Editing Solution (chemistry) (section)

== Solubility ==
{{Main article|Solubility|Solvation}}
The ability of one [[Chemical compound|compound]] to dissolve in another compound is called [[solubility]].{{clarify|what if one or both of the components is not a compound?|date=August 2021}} When a liquid can completely dissolve in another liquid the two liquids are ''miscible''. Two substances that can never mix to form a solution are said to be ''immiscible''.

All solutions have a positive [[entropy]] of mixing. The interactions between different molecules or ions may be energetically favored or not. If interactions are unfavorable, then the [[Thermodynamic free energy|free energy]] decreases with increasing solute concentration. At some point, the energy loss outweighs the entropy gain, and no more solute particles{{clarify|kind of particles|date=August 2021}} can be dissolved; the solution is said to be [[Saturated solution|saturated]]. However, the point at which a solution can become saturated can change significantly with different environmental factors, such as [[temperature]], [[pressure]], and contamination. For some solute-solvent combinations, a [[supersaturated]] solution can be prepared by raising the solubility (for example by increasing the temperature) to dissolve more solute and then lowering it (for example by cooling).

Usually, the greater the temperature of the solvent, the more of a given solid solute it can dissolve. However, most gases and some compounds exhibit solubilities that decrease with increased temperature. Such behavior is a result of an [[exothermic]] [[enthalpy of solution]]. Some [[surfactant]]s exhibit this behaviour. The solubility of liquids in liquids is generally less temperature-sensitive than that of solids or gases.