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Dicalcium phosphate

 

Dicalcium phosphate

Dicalcium phosphate
Names
IUPAC name
Calcium hydrogen phosphate dihydrate
Other names
Calcium monohydrogen phosphate
Phosphoric acid, calcium salt (1:1)
Identifiers
 Y
(dihydrate) N
ChemSpider  N
Jmol-3D images Image
PubChem
UNII  Y
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
Hazards
NFPA 704
0
1
0
Flash point Non-flammable
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  (: Y/N?)

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 [1][2] In the dihydrate (brushite) form it is found in some kidney stones and in dental calculi.[3][4]


Contents

  • Preparation 1
  • Uses 2
  • References 3
  • See also 4

Preparation

Dibasic calcium phosphate is produced by the reaction of calcium chloride and phosphoric acid:

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

Calcium carbonate 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 [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. ^ a b Corbridge, D. (1995). "Chapter 3: Phosphates". Studies in inorganic Chemistry vol. 20. Elsevier Science B.V. pp. 169–305.   – via ScienceDirect (Subscription may be required or content may be available in libraries.)
  2. ^ Salinas, Antonio J.; Vallet-Regi, Maria (2013). "Bioactive ceramics: from bone grafts to tissue engineering". RSC Advances ( 
  3. ^ Pak, Charles Y.C, Poindexter, John R, Adams-Huet, Beverley, Pearle, Margaret S (July 2003). "Predictive value of kidney stone composition in the detection of metabolic abnormalities". The American Journal of Medicine 115 (1): 26– 2.    – via ScienceDirect (Subscription may be required or content may be available in libraries.)
  4. ^ a b Rey, C.; Combes, C.; Drouet, C.; Grossin, D. (2011). "1.111 - Bioactive Ceramics: Physical Chemistry". In Ducheyne, Paul. Comprehensive Biomaterials 1. Elsevier. pp. 187–281.    – via ScienceDirect (Subscription may be required or content may be available in libraries.)
  5. ^ Ropp, R.C. (2013). "Chapter 4 - Group 15 (N, P, As, Sb and Bi) Alkaline Earth Compounds". Encyclopedia of the Alkaline Earth Compounds 1. Elsevier.   – via ScienceDirect (Subscription may be required or content may be available in libraries.)
  6. ^ Tamimi, Faleh; Sheikh, Zeeshan; Barralet, Jake (February 2012). "Dicalcium phosphate cements: Brushite and monetite". Acta Biomaterialia 8 (2): 474–484.    – 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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