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{{Short description|Sodium salts of phosphoric acid}}
[[File:monosodium phosphate.png|thumb|right|100px|[[Sodium dihydrogen phosphate]]]]▼
[[File:disodium{{about||the hydrogenchemical known as sodium phosphate.png|thumb|100px|right|[[Sodium hydrogenTrisodium phosphate]]]]}}
[[File:trisodiummonosodium phosphate.png|thumb|right|100px150px|[[TrisodiumSodium dihydrogen phosphate]]]]
[[File:disodium hydrogen phosphate.png|thumb|150px|right|[[Sodium hydrogen phosphate]]]]
▲[[File:monosodiumtrisodium phosphate.png|thumb|right|100px150px|[[Sodium dihydrogenTrisodium phosphate]]]]
 
A '''Sodiumsodium phosphate''' is a generic term for a variety of [[salt (chemistry)|salt]]s of [[sodium]] ({{chem2|Na<sup>+</sup>}}) and [[phosphate]] (PO<sub>4</sub><sup>{{chem2|PO4(3−</sup>)}}). Phosphate also forms families or condensed anions[[anion]]s including di-, tri-, tetra-, and polyphosphates[[polyphosphate]]s. Most of these salts are known in both [[anhydrous]] (water-free) and [[hydrated]] forms. The hydrates are more common than the anhydrous forms.<ref name=Ullmann>{{Ullmann|author1=Klaus Schrödter, |author2=Gerhard Bettermann, |author3=Thomas Staffel, |author4=Friedrich Wahl, |author5=Thomas Klein, |author6=Thomas Hofmann "|title=Phosphoric Acid and Phosphates" in ''Ullmann's Encyclopedia of Industrial Chemistry'' 2008, Wiley-VCH, Weinheim. {{|doi|=10.1002/14356007.a19_465.pub3|year=2012}}</ref>
 
==Uses==
Sodium phosphates have many applications in food and for water treatment. For example, sodium phosphates are often used as [[emulsifier]]s (such as in [[processed cheese]]),<ref>{{cite web |url=http://www.sodiumphosphateformula.com/tag/monosodium-phosphate |url-status=dead |archive-url=https://web.archive.org/web/20150402120338/http://www.sodiumphosphateformula.com/tag/monosodium-phosphate |archive-date=2015-04-02 |title=Monosodium Phosphate {{!}} Sodium Phosphate Formula}}</ref> [[thickening agent]]s, and [[leavening agent]]s for baked goods. They are also used to control pH of processed foods.<ref>{{cite journal | last1 = Lampila | first1 = Lucina E. Lampila| year = 2013 | title = "Applications and functions of food-grade phosphates" | journal = Ann. N.Y. Acad. Sci. 2013,| vol.volume = 1301, pp.| issue = 1| pages = 37–44. {{doi| doi = 10.1111/nyas.12230 | pmid = 24033359 | bibcode = 2013NYASA1301...37L | s2cid = 206223856 | doi-access = free}}</ref> They are also used in medicine for [[constipation]] and to prepare the bowel for medical procedures. Moreover, theyThey are also used in detergents for softening water, and as an efficient anti -[[rust]] solution.
 
==Adverse effects==
OralSodium phosphates are popular in commerce in part because they are inexpensive and because they are nontoxic at normal levels of consumption.<ref>{{cite journal | pmc = 3120105| year = 2011| last1 = Razzaque| first1 = M. S.| title = Phosphate toxicity: New insights into an old problem| journal = Clinical Science| volume = 120| issue = 3| pages = 91–97| doi = 10.1042/CS20100377| pmid=20958267}}</ref> However, oral sodium phosphates when taken at high doses for [[bowel preparation]] for [[colonoscopy]] may in some individuals carry a risk of kidney injury under the form of [[phosphate nephropathy]]. There are several oral phosphate formulations which are prepared extemporaneously. Oral phosphate prep drugs have been withdrawn in the United States, although evidence of causality is equivocal.<ref>▼
Sodium phosphates are popular in commerce in part because they are inexpensive and nontoxic.
 
