Chemistry:Calcium phosphate

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Short description: Chemical compound
Calcium phosphate
Smelly cat.png
Calcium Phosphate nanowires seen in SEM
Identifiers
EC Number
  • 233-283-6
UNII
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
Safety data sheet fishersci.com
GHS pictograms GHS07: Harmful
GHS Signal word Warning
H315, H319, H335
P101, P102, P103, P261, P264, P271, P280, P270, P302+352, P304+340, P305+351+338
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
2
1
Flash point Non-flammable
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

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 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).[citation needed]

Orthophosphates, di- and monohydrogen phosphates

These materials contain Ca2+ combined with PO3−4, HPO2−4, or H2PO−4:

  • Monocalcium phosphate, E341 (CAS# 7758-23-8 for anhydrous; CAS#10031-30-8 for monohydrate: Ca(H2PO4)2 and Ca(H2PO4)2(H2O)
  • Dicalcium phosphate (dibasic calcium phosphate), E341(ii) (CAS# 7757-93-9): CaHPO4 (mineral: monetite), dihydrate CaHPO4(H2O)2 (mineral: brushite) and monohydrate CaHPO4(H2O)
  • Tricalcium phosphate (tribasic calcium phosphate or tricalcic phosphate, sometimes referred to as calcium phosphate or calcium orthophosphate, whitlockite), E341(iii) (CAS#7758-87-4): Ca3(PO4)2
  • Octacalcium phosphate (CAS# 13767-12-9): Ca8H2(PO4)6·5H2O
  • Amorphous calcium phosphate, a glassy precipitate of variable composition that may be present in biological systems.

Di- and polyphosphates

These materials contain Ca2+ combined with the polyphosphates, such as P2O4−7 and triphosphate P3O5−10:

  • Dicalcium diphosphate (CAS#7790-76-3]: Ca2P2O7
  • Calcium triphosphate (CAS# 26158-70-3): Ca5(P3O10)2

Hydroxy- and oxo-phosphates

These materials contain other anions in addition to phosphate:[citation needed]

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.[5]

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. [6]

  • 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.

References

  1. ↑ 1.0 1.1 "Calcium Phosphate". https://pubchem.ncbi.nlm.nih.gov/compound/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. 
  3. ↑ "What Substances Make Up Your Teeth? – Affordable Dental Care" (in en-us). 2015-07-15. https://www.towncaredental.com/blog/what-substances-make-up-your-teeth/. 
  4. ↑ A. Y. Tamime, ed (2006). Brined cheeses - The Society of Dairy Technology (SDT). Wiley-Blackwell. ISBN 978-1-4051-2460-7. 
  5. ↑ Frassetto L, Kohlstadt I (2011). "Treatment and prevention of kidney stones: an update.". Am Fam Physician 84 (11): 1234–42. PMID 22150656. https://pubmed.ncbi.nlm.nih.gov/22150656. 
  6. ↑ 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. PMID 19881103. 



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