Dicalcium phosphate

Dicalcium phosphate
Names


IUPAC name calcium hydrogen phosphate
Other names calcium hydrogen phosphate, phosphoric acid calcium salt (1:1)
Identifiers
CAS Number	7757-93-9^Y 7789-77-7 (dihydrate)^Y
3D model (JSmol)	Interactive image
ChemSpider	94606^N
ECHA InfoCard	100.028.933
E number	E341(ii) (antioxidants, ...)
PubChem CID	104805
UNII	L11K75P92J^Y O7TSZ97GEP (dihydrate)^Y
CompTox Dashboard (EPA)	DTXSID90872536
InChI InChI=1S/Ca.H3O4P.2H2O/c;1-5(2,3)4;;/h;(H3,1,2,3,4);21H2/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);21H2/q+2;;;/p-2 Key: XAAHAAMILDNBPS-NUQVWONBAM
SMILES O.O.OP(=O)([O-])[O-].[Ca+2]
Properties
Chemical formula	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
Solubility in water	0.02 g/100 mL (anhydrous) 0.02 g/100 mL (dihydrate)
Structure
Crystal structure	triclinic
Hazards
NFPA 704 (fire diamond)	1 0 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 verify (what is ^YN ?) Infobox references

Chemical compound

Dicalcium phosphate is the calcium phosphate with the formula CaHPO₄ and its dihydrate. The "di" prefix in the common name arises because the formation of the HPO₄^2– anion involves the removal of two protons from phosphoric acid, H₃PO₄. It is also known as dibasic calcium phosphate or calcium monohydrogen phosphate. Dicalcium phosphate is used as a food additive, it is found in some toothpastes as a polishing agent and is a biomaterial.^[1]^[2]

Preparation

Dibasic calcium phosphate is produced by the neutralization of calcium hydroxide with phosphoric acid, which precipitates the dihydrate as a solid. At 60 °C the anhydrous form is precipitated:^[3]

H₃PO₄ + Ca(OH)₂ → CaHPO₄ +2H₂O

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]

In a continuous process CaCl₂ can be treated with (NH₄)₂HPO₄ to form the dihydrate:

CaCl₂ + (NH₄)₂HPO₄ → CaHPO₄•2H₂O + 2NH₄Cl

A slurry of the dihydrate is then heated to around 65–70 °C to form anhydrous CaHPO₄ as a crystalline precipitate, typically as flat diamondoid crystals, which are suitable for further processing.^{[citation needed]}

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:^[4]

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

Portion of the lattice of dicalcium phosphate dihydrate, highlighting the 8-coordinated Ca²⁺ center and the location the protons on three ligands (green = calcium, red = oxygen, orange = phosphorus, white = hydrogen)

Structure

Three forms of dicalcium phosphate are known:

dihydrate, CaHPO₄•2H₂O ('DCPD'), the mineral brushite
monohydrate, CaHPO₄•H₂O ('DCPM')
anhydrous CaHPO₄, ('DCPA'), the mineral monetite. Below pH 4.8 the dihydrate and anhydrous forms of dicalcium phosphate are the most stable (insoluble) of the calcium phosphates.

The structure of the anhydrous and dihydrated forms have been determined by X-ray crystallography and the structure of the monohydrate was determined by electron crystallography. The dihydrate^[5] (shown in table above) as well as the monohydrate^[6] adopt layered structures.

Uses and occurrence

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]

Heating dicalcium phosphate gives dicalcium diphosphate, a useful polishing agent:

2 CaHPO₄ → Ca₂P₂O₇ + H₂O

In the dihydrate (brushite) form it is found in some kidney stones and in dental calculi.^[8]^[3]

References

^ ^a ^b Corbridge, D. E. C. (1995). "Phosphates". Phosphorus - an Outline of its Chemistry, Biochemistry and Uses. Studies in Inorganic Chemistry. Vol. 20. pp. 169–305. doi:10.1016/B978-0-444-89307-9.50008-8. ISBN 9780444893079.
^ Salinas, Antonio J.; Vallet-Regí, María (2013). "Bioactive ceramics: From bone grafts to tissue engineering". RSC Advances. 3 (28): 11116. Bibcode:2013RSCAd...311116S. doi:10.1039/C3RA00166K.
^ ^a ^b Rey, C.; Combes, C.; Drouet, C.; Grossin, D. (2011). "Bioactive Ceramics: Physical Chemistry". Comprehensive Biomaterials. pp. 187–221. doi:10.1016/B978-0-08-055294-1.00178-1. ISBN 9780080552941.
^ Tamimi, Faleh; Sheikh, Zeeshan; Barralet, Jake (2012). "Dicalcium phosphate cements: Brushite and monetite". Acta Biomaterialia. 8 (2): 474–487. doi:10.1016/j.actbio.2011.08.005. PMID 21856456.
^ Curry, N. A.; Jones, D. W. (1971). "Crystal structure of brushite, calcium hydrogen orthophosphate dihydrate: A neutron-diffraction investigation". Journal of the Chemical Society A: Inorganic, Physical, Theoretical: 3725. doi:10.1039/J19710003725.
^ Lu, Bing-Qiang; Willhammar, Tom; Sun, Ben-Ben; Hedin, Niklas; Gale, Julian D.; Gebauer, Denis (2020-03-24). "Introducing the crystalline phase of dicalcium phosphate monohydrate". Nature Communications. 11 (1): 1546. Bibcode:2020NatCo..11.1546L. doi:10.1038/s41467-020-15333-6. ISSN 2041-1723. PMC 7093545. PMID 32210234.
^ Schrödter, Klaus; Bettermann, Gerhard; Staffel, Thomas; Wahl, Friedrich; Klein, Thomas; Hofmann, Thomas (2008). "Phosphoric Acid and Phosphates". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a19_465.pub3. ISBN 978-3527306732. S2CID 94458523.
^ Pak, Charles Y.C.; Poindexter, John R.; Adams-Huet, Beverley; Pearle, Margaret S. (2003). "Predictive value of kidney stone composition in the detection of metabolic abnormalities". The American Journal of Medicine. 115 (1): 26–32. doi:10.1016/S0002-9343(03)00201-8. PMID 12867231.