▲Oral sodium phosphates when taken at high doses for [[bowel preparation]] for [[colonoscopy]] may in some individuals carry a risk of kidney injury under the form of [[phosphate nephropathy]]. There are several oral phosphate formulations which are prepared extemporaneously. Oral phosphate prep drugs have been withdrawn in the United States, although evidence of causality is equivocal.<ref>
{{Citation
|last1= Markawitz
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|first2= MA
|date= Aug 12, 2007
|title= Acute Phosphate NephropathyNephropathyl
|periodical= Kidney Int.
|volume= 76
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|doi= 10.1038/ki.2009.308
|pmid= 19675530
|doi-access= free
}}
</ref> Since safe and effective replacements for phosphate purgatives are available, several medical authorities have recommended general disuse of oral phosphates.<ref>
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|doi= 10.1038/ajg.2009.342
|pmid= 19661931
|s2cid= 12551005
|url= https://zenodo.org/record/1233245
}}
</ref>
 
==Monophosphates==
Three families of sodium monophosphates are common, those derived from orthophosphate (PO<sub>4</sub><sup>{{chem2|PO4(3−</sup>)}}), hydrogen phosphate (HPO<sub>4</sub><sup>{{chem2|HPO4(2−</sup>)}}), and dihydrogenphosphate (H<sub>2</sub>PO<sub>4</sub><sup>−</sup>{{chem2|H2PO4−}}). Some of the most wellbest known salts are shown in the following table.
 
{|class="wikitable"
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! [[CAS registry number]]
|-
| [[monosodium phosphate]] (anhydrous) || NaH<sub>2</sub>PO<sub>4</sub>{{chem2|NaH2PO4}}||7558-80-7
|-
| monosodium phosphate (monohydrate) || NaH<sub>2</sub>PO<sub>4</sub>(H<sub>2</sub>O){{chem2|NaH2PO4*H2O}}||10049-21-5
|-
| monosodium phosphate (dihydrate) || NaH<sub>2</sub>PO<sub>4</sub>(H<sub>2</sub>O)<sub>2</sub>{{chem2|NaH2PO4*2H2O}}||13472-35-0
|-
| [[disodium phosphate]] (anhydrous) || Na<sub>2</sub>HPO<sub>4</sub>{{chem2|Na2HPO4}} || 7558-79-47558–79–4
|-
| disodium phosphate (dihydrate) || HNa<sub>2</sub>PO<sub>4</sub>(H<sub>2</sub>O)<sub>2</sub>{{chem2|Na2HPO4*2H2O}}||10028-24-7
|-
| disodium phosphate (heptahydrate) || HNa<sub>2</sub>PO<sub>4</sub>(H<sub>2</sub>O)<sub>7</sub>{{chem2|Na2HPO4*7H2O}} || 7782-85-67782–85–6
|-
| disodium phosphate (octahydrate) || HNa<sub>2</sub>PO<sub>4</sub>(H<sub>2</sub>O)<sub>8</sub>{{chem2|Na2HPO4*8H2O}}||
|-
| disodium phosphate (dodecahydrate) || HNa<sub>2</sub>PO<sub>4</sub>(H<sub>2</sub>O)<sub>12</sub>{{chem2|Na2HPO4*12H2O}} || 10039-32-410039–32–4
|-
| [[trisodium phosphate]] (anhydrous, hexagonal) || Na<sub>3</sub>PO<sub>4</sub>{{chem2|Na3PO4}}||
|-
| trisodium phosphate (anhydrous, cubic) || Na<sub>3</sub>PO<sub>4</sub>{{chem2|Na3PO4}} || 7601-54-97601–54–9
|-
| trisodium phosphate (hemihydrate) || Na<sub>3</sub>PO<sub>4</sub>(H<sub>2</sub>O)<sub>{{chem2|Na3PO4*0.5</sub>5H2O}}||
|-
| trisodium phosphate (hexahydrate) || Na<sub>3</sub>PO<sub>4</sub>(H<sub>2</sub>O)<sub>6</sub>{{chem2|Na3PO4*6H2O}} ||
|-
| trisodium phosphate (octahydrate) || Na<sub>3</sub>PO<sub>4</sub>(H<sub>2</sub>O)<sub>8</sub>{{chem2|Na3PO4*8H2O}}||
|-
| trisodium phosphate (dodecahydrate) || Na<sub>3</sub>PO<sub>4</sub>(H<sub>2</sub>O)<sub>12</sub>{{chem2|Na3PO4*12H2O}}||10101-89-0
|-
|}
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! CAS Registry number
|-
| [[monosodium diphosphate]] (anhydrous) || NaH<sub>3</sub>P<sub>2</sub>O<sub>7</sub>{{chem2|NaH3P2O7}}||
|-
| [[disodium diphosphate]] (anhydrous) || Na<sub>2</sub>H<sub>2</sub>P<sub>2</sub>O<sub>7</sub>{{chem2|Na2H2P2O7}}||7758-16-9
|-
| disodium diphosphate (hexahydrate) || Na<sub>2</sub>H<sub>2</sub>P<sub>2</sub>O<sub>7</sub>(H<sub>2</sub>O)<sub>6</sub>{{chem2|Na2H2P2O7*6H2O}}||
|-
| [[trisodium diphosphate]] (anhydrous) || Na<sub>3</sub>HP<sub>2</sub>O<sub>7</sub>{{chem2|Na3HP2O7}}||
|-
| trisodium diphosphate (monohydrate) || Na<sub>3</sub>HP<sub>2</sub>O<sub>7</sub>(H<sub>2</sub>O){{chem2|Na3HP2O7*H2O}}||
|-
| trisodium diphosphate (nonahydrate) || Na<sub>3</sub>HP<sub>2</sub>O<sub>7</sub>(H<sub>2</sub>O)<sub>9</sub>{{chem2|Na3HP2O7*9H2O}}||
|-
| [[tetrasodium diphosphate]] (anhydrous) || Na<sub>4</sub>P<sub>2</sub>O<sub>7</sub>{{chem2|Na4P2O7}}||7722-88-5
|-
| tetrasodium diphosphate (decahydrate) || Na<sub>4</sub>P<sub>2</sub>O<sub>7</sub>(H<sub>2</sub>O)<sub>10</sub>{{chem2|Na4P2O7*10H2O}}||13472-36-1
|-
|}
 
