Changes

==Etymology==

==Etymology==

[[Latin]] saturatus, past participle of saturare,  from satur well-fed

[[Latin]] saturatus, past participle of saturare,  from satur well-fed

*Date: [http://www.wikipedia.org/wiki/16th_Century 1538]

*Date: [https://www.wikipedia.org/wiki/16th_Century 1538]

==Definitions==

==Definitions==

*1 : to [[satisfy]] fully : satiate

*1 : to [[satisfy]] fully : satiate

*4 : to [[cause]] to combine until there is no further tendency to combine

*4 : to [[cause]] to combine until there is no further tendency to combine

==Description==

==Description==

In physical [[chemistry]], '''saturation''' is the point at which a [http://en.wikipedia.org/wiki/Solution solution] of a substance can dissolve no more of that substance and additional amounts of it will [[appear]] as a [http://en.wikipedia.org/wiki/Precipitation_(chemistry) precipitate]. This point of maximum [[concentration]], the ''saturation point'', depends on the [[temperature]] of the [[liquid]] as well as the [[chemical]] [[nature]] of the substances involved. This can be used in the [[process]] of recrystallisation to [[purify]] a [[chemical]]: it is dissolved to the point of saturation in hot solvent, then as the solvent cools and the solubility decreases, excess solute precipitates. Impurities, being present in much lower [[concentration]], do not saturate the solvent and so remain dissolved in the [[liquid]]. If a [[change]] in conditions (e.g. cooling) means that the [[concentration]] is actually higher than the ''saturation point'', the solution has become [http://en.wikipedia.org/wiki/Supersaturated supersaturated].

In physical [[chemistry]], '''saturation''' is the point at which a [https://en.wikipedia.org/wiki/Solution solution] of a substance can dissolve no more of that substance and additional amounts of it will [[appear]] as a [https://en.wikipedia.org/wiki/Precipitation_(chemistry) precipitate]. This point of maximum [[concentration]], the ''saturation point'', depends on the [[temperature]] of the [[liquid]] as well as the [[chemical]] [[nature]] of the substances involved. This can be used in the [[process]] of recrystallisation to [[purify]] a [[chemical]]: it is dissolved to the point of saturation in hot solvent, then as the solvent cools and the solubility decreases, excess solute precipitates. Impurities, being present in much lower [[concentration]], do not saturate the solvent and so remain dissolved in the [[liquid]]. If a [[change]] in conditions (e.g. cooling) means that the [[concentration]] is actually higher than the ''saturation point'', the solution has become [https://en.wikipedia.org/wiki/Supersaturated supersaturated].

[[Category: Chemistry]]

[[Category: Chemistry]]