// Workers AI · dad joke modeWhat did Strontium phosphate say? I'm bonded to you.
| Identifiers | |
|---|---|
3D model (JSmol) |
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| ChemSpider | |
| ECHA InfoCard | 100.028.369 |
| EC Number |
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PubChem CID |
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| UNII | |
CompTox Dashboard (EPA) |
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| Properties | |
| Sr3(PO4)2 | |
| Molar mass | 452.8 g/mol |
| Appearance | White solid |
| Density | 4.53 g/cm3 |
| Melting point | 1,620 °C (2,950 °F; 1,890 K)[1] |
| Insoluble[2][3] | |
| Structure[4] | |
| Rhombohedral | |
| R3m | |
a = 5.39 Å, c = 19.78 Å | |
Lattice volume (V) |
497.8 Å3 |
| Related compounds | |
Other anions |
Strontium sulfate |
Other cations |
Tricalcium phosphate Barium 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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Strontium phosphate is the phosphate salt of strontium, with the molecular formula Sr3(PO4)2. It is a white solid insoluble in water.[5]
Preparation and properties
[edit]Strontium phosphate is commonly produced by the reaction of soluble strontium compounds, such as strontium nitrate, and a phosphate source, such as phosphoric acid or tripotassium phosphate, in water, resulting in a white precipitate of the tetrahydrate:[6][7]
- 3 Sr(NO3)2 + 2 K3PO4 + 4 H2O → Sr3(PO4)2·4H2O↓ + 6 KNO3
Under water, the tetrahydrate slowly hydrolyses to strontium hydroxyapatite (Sr10(PO4)6(OH)2). The tetrahydrate decomposes to the anhydrous form when heated to 900 °C.[6][7]
The anhydrous form can be produced without the presence of water, to avoid hydrolysis, by the heating of ammonium dihydrogen phosphate and strontium carbonate at 1030 °C and 30 MPa of pressure.[4][8]
References
[edit]- ↑ Looney, James R.; Brown, Jesse J. (1971). "Phase Equilibria in the Sr3(PO4)2-Cd3(PO4)2 System and Eu2+-Activated Luminescence of Sr3(PO4)2 and Related Phases". Journal of the Electrochemical Society. 118 (3): 470. doi:10.1149/1.2408084.
- ↑ Haynes, W. M., ed. (2014). CRC Handbook of Chemistry and Physics (95th ed.). Boca Raton, Florida: CRC Press. p. 4-92. ISBN 9781482208672.
- ↑ Verbeeck, R. M. H.; Kiekens, P.; Driessens, F. C. M. (1981). "Phase Equilibria in Strontium Orthophosphate Solutions at 25° C". Zeitschrift für Physikalische Chemie. 124 (1): 45–53. doi:10.1524/zpch.1981.124.1.045. ISSN 2196-7156.
- 1 2 Sugiyama, Kazumasa; Tokonami, Masayasu (1990). "The crystal structure refinements of the strontium and barium orthophosphates". Mineralogical Journal. 15 (4): 141–146. Bibcode:1990MinJ...15..141S. doi:10.2465/minerj.15.141. ISSN 0544-2540.
- ↑ "Strontium phosphate". PubChem. Retrieved 4 July 2025.
- 1 2 Collin, Robert L. (1966). "Precipitate Formation in the Strontium-Phosphate System". Science. 151 (3716): 1386–1388. Bibcode:1966Sci...151.1386C. doi:10.1126/science.151.3716.1386. ISSN 0036-8075. PMID 5909785.
- 1 2 Collin, Robert L. (1964). "Preparation and Properties of Two Strontium Orthophosphates-Sr 3 (PO 4 ) 2 ˙4H 2 O and Sr 6 H 3 -(PO 4 ) 5 ˙2H 2 O.". Journal of Chemical & Engineering Data. 9 (2): 165–166. doi:10.1021/je60021a002. ISSN 0021-9568.
- ↑ Zhai, Shuangmeng; Liu, Ang; Xue, Weihong; Song, Yang (2011). "High-pressure Raman spectroscopic studies on orthophosphates Ba3(PO4)2 and Sr3(PO4)2". Solid State Communications. 151 (4): 276–279. doi:10.1016/j.ssc.2010.12.007.