
Examples of solid solutions are alloys, certain minerals and polymers containing plasticizers. The ability of one compound to dissolve in another compound is called solubility. The physical properties of compounds such as melting point and boiling point change when other compounds are added. Together they are called colligative properties. There are several ways to quantify the amount of one compound dissolved in the other compounds collectively called concentration. Examples include molarity, molality, and parts per million (ppm).
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Examples of solid solutions are alloys, certain minerals and polymers containing plasticizers. The ability of one compound to dissolve in another compound is called solubility. The physical properties of compounds such as melting point and boiling point change when other compounds are added. Together they are called colligative properties. There are several ways to quantify the amount of one compound dissolved in the other compounds collectively called concentration. Examples include molarity, molality, and parts per million (ppm).
Solutions should be distinguished from non-homogeneous mixtures such as colloids and suspensions.
Types of solutions
Many types of solutions exist, as solids, liquids and gases can be both solvent and solute, in any combination:
| Examples of solutions | Solute | Gas | Liquid | Solid | Solvent | Gas | Oxygen and other gases in nitrogen (air) | Water vapor in air | Naphthalene slowly sublimes in air, going into solution. | Liquid | Carbon dioxide in water (carbonated water; the visible bubbles, however, are not the dissolved gas, but only an effervescence; the dissolved gas itself is not visible in the solution) | Ethanol (common alcohol) in water; various hydrocarbons in each other (petroleum) | Sucrose (table sugar) in water; sodium chloride (table salt) in water; gold in mercury, forming an amalgam | Solid | Hydrogen dissolves rather well in metals; platinum has been studied as a storage medium. | Hexane in paraffin wax, mercury in gold. | Steel, duralumin, other metal alloys |
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Solvation
During solvation, especially when the solvent is polar, a structure forms around it, which allows the solute-solvent interaction to remain stable.
When no more of a solute can be dissolved into a solvent, the solution is said to be 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 solubility that decrease with increased temperature. Such behavior is a result of an exothermic enthalpy of solution. Some surfactants exhibit this behaviour. The solubility of liquids in liquids is generally less temperature-sensitive than that of solids or gases.
























