and a non-ideal solution is that in ideal solutions, all molecules have the same intermolecular interactions, whereas in non-ideal solutions, the forces between molecules between solutes and solvent molecules are different.
Ideal Solution
An ideal solution is one in which all of the molecules or ions have the same interactions with each other. There is also no resultant force between the solution’s parts. As a result, after combining a solute with a solvent, the spacing among molecules somehow doesn’t change. This is because, in order to alter the distance, a force must operate upon every as well as every molecule of the solute substance. An ideal solution has an enthalpy change of zero or very close to zero. This means that the enthalpy of the original parts is the same as the enthalpy of the mixed solution. As a result, the enthalpy of missing is equal to zero.
Non-Ideal Solution
A non-ideal solution is one in which the interaction among different molecules constituents in the solutions are not perfect. The magnitude of the intermolecular function can be used to identify a non-ideal solution. The interactions between the solvent and the solvent, as well as the solvent and the solute, can influence the value of a non-ideal solution. The solute has been well soluble in that solvent if the solvent-solute interactions are greater than the other two kinds of interactions. The end outcome is a less-than-ideal solution. On the other hand, highly dilute solutions exhibit ideal solution behaviour more often than non-ideal solution behaviour. This is because the number of solutes in a dilute is lower, resulting in less attraction between them.
Ideal and a Non-Ideal Solution: Difference
An ideal solution is one in which the connections between molecules are the same for all molecules or ions.
Non-ideal Solution: A non-ideal solution is one in which the actions with different molecule constituents in the solution differ.
Interactions of Various Types
- Ideal Solution: In an ideal solution, all of the molecules in all components interact in the same way
- Non-ideal solutions have interactions between the solvent and the solvent, the solvent and the solute, and the solute
Enthalpy
- Ideal Solution: When an ideal solution occurs, the enthalpy change is zero or almost zero
- Non-ideal Solution: When a non-ideal solution arises, the enthalpy change is either positive or negative
Realistic Alternatives
- Highly dilute solutions have the potential to function like perfect solutions
- Concentrated solutions have the properties of non-ideal solutions
| Ideal Solution | Non-Ideal Solution |
| They follow Raoult’s rules | They don’t follow Raoult’s rules |
| The solute-solvent molecular interactions are identical to that of pure components | The interaction between solute and the solvent is lower or higher than the connection among pure components |
| Raoult’s law predicts that the overall vapour pressure will be the same | According to Raoult’s law, the absolute vapour pressure increases or lowers the projected value |
| The enthalpy of mixing, Hmix = 0, is zero since no heat is emitted or absorbed | Heat will be either emitted or absorbed, resulting in a positive or negative enthalpy of mixing, Hmix 0 |
| Because the overall volume equals the sum of the component volumes (solute and solvent), the volume of the mixture is zero, Vmix = 0 | Vmix is not zero since the volume of blending is not zero. Either volume change occurs |
| Fractional distillation can be used to separate components | Fractional distillation cannot separate components in their pure form |
Hexane and heptane, for example, are benzene and toluene derivatives All of the dilute behave almost exactly like an ideal solution | Carbon disulphide and acetone, phenol and aniline, chloroform and acetone, and so on |
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Conclusion
Although no ideal gases exist, ideal solutions may exist in the real world. Because there is less interaction amongst solutes and solute-solvent molecules in very diluted solutions, they behave like perfect solutions. The major difference between an ideal solution and a non-ideal solution is that all molecules have the same intermolecular interactions in ideal solutions. In non-ideal solutions, the interaction forces between solvent and solute molecules are distinct.
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