Beyond the diphosphates, sodium salts are known triphosphates, e.g. [[sodium triphosphate]] and tetraphospatestetraphosphates. The cyclic polyphosphates, called metaphosphates, include the trimer [[sodium trimetaphosphate]] and the tetramer, Na<sub>3</sub>P<sub>3</sub>O<sub>9</sub>{{chem2|Na3P3O9}} and Na<sub>4</sub>P<sub>4</sub>O<sub>12</sub>{{chem2|Na4P4O12}}, respectively.
 
Polymeric sodium phosphates are formed upon heating mixtures of NaH<sub>2</sub>PO<sub>4</sub>{{chem2|NaH2PO4}} and Na<sub>2</sub>HPO<sub>4</sub>{{chem2|Na2HPO4}}, which induces a [[condensation reaction]]. The specific polyphosphate generated depends on the details of the heating and anneallingannealing. One derivative is the [[glass]]y (i.e., amorphous) [['''Graham's salt''' ([[sodium hexametaphosphate]]). It is a cyclic polyphosphate with the formula {{chem2|Na6[(PO3)6]}}. Crystalline high molecular weight polyphosphates include '''Kurrol's salt''' and '''Maddrell's salt''' (CAS#10361-03-2). These species have the formula {{chem2|[NaPO<sub>3</sub>NaPO3]<sub>_{''n</sub>''}[NaPO<sub>3</sub>NaPO3(OH)]<sub>2</sub>}} where ''n'' can be as great as 2000, and it is a white powder practically insoluble in water. In terms of their structures, these polymers consist of PO<sub>3</sub><sup>−</sup>{{chem2|PO3−}} "monomers"units, with the chains are terminated by protonated phosphates.<ref name=Ullmann/><ref name=G&E>{{Greenwood&Earnshaw2nd|page=530}}</ref>
 
==References==
<references />
 
==External links==
* {{Cite patent
*{{Citation
|last1inventor= Bell, Russel N
|pubdate= 1973
|first1= Russel N
|date= April 1973
|title= Sodium Aluminum Phosphate Cheese Emulsifying Agent
|periodicalnumber= US Patent 3726960
|country=US
}}
* {{CitationCite journal |last1= Lien |first1= YH |title= Is bowel preparation before colonoscopy a risky business for the kidney? |volume= 4 |issue= 11 |pages= 606–14 |date= 16 July 2008 |journal= Nature Clinical Practice Nephrology |doi= 10.1038/ncpneph0939 |pmid= 18797448|s2cid= 340122}}
 
{{Sodium compounds}}
{{Phosphates}}
 
[[Category:Phosphates]]
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