Sodium phosphates
Sodium phosphate is a generic term for a variety of salts of sodium (Na+) and phosphate (PO43−). 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.[1]
Contents
Uses
Sodium phosphates have many applications in food and for water treatment. For example, sodium phosphates are often used as emulsifiers,[2] thickening agents, and leavening agents for baked goods. They are also used to control pH of processed foods.[3] 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.
Adverse effects
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 Oral phosphate prep drugs have been withdrawn in the United States, although evidence of causality is equivocal.[4] Since safe and effective replacements for phosphate purgatives are available, several medical authorities have recommended general disuse of oral phosphates.[5]
Monophosphates
Three families of sodium monophosphates are common, those derived from orthophosphate (PO43−), hydrogen phosphate (HPO42−), and dihydrogenphosphate (H2PO4−). Some of the most well known salt are shown in the table.
| 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 |
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.
| name | formula | CAS Registry number |
|---|---|---|
| monosodium diphosphate (anhydrous) | NaH3P2O7 | |
| disodium diphosphate (anhydrous) | Na2H2P2O7 | 7758-16-9 |
| disodium diphosphate (hexahydrate) | Na2H2P2O7(H2O)6 | |
| trisodium diphosphate (anhydrous) | Na3HP2O7 | |
| trisodium diphosphate (monohydrate) | Na3HP2O7(H2O) | |
| trisodium diphosphate (nonahydrate) | Na3HP2O7(H2O)9 | |
| tetrasodium diphosphate (anhydrous) | Na4P2O7 | 7722-88-5 |
| tetrasodium diphosphate (decahydrate) | Na4P2O7(H2O)10 | 13472-36-1 |
Beyond the diphosphates, sodium salts are known triphosphates, e.g. sodium triphosphate and tetraphospates. The cyclic polyphosphates, called metaphosphates, include the trimer sodium trimetaphosphate and the tetramer, Na3P3O9 and Na4P4O12, respectively.
Polymeric sodium phosphates are formed upon heating mixtures of NaH2PO4 and Na2HPO4, which induces condensation. The specific polyphosphate generated depends on the details of the heating and annealling. One derivative is the glassy (i.e., amorphous) Graham’s salt. Crystalline high molecular weight polyphosphates include Kurrol’s salt and Maddrell’s salt (CAS#10361-03-2). These species have the formula [NaPO3]n[NaPO3(OH)]2 where n can be as great as 2000. In terms of their structures, these polymers consist of PO3− "monomers", with the chains are terminated by protonated phosphates.[1]
References
- ↑ 1.0 1.1 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
- ↑ http://www.sodiumphosphateformula.com/tag/monosodium-phosphate
- ↑ 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
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External links
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