Dicalcium phosphate
Names | |
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IUPAC name
calcium hydrogen phosphate
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Other names
calcium hydrogen phosphate,
phosphoric acid calcium salt (1:1) | |
Identifiers | |
3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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100.028.933 |
E number | E341(ii) (antioxidants, ...) |
PubChem CID
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UNII |
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CompTox Dashboard (EPA)
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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 (fire diamond) | |
Flash point | Non-flammable |
Related compounds | |
Other anions
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Calcium pyrophosphate |
Other cations
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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).
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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 HPO42– 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]
To prevent degradation that would form
In a continuous process CaCl2 can be treated with (NH4)2HPO4 to form the dihydrate:
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]
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
Heating dicalcium phosphate gives
In the dihydrate (brushite) form it is found in some
See also
References
- ^ ISBN 9780444893079.
- .
- ^ ISBN 9780080552941.
- PMID 21856456.
- .
- PMID 32210234.
- S2CID 94458523.
- PMID 12867231.