IdeaWazaWiki - User contributions [en]

Precipitation (chemistry)

2005-12-05T02:20:14Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the formation of a [[solid]] in a [[solution]] during a [[chemical reaction]]. This can occur when an insoluble substance is formed in the solution due to a reaction or when the solution has been [[supersaturated]] by a compound. 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]]).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:18:44Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the formation of a [[solid]] in a [[solution]] during a [[chemical reaction]]. This can occur when an insoluble substance is formed in the solution due to a reaction or when the solution has been [[supersaturated]] by a compound or compounds. 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]]).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:18:09Z

134.82.76.105:

Precipitation (chemistry)

2005-12-05T02:17:39Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the formation of a [[solid]] in a [[solution]] during a [[chemical reaction]]. This can occur when an insoluble substance is formed in the solution due to a reaction or when the solution has been [[supersaturated]] by a compound. 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 possibly precipitate in [[suspension (chemistry)|suspension]]).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:17:09Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the formation of a [[solid]] in a [[solution]] during a [[chemical reaction]]. This can occur when an insoluble substance is formed in the solution due to a reaction or when the solution has been [[supersaturated]] by a compound. 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 possibly precipitate in [[suspension(chemistry)|suspension|]]).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:13:59Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the formation of a [[solid]] in a [[solution]] during a [[chemical reaction]]. This can occur when the solution is [[supersaturated]] by a given compound or when an insoluble substance is formed in the solution due to a reaction. In most situations, the solid forms 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 possibly precipitate in [[suspension|suspension(chemistry)]]).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:11:29Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This can occur when the solution is [[supersaturated]] by a given compound or when an insoluble substance is formed in the solution. In most situations, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent or precipitate in [[suspension|suspension (chemistry)]]).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:10:54Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This can occur when the solution is [[supersaturated]] by a given compound or when an insoluble substance is formed in the solution. In most situations, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent or precipitate in [[suspension|chemistry]]).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:10:03Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This can occur when the solution is [[supersaturated]] by a given compound or when an insoluble substance is formed in the solution. In most situations, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent or precipitate in [[suspension]]).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:09:05Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This can occur when the solution is [[supersaturated]] by a given compound or when an insoluble substance is formed in the solution. In most situations, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent or exist in [[suspension]]).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:01:47Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl 101)
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:01:05Z

134.82.76.105: /* Reference */

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:00:53Z

134.82.76.105: /* Reference */

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. <Chemical Principals.> 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:00:41Z

134.82.76.105: /* Reference */

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. ''Chemical Principals.'' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T02:00:26Z

134.82.76.105: /* Reference */

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. 'Chemical Principals.' 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T01:57:28Z

134.82.76.105: /* Reference */

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S. <und>Chemical Principals.</und> 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T01:56:14Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==Reference==

Zumdahl, Steven S., ed. Chemical Principals. 4th ed. New York: Houghton Mifflin Company, 2005.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T01:48:49Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T01:45:35Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction: Aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T01:44:51Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction:

When aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]

Precipitation (chemistry)

2005-12-05T01:44:11Z

134.82.76.105:

: ''"Precipitate" redirects here, for the [[Interpol (band)|Interpol]] [[Extended play|EP]] see [[Precipitate (EP)]].''

'''Precipitation''' is the condensation of a [[solid]] from a [[solution]] during a [[chemical reaction]]. This occurs when the solution is [[supersaturated]] (this includes the obvious case that an [[solubility|insoluble]] compound is present). In this situation, the solid forms from the solute phase, and usually sinks to the bottom of the solution (though it will float if less dense than the solvent).

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.

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.

An example of a precipitation reaction:
When aqueous silver nitrate (AgNO3) is added to a solution containing potassium chloride (KCl) the precipitation of a white solid, silver chloride is observed.
AgNO3(aqueous) + KCl(aqueous) ---> AgCl(solid) + KNO3(aqueous)
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+, NO3-, K+, Cl- ---> AgCl(solid), K+, NO3-

==Cation sensitivity==
Precipitate formation is useful in the detection of the type of [[cation]] in an unknown [[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]] metals.

==External links==
* http://www.hci.edu.sg/~limth/lessons/2002/qa/cations.htm
[[Category:Chemical processes]]

[[de:Fällungsreaktion]]
[[es:Precipitado]]
[[ja:%E6%B2%88%E6%AE%BF]]
[[nl:Neerslag (scheikunde)]]
[[zh:沉淀]]