View source for Precipitation (chemistry)

'''Precipitation''' is the formation of a [[solid]] in a [[solution]] during a [[chemical reaction]].   When the chemical reaction occurs the solid formed is called the '''precipitate'''. This can occur when an insoluble substance, the '''precipitate''', is formed in the solution due to a reaction or when the solution has been ''supersaturated'' by a compound. The formation of a precipitate is a sign of a chemical change. In most situations, the solid forms ("falls") out of the solute phase, and sinks to the bottom of the solution (though it will float if it is less dense than the solvent, or form a [[suspension (chemistry)|suspension]]).

==Uses==

Precipitation reactions can be used for making pigments, removing salts from water in water treatment, and for qualitative chemical analysis.

This effect is useful in many industrial and scientific applications whereby a chemical reaction may produce a solid that can be collected from the solution by various methods (e.g. filtration, decanting, centrifuging).  Precipitation from a [[solid solution]] is also a useful way to [[precipitation strengthening|strengthen]] [[alloy]]s; this process is known as [[solid solution strengthening]].

==Mechanism==

An important stage of the precipitation process is the onset of [[nucleation]].  The creation of a hypothetical solid particle includes the formation of an interface, which requires some energy based on the relative [[surface energy]] of the solid and the solution.  If this energy is not available, and no suitable nucleation surface is available, [[supersaturation]] occurs.

==Representation using chemical equations==

An example of a precipitation reaction: Aqueous silver nitrate (AgNO<sub>3</sub>) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl, 2005)

:AgNO<sub>3</sub>(aq) + KCl(aq) → AgCl(s) + KNO<sub>3</sub>(aq)
     
The silver chloride(AgCl) has formed a solid, which is observed as a precipitate.

This reaction can be written emphasizing the dissociated ions in a combined solution
:Ag<sup>+</sup>(aq) + NO<sub>3</sub><sup>-</sup>(aq) + K<sup>+</sup>(aq) + Cl<sup>-</sup>(aq) → AgCl(solid) + K<sup>+</sup>(aq) + NO<sub>3</sub><sup>-</sup>(aq)

A final way to represent a precipitate reaction is known as a ''net ionic reaction''. In this case, any spectator ions (those which do not contribute to the reaction) are left out of the formula completely. This simplifies the above equations to the following:
:Ag<sup>+</sup>(aq) + Cl<sup>-</sup>(aq) → AgCl(s)


==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in [[salt]]. To do this, an [[alkali]] first reacts with the unknown salt to produce a precipitate which is the hydroxide of the unknown salt. 

To identify the cation, the colour of the precipitate and its solubility in excess are noted.

Similar processes are often used to separate chemically similar elements, such as the [[Rare earth element|rare earth]] metals.

==Digestion==

Digestion, or ''precipitate ageing'', happens when a freshly-formed precipitate is left, usually at a higher temperature, in the solution from which it is precipitated. It results in cleaner and bigger particles.<ref>[http://www.ktf-split.hr/glossary/en_o.php?def=digestion Chemical dictionary definition.]</ref>

==References==
*Zumdahl, Steven S. ''Chemical Principles.'' 4<sup>th</sup> ed. New York: Houghton Mifflin Company, 2005.
*Mark Smith ''Principles of Science'' 1993

<references/>

==Further reading==
*Banert, T., Brenner, G., Peuker, U. A. (2006), Operating parameters of a continuous sono-chemical precipitation reactor, Proc. 5. WCPT, Orlando Fl., 23.-27. April 2006.

==External links==
* [http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm Test for Cations]
* [http://www.hielscher.com/ultrasonics/precipitation_01.htm Continuous Precipitation Using Ultrasonication (e.g. for nano-size magnetite particles)]

[[Category:Chemical processes]]

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