Calcium phosphate

For the function of calcium phosphate in organisms, see Calcium metabolism.
Calcium phosphate
Hydroxyapatite crystal
Identifiers
EC Number
  • 233-283-6
E number E341 (antioxidants, ...)
UNII
  • Key: QORWJWZARLRLPR-UHFFFAOYSA-H
Properties
Ca3(PO4)2
Molar mass 310.18 g/mol
Appearance White Solid
Odor Odorless
Density 3.14 g/cu cm[1]
Melting point 1,670 °C (3,040 °F; 1,940 K)[1]
Practically insoluble with water
Solubility in Ethanol Insoluble with ethanol (also acetic acid)
Hazards
GHS labelling:
GHS07: Exclamation mark
Warning
H315, H319, H335
P101, P102, P103, P261, P264, P270, P271, P280, P302+P352, P304+P340, P305+P351+P338
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
2
0
1
Flash point Non-flammable
Safety data sheet (SDS) fishersci.com
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

The term calcium phosphate refers to a family of materials and minerals containing calcium ions (Ca2+) together with inorganic phosphate anions. Some so-called calcium phosphates contain oxide and hydroxide as well. Calcium phosphates are white solids of nutritional value[2] and are found in many living organisms, e.g., bone mineral and tooth enamel.[3] In milk, it exists in a colloidal form in micelles bound to casein protein with magnesium, zinc, and citrate–collectively referred to as colloidal calcium phosphate (CCP).[4] Various calcium phosphate minerals, which often are not white owing to impurities, are used in the production of phosphoric acid and fertilizers. Overuse of certain forms of calcium phosphate can lead to nutrient-containing surface runoff and subsequent adverse effects upon receiving waters such as algal blooms and eutrophication (over-enrichment with nutrients and minerals).[5]

Orthophosphates, di- and monohydrogen phosphates

These materials contain Ca2+ combined with PO3−
4, HPO2−
4, or H
2PO−
4:

Di- and polyphosphates

These materials contain Ca2+ combined with the polyphosphates, such as P
2O4−
7 and triphosphate P
3O5−
10:

Hydroxy- and oxo-phosphates

These materials contain other anions in addition to phosphate:

Clinical significance

Calcium phosphate stones account for approximately 15% of kidney stone disease. Calcium phosphate stones tend to grow in alkaline urine, especially when Proteus bacteria are present. It is the most common type in pregnant women.[6]

Calcium phosphate is the usual constitution of microcalcifications of the breast, particularly dystrophic calcifications. Microcalcifications as can be seen on mammography can be an early sign of breast cancer. Based on morphology, it is possible to classify by radiography how likely microcalcifications are to indicate cancer.[7]

  • Urine crystals comparison, with calcium phosphate crystal depicted at top center.
    Urine crystals comparison, with calcium phosphate crystal depicted at top center.
  • Histopathology of dystrophic calcium phosphate microcalcifications in ductal carcinoma in situ (DCIS) of the breast, H&E stain.
    Histopathology of dystrophic calcium phosphate microcalcifications in ductal carcinoma in situ (DCIS) of the breast, H&E stain.

References

  1. ^ a b "Calcium Phosphate".
  2. ^ Klaus Schrödter; Gerhard Bettermann; Thomas Staffel; Friedrich Wahl; Thomas Klein; Thomas Hofmann (2008). "Phosphoric Acid and Phosphates". Ullmann's Encyclopedia of Industrial Chemistry. Ullmann’s Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_465.pub3. ISBN 978-3527306732. S2CID 94458523.
  3. ^ "What Substances Make Up Your Teeth? – Affordable Dental Care". www.towncaredental.com. 2015-07-15. Retrieved 2021-01-29.
  4. ^ A. Y. Tamime, ed. (2006). Brined cheeses - The Society of Dairy Technology (SDT). Wiley-Blackwell. ISBN 978-1-4051-2460-7.
  5. ^ Xiao, Zhengyang; Tan, Albern X.; Xu, Vincent; Jun, Young-Shin; Tang, Yinjie J. (2022). "Mineral-hydrogel composites for mitigating harmful algal bloom and supplying phosphorous for photo-biorefineries". Science of the Total Environment. 847: 157533. Bibcode:2022ScTEn.84757533X. doi:10.1016/j.scitotenv.2022.157533. PMC 9755271. PMID 35878849.
  6. ^ Frassetto L, Kohlstadt I (2011). "Treatment and prevention of kidney stones: an update". Am Fam Physician. 84 (11): 1234–42. PMID 22150656.
  7. ^ Nalawade, Yojana V (November 2009). "Evaluation of breast calcifications". The Indian Journal of Radiology & Imaging. 19 (4): 282–286. doi:10.4103/0971-3026.57208. ISSN 0971-3026. PMC 2797739. PMID 19881103.

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