Dicalcium phosphate

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Dicalcium phosphate
Dicalcium phosphate.png
Names
IUPAC name
Calcium hydrogen phosphate dihydrate
Other names
Calcium monohydrogen phosphate
Phosphoric acid, calcium salt (1:1)
Identifiers
7757-93-9 YesY
7789-77-7 (dihydrate) N
ChemSpider 94606 N
Jmol 3D model Interactive image
PubChem 104805
UNII L11K75P92J YesY
  • InChI=1S/Ca.H3O4P.2H2O/c;1-5(2,3)4;;/h;(H3,1,2,3,4);2*1H2/q+2;;;/p-2 N
    Key: XAAHAAMILDNBPS-UHFFFAOYSA-L N
  • InChI=1/Ca.H3O4P.2H2O/c;1-5(2,3)4;;/h;(H3,1,2,3,4);2*1H2/q+2;;;/p-2
    Key: XAAHAAMILDNBPS-NUQVWONBAM
  • O.O.OP(=O)([O-])[O-].[Ca+2]
Properties
CaHPO4
Molar mass 136.06 g/mol (anhydrous)
172.09 (dihydrate)
Appearance white powder
Odor odorless
Density 2.929 g/cm3 (anhydrous)
2.31 g/cm3 (dihydrate)
Melting point decomposes
0.02 g/100 mL (anhydrous)
0.02 g/100 mL (dihydrate)
Structure
triclinic
Vapor pressure {{{value}}}
Related compounds
Other anions
 Calcium pyrophosphate
Other cations
 Magnesium phosphate
Monocalcium phosphate
Tricalcium phosphate
Strontium phosphate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Dicalcium phosphate is a misnomer for dibasic calcium phosphate. Its chemical formula is CaHPO4. Hence the name "dicalcium" is incorrect. The correct names of this material are dibasic calcium phosphate or calcium monohydrogen phosphate. There are three crystalline forms: a dihydrate, CaHPO4•2H2O ('DPCD'), the mineral brushite; a hemihydrate, CaHPO4•0.5H2O; and anhydrous CaHPO4 ('DCPA'), the mineral monetite. Below pH 4.8 the dihydrate and anhydrous forms of dibasic calcium phosphate are the most stable (insoluble) of the calcium phosphates. Dibasic calcium phosphate is used as a food additive, it is found in some toothpastes as a polishing agent and is a biomaterial.[1][2] In the dihydrate (brushite) form it is found in some kidney stones and in dental calculi.[3][4]


Preparation

Dibasic calcium phosphate is produced by the reaction of calcium chloride and phosphoric acid:[citation needed]

CaCl2 + H3PO4 + 2 NaOH → CaHPO4 + 2 NaCl + 2 H2O

Calcium hydroxide is also used in place of the calcium chloride and sodium hydroxide. The room temperature neutralisation of phosphoric acid with calcium hydroxide at pH 3-4 precipitates the dihydrate. At 60°C the anhydrous form is precipitated:[4]

H3PO4 + Ca(OH)2 → CaHPO4

One industrial preparation of the dihydrate involves the reaction of H3PO4 with a slurry of Ca(OH)2 below 40°C. To prevent degradation that would form hydroxyapatite, Sodium pyrophosphate or trimagnesium phosphate octahydrate are added when for example, dibasic calcium phosphate dihydrate is to be used as a polishing agent in toothpaste.[1]

Anhydrous CaHPO4 is an intermediate in the production of halophosphate phosphors that were used in fluorescent lamps. In a continuous process CaCl2 was reacted with (NH4)2HPO4 to form the dihydrate, CaHPO4•2H2O.

CaCl2 + (NH4)2HPO4 → CaHPO4•2H2O

A slurry of the dihydrate is then heated to around 65–70°C to form anhydrous CaHPO4 as a crystalline precipitate in the desired form, (typically a flat diamond shaped crystal, 7-9 μm), which was suitable for further processing.[5]

Dibasic calcium phosphate dihydrate is formed in "brushite" calcium phosphate cements (CPC's) which have medical applications. An example of the overall setting reaction in the formation of "β-TCP/MCPM" (β-tricalcium phosphate/monocalcium phosphate) calcium phosphate cements is:[6]

Ca3(PO4)2 + Ca(H2PO4)2•H2O + 7 H2O → 4 CaHPO4•2H2O

Uses

Dibasic calcium phosphate is mainly used as a dietary supplement in prepared breakfast cereals, dog treats, enriched flour, and noodle products. It is also used as a tableting agent in some pharmaceutical preparations, including some products meant to eliminate body odor. Dibasic calcium phosphate is also found in some dietary calcium supplements (e.g. Bonexcin). It is used in poultry feed. It is also used in some toothpastes as a tartar control agent.[7]

References

  1. ↑ 1.0 1.1 Lua error in package.lua at line 80: module 'strict' not found. – via ScienceDirect (Subscription may be required or content may be available in libraries.)
  2. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  3. ↑ Lua error in package.lua at line 80: module 'strict' not found.  – via ScienceDirect (Subscription may be required or content may be available in libraries.)
  4. ↑ 4.0 4.1 Lua error in package.lua at line 80: module 'strict' not found.  – via ScienceDirect (Subscription may be required or content may be available in libraries.)
  5. ↑ Lua error in package.lua at line 80: module 'strict' not found. – via ScienceDirect (Subscription may be required or content may be available in libraries.)
  6. ↑ Lua error in package.lua at line 80: module 'strict' not found.  – via ScienceDirect (Subscription may be required or content may be available in libraries.)
  7. ↑ 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

See also

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