sodium phosphate
{{Short description|Sodium salts of phosphoric acid}}
{{about||the chemical known as sodium phosphate|Trisodium phosphate}}
File:monosodium phosphate.png]]
File:disodium hydrogen phosphate.png]]
File:trisodium phosphate.png]]
A sodium phosphate is a generic variety of salts of sodium ({{chem2|Na+}}) and phosphate ({{chem2|PO4(3−)}}). Phosphate also forms families or condensed anions including di-, tri-, tetra-, and polyphosphates. Most of these salts are known in both anhydrous (water-free) and hydrated forms. The hydrates are more common than the anhydrous forms.{{Ullmann|author1=Klaus Schrödter|author2=Gerhard Bettermann|author3=Thomas Staffel|author4=Friedrich Wahl|author5=Thomas Klein|author6=Thomas Hofmann|title=Phosphoric Acid and Phosphates|doi=10.1002/14356007.a19_465.pub3|year=2012}}
Uses
Sodium phosphates have many applications in food and for water treatment. For example, sodium phosphates are often used as emulsifiers (as in processed cheese),{{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}} thickening agents, and leavening agents for baked goods. They are also used to control pH of processed foods.{{cite journal | last1 = Lampila | first1 = Lucina E. | year = 2013 | title = Applications and functions of food-grade phosphates | journal = Annals of the New York Academy of Sciences| volume = 1301 | issue = 1| pages = 37–44 | doi = 10.1111/nyas.12230 | pmid = 24033359 | bibcode = 2013NYASA1301...37L | s2cid = 206223856 | doi-access = free}} They are also used in medicine for constipation and to prepare the bowel for medical procedures. They are also used in detergents for softening water and as an efficient anti-rust solution.
Adverse effects
Sodium phosphates are popular in commerce in part because they are inexpensive and because they are nontoxic at normal levels of consumption.{{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}} 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.{{cite journal |last1= Markawitz |first1= GB |last2= Parezelli |first2= MA |date= Aug 12, 2007 |title= Acute Phosphate Nephropathyl |journal=Kidney International |volume= 76 |issue= 10 |pages= 1027–34 |doi= 10.1038/ki.2009.308 |pmid= 19675530 |doi-access= free }} Since safe and effective replacements for phosphate purgatives are available, several medical authorities have recommended general disuse of oral phosphates.{{Cite journal |last1= Mackey |first1= AC |last2= Breen |first2= L |last3= Amand |first3= KS |last4= Evigan |first4= M |date= August 2007 |title= Sodium phosphate tablets and acute Phosphate Nephropathy |journal= The American Journal of Gastroenterology|volume=104 |issue=8 |pages=1903–1906 |doi= 10.1038/ajg.2009.342 |pmid= 19661931 |s2cid= 12551005 |url= https://zenodo.org/record/1233245}}
Monophosphates
Three families of sodium monophosphates are common, those derived from orthophosphate ({{chem2|PO4(3−)}}), hydrogen phosphate ({{chem2|HPO4(2−)}}), and dihydrogenphosphate ({{chem2|H2PO4−}}). Some of the best known salts are shown in the following table.
| class="wikitable" | ||
| name
! formula | ||
|---|---|---|
| monosodium phosphate (anhydrous) | {{chem2|NaH2PO4}} | 7558-80-7 |
| monosodium phosphate monohydrate | {{chem2|NaH2PO4*H2O}} | 10049-21-5 |
| monosodium phosphate dihydrate | {{chem2|NaH2PO4*2H2O}} | 13472-35-0 |
| disodium phosphate (anhydrous) | {{chem2|Na2HPO4}} | 7558–79–4 |
| disodium phosphate dihydrate | {{chem2|Na2HPO4*2H2O}} | 10028-24-7 |
| disodium phosphate heptahydrate | {{chem2|Na2HPO4*7H2O}} | 7782–85–6 |
| disodium phosphate octahydrate | {{chem2|Na2HPO4*8H2O}} | |
| disodium phosphate dodecahydrate | {{chem2|Na2HPO4*12H2O}} | 10039–32–4 |
| trisodium phosphate (anhydrous, hexagonal) | {{chem2|Na3PO4}} | |
| trisodium phosphate (anhydrous, cubic) | {{chem2|Na3PO4}} | 7601–54–9 |
| trisodium phosphate hemihydrate | {{chem2|Na3PO4*0.5H2O}} | |
| trisodium phosphate hexahydrate | {{chem2|Na3PO4*6H2O}} | |
| trisodium phosphate octahydrate | {{chem2|Na3PO4*8H2O}} | |
| trisodium phosphate dodecahydrate | {{chem2|Na3PO4*12H2O}} | 10101-89-0 |
Di- and polyphosphates
In addition to these phosphates, sodium forms a number of useful salts with pyrophosphates (also called diphosphates), triphosphates and high polymers. Of these salts, those of the diphosphates are particularly common commercially.
| class="wikitable" | ||
| name
! formula ! CAS Registry number | ||
|---|---|---|
| monosodium diphosphate (anhydrous) | {{chem2|NaH3P2O7}} | |
| disodium diphosphate (anhydrous) | {{chem2|Na2H2P2O7}} | 7758-16-9 |
| disodium diphosphate hexahydrate | {{chem2|Na2H2P2O7*6H2O}} | |
| trisodium diphosphate (anhydrous) | {{chem2|Na3HP2O7}} | |
| trisodium diphosphate monohydrate | {{chem2|Na3HP2O7*H2O}} | |
| trisodium diphosphate nonahydrate | {{chem2|Na3HP2O7*9H2O}} | |
| tetrasodium diphosphate (anhydrous) | {{chem2|Na4P2O7}} | 7722-88-5 |
| tetrasodium diphosphate decahydrate | {{chem2|Na4P2O7*10H2O}} | 13472-36-1 |
Beyond the diphosphates, sodium salts are known triphosphates, e.g. sodium triphosphate and tetraphosphates. The cyclic polyphosphates, called metaphosphates, include the trimer sodium trimetaphosphate and the tetramer, {{chem2|Na3P3O9}} and {{chem2|Na4P4O12}}, respectively.
Polymeric sodium phosphates are formed upon heating mixtures of {{chem2|NaH2PO4}} and {{chem2|Na2HPO4}}, which induces a condensation reaction. The specific polyphosphate generated depends on the details of the heating and annealing. One derivative is the glassy (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|[NaPO3]_{n}[NaPO3(OH)]2}} 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 {{chem2|PO3−}} units, with the chains are terminated by protonated phosphates.{{Greenwood&Earnshaw2nd|page=530}}
References
External links
- {{Cite patent
|inventor= Bell, Russel N
|pubdate= 1973
|title= Sodium Aluminum Phosphate Cheese Emulsifying Agent
|number= 3726960
|country=US
}}
- {{Cite 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}}