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Revision as of 05:00, 5 January 2014 editSmokefoot (talk | contribs)Autopatrolled, Extended confirmed users, Pending changes reviewers, Rollbackers74,246 edits expand table to include CAS← Previous edit Revision as of 14:38, 5 January 2014 edit undoSmokefoot (talk | contribs)Autopatrolled, Extended confirmed users, Pending changes reviewers, Rollbackers74,246 edits Kurrol’s salt, Graham’s salt, Maddrell’s salt Sodium trimetaphosphateNext edit →
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Beyond the mono and diphosphates, sodium forms triphosphates, e.g. ]. Polymeric sodium phosphates are also well known, these include Kurrol’s salt, Graham’s salt, and Maddrell’s salt. Cyclic phosphates are called metaphosphates, they include the trimer and the tetramer Na<sub>3</sub>P<sub>3</sub>O<sub>9</sub> and Na<sub>4</sub>P<sub>4</sub>O<sub>12</sub>. <ref name=Ullmann/> Beyond the mono and diphosphates, sodium forms triphosphates, e.g. ]. Polymeric sodium phosphates are also well known, these include Kurrol’s salt, Graham’s salt, and Maddrell’s salt. These species have the formula <sub>n</sub> where n can be as great as 2000. Of the same empirical formula as the polyphosphates are the cyclic phosphates are called metaphosphates, they include the trimer ] and the tetramer, Na<sub>3</sub>P<sub>3</sub>O<sub>9</sub> and Na<sub>4</sub>P<sub>4</sub>O<sub>12</sub>, respectively.<ref name=Ullmann/>


==Applications== ==Applications==

Revision as of 14:38, 5 January 2014

Sodium Dihydrogen Phosphate
Sodium Hydrogen Phosphate
Sodium Phosphate

Sodium phosphate is a generic term for a variety of salts of Na and phosphate (PO4), hydrogen phosphate (HPO4), and dihydrogenphosphate (H2PO4). Known compounds are shown in the table. Usually the hydrated salts are more common than the anhydrous forms.

name formula CAS registry number
monosodium phosphate (anhydrous) NaH2PO4 7558-80-7
monosodium phosphate (monohydrate) NaH2PO4(H2O)
monosodium phosphate (dihydrate) NaH2PO4(H2O)2
disodium phosphate (anhydrous) Na2HPO4 7558-79-4
disodium phosphate (dihydrate) HNa2PO4(H2O)2 10028-24-7
disodium phosphate (heptahydrate) HNa2PO4(H2O)7 7782-85-6
disodium phosphate (octahydrate) HNa2PO4(H2O)8
disodium phosphate (dodecahydrate) HNa2PO4(H2O)12 10039-32-4
trisodium phosphate (anhydrous, hexagonal) Na3PO4
trisodium phosphate (anhydrous, cubic) Na3PO4 7601-54-9
trisodium phosphate (hemihydrate) Na3PO4(H2O)0.5
trisodium phosphate (hexahydrate) Na3PO4(H2O)6
trisodium phosphate (octahydrate) Na3PO4(H2O)8
trisodium phosphate (dodecahydrate) Na3PO4(H2O)12 10101-89-0

In addition to these phosphates, sodium forms a number of useful salts with pyrophosphates (called diphosphates):

name formula
monosodium diphosphate (anhydrous) NaH3P2O7
disodium diphosphate (anhydrous) Na2H2P2O7
disodium diphosphate (hexahydrate) Na2H2P2O7(H2O)6
trisodium diphosphate (anhydrous) Na3HP2O7
trisodium diphosphate (hydrate) Na3HP2O7(H2O)
trisodium diphosphate nonahydrate Na3HP2O7(H2O)9
tetrasodium phosphate (anhydrous) Na4P2O7
tetrasodium diphosphate (decahydrate) Na4P2O7(H2O)10

Beyond the mono and diphosphates, sodium forms triphosphates, e.g. sodium triphosphate. Polymeric sodium phosphates are also well known, these include Kurrol’s salt, Graham’s salt, and Maddrell’s salt. These species have the formula n where n can be as great as 2000. Of the same empirical formula as the polyphosphates are the cyclic phosphates are called metaphosphates, they include the trimer sodium trimetaphosphate and the tetramer, Na3P3O9 and Na4P4O12, respectively.

Applications

Sodium phosphates have many applications in the food industry and for water treatment. For example, sodium phosphates are often used as leavening agents for baked goods. They are used to control pH of processed foods.

Safety

Sodium phosphates are popular in commerce in part because they are inexpensive and nontoxic.

Oral sodium phosphates 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. Since safe and effective replacements for phosphate purgatives are available, several medical authorities have recommended general disuse of oral phosphates.

References

  1. ^ Klaus Schrödter, Gerhard Bettermann, Thomas Staffel, Friedrich Wahl, Thomas Klein, Thomas Hofmann "Phosphoric Acid and Phosphates" in Ullmann’s Encyclopedia of Industrial Chemistry 2008, Wiley-VCH, Weinheim. doi:10.1002/14356007.a19_465.pub3
  2. Lucina E. Lampila "Applications and functions of food-grade phosphates" Ann. N.Y. Acad. Sci. 2013, vol. 1301, pp. 37–44. doi:10.1111/nyas.12230
  3. Markowitz, GS; Perazella, MA (Aug 12), "Acute Phosphate Nephropathy", Kidney Int., vol. 76, no. 10, pp. 1027–34, doi:10.1038/ki.2009.308, PMID 19675530 {{citation}}: Check date values in: |date= and |year= / |date= mismatch (help)
  4. Mackey, AC; Green, L; Amand, KS; Avigan, M (2009), "Sodium phosphate tablets and acute Phosphate Nephropathy", Am J Gastroenterol, vol. 104, no. 8 (published Aug), pp. 1903–6, doi:10.1038/ajg.2009.342, PMID 19661931 {{citation}}: Check date values in: |publication-date= (help)

External links

  • Bell, Russel N (1973), "SODIUM ALUMINUM PHOSPHATE CHEESE EMULSIFYING AGENT", US Patent 3726960 (published April) {{citation}}: Check date values in: |publication-date= (help)
  • Lien, YH (2008), "Is bowel preparation before colonoscopy a risky business for the kidney?", Nature Clinical Practice Nephrology, 4 (11): 606–14, doi:10.1038/ncpneph0939, PMID 18797448.
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