1. Non-polar solvent:
* Dissolves: The solute will dissolve readily in the non-polar solvent due to the principle of "like dissolves like". Both the solute and solvent have similar intermolecular forces, primarily van der Waals forces, which allow them to interact and mix freely. Examples include oil dissolving in gasoline.
2. Polar solvent:
* Does not dissolve: The solute will not dissolve significantly in a polar solvent. This is because the non-polar solute's intermolecular forces are weaker than the strong hydrogen bonds or dipole-dipole interactions present in the polar solvent. The solvent molecules will prefer to interact with each other rather than the non-polar solute. Examples include oil not dissolving in water.
3. Amphiphilic solvent:
* Partially dissolves: Some non-polar solutes can partially dissolve in amphiphilic solvents (having both polar and non-polar parts). This is because the non-polar part of the solvent can interact with the solute, while the polar part can interact with the surrounding water molecules. This is how soap and detergents work, with their non-polar tails interacting with grease and their polar heads interacting with water.
Key principles:
* "Like dissolves like": Solutes tend to dissolve best in solvents that have similar intermolecular forces.
* Intermolecular forces: The strength and type of intermolecular forces between solute and solvent molecules determine the solubility.
Examples:
* Non-polar solute & non-polar solvent: Oil in gasoline
* Non-polar solute & polar solvent: Oil in water
* Non-polar solute & amphiphilic solvent: Grease in soap solution
Note: Even though a non-polar solute may not fully dissolve in a polar solvent, it may still form a suspension or emulsion where small droplets of the solute are dispersed throughout the solvent.
