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{{short description|Chemical compound}}
'''Calcium phosphate''' is the name given to a family of [[mineral|minerals]] containing calcium ions (Ca<sup>2+</sup>) together with orthophosphates (PO<sub>4</sub><sup>3-</sup>), metaphosphates or pyrophosphates (P<sub>2</sub>O<sub>7</sub><sup>4-</sup>) and occasionally hydrogen or hydroxide ions.
{{For|the function of calcium phosphate in organisms|Calcium metabolism}}
{{refimprove|date=March 2019}}
{{Chembox
| ImageFile = Smelly cat.png
| ImageCaption = Calcium Phosphate nanowires seen in SEM
| Section1 = {{Chembox Identifiers
| CASNo = 7758-87-4
| EC_number = 233-283-6
| PubChem = 24456
| UNII = K4C08XP666
| StdInChIKey = QORWJWZARLRLPR-UHFFFAOYSA-H
⚫
}}
| Section2 = {{Chembox Properties
⚫
| Formula = Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>
| MolarMass = 310.18 g/mol
| Appearance = White Solid
| Odor = Odorless
| Density = 3.14 g/cu cm<ref name=crc>{{cite web | url=https://pubchem.ncbi.nlm.nih.gov/compound/Calcium-phosphate | title=Calcium Phosphate }}</ref>
| MeltingPtC = 1670
| MeltingPt_ref = <ref name=crc/>
| Solubility = Practically insoluble with [[water]]
| Solvent2 = Ethanol
| Solubility2 = Insoluble with [[ethanol]] (also [[acetic acid]])
}}
| Section3 = {{Chembox Hazards
| GHSPictograms = {{GHS07}}
| GHSSignalWord = Warning
| HPhrases = {{H-phrases|315|319|335}}
| PPhrases = {{P-phrases|101|102|103|261|264|271|280|270|302+352|304+340|305+351+338}}
| NFPA-H = 2
| NFPA-F = 0
| NFPA-R = 1
| NFPA-S =
| FlashPt = Non-flammable
| ExternalSDS = [https://beta-static.fishersci.com/content/dam/fishersci/en_US/documents/programs/education/regulatory-documents/sds/chemicals/chemicals-c/S25229.pdf fishersci.com]
}}
}}
The term '''calcium phosphate''' refers to a family of materials and [[mineral]]s containing [[calcium]] [[ion]]s (Ca<sup>2+</sup>) together with inorganic [[phosphate]] anions. Some so-called calcium phosphates contain [[oxide]] and [[hydroxide]] as well. Calcium phosphates are white solids of nutritional value<ref name=Ullmann>{{cite book|author1=Klaus Schrödter|author2=Gerhard Bettermann|author3=Thomas Staffel|author4=Friedrich Wahl|author5=Thomas Klein|author6=Thomas Hofmann|title=Ullmann's Encyclopedia of Industrial Chemistry|chapter=Phosphoric Acid and Phosphates|series=Ullmann’s Encyclopedia of Industrial Chemistry|year=2008|publisher=Wiley-VCH|place=Weinheim|doi=10.1002/14356007.a19_465.pub3|isbn=978-3527306732|s2cid=94458523 }}</ref> and are found in many living organisms, e.g., [[bone mineral]] and [[tooth enamel]].<ref>{{Cite web|date=2015-07-15|title=What Substances Make Up Your Teeth? – Affordable Dental Care|url=https://www.towncaredental.com/blog/what-substances-make-up-your-teeth/|access-date=2021-01-29|website=www.towncaredental.com|language=en-us}}</ref> 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).<ref>{{cite book|title=Brined cheeses - The Society of Dairy Technology (SDT)|publisher=Wiley-Blackwell|year=2006|isbn=978-1-4051-2460-7|editor=A. Y. Tamime}}</ref> Various calcium phosphate minerals are used in the production of [[phosphoric acid]] and [[fertilizer]]s. Overuse of certain forms of calcium phosphate can lead to [[nutrient]]-containing [[surface runoff]] and subsequent adverse effects upon receiving waters such as [[algal bloom]]s and [[eutrophication]] (over-enrichment with nutrients and minerals).{{cn|date=July 2022}}


==Orthophosphates, di- and monohydrogen phosphates==
==Varieties of CaP==
These materials contain Ca<sup>2+</sup> combined with {{chem|PO|4|3−}}, {{chem|HPO|4|2−}}, or {{chem|H|2|PO|4|−}}:
{|
|[[Tricalcium phosphate]] || Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub> (occurs in alpha and hi phases; beta also known as [[Whitlockite]])
* [[Monocalcium phosphate]], E341 (CAS# 7758-23-8 for anhydrous; CAS#10031-30-8 for monohydrate: Ca(H<sub>2</sub>PO<sub>4</sub>)<sub>2</sub> and Ca(H<sub>2</sub>PO<sub>4</sub>)<sub>2</sub>(H<sub>2</sub>O)
* [[Dicalcium phosphate]] (dibasic calcium phosphate), E341(ii) (CAS# 7757-93-9): CaHPO<sub>4</sub> (mineral: [[monetite]]), dihydrate CaHPO<sub>4</sub>(H<sub>2</sub>O)<sub>2</sub> (mineral: [[brushite]]) and monohydrate CaHPO<sub>4</sub>(H<sub>2</sub>O)
|-
* [[Tricalcium phosphate]] (tribasic calcium phosphate or tricalcic phosphate, sometimes referred to as calcium phosphate or calcium orthophosphate, [[whitlockite]]), E341(iii) (CAS#7758-87-4): Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>
|[[Calcium monohydrogen phosphate]] || CaHPO<sub>4</sub>
⚫
* [[Octacalcium phosphate]] (CAS# 13767-12-9): Ca<sub>8</sub>H<sub>2</sub>(PO<sub>4</sub>)<sub>6</sub>·5H<sub>2</sub>O
|-
* [[Amorphous calcium phosphate]], a glassy precipitate of variable composition that may be present in biological systems.
⚫
|[[Calcium dihydrogen phosphate]] || Ca(H<sub>2</sub>PO<sub>4</sub>)<sub>2</sub>
|-
|[[Calcium pyrophosphate]] || Ca<sub>2</sub>P<sub>2</sub>O<sub>7</sub> (occurs as alpha, beta and gamma phases)
|-
⚫
|[[Hydroxylapatite]] || Ca<sub>10</sub>(PO<sub>4</sub>)<sub>6</sub>(OH)<sub>2<sub/>
⚫
|}


==Di- and polyphosphates==
==Natural Abundance==
These materials contain Ca<sup>2+</sup> combined with the [[polyphosphate]]s, such as [[pyrophosphate|{{chem|P|2|O|7|4−}}]] and triphosphate {{chem|P|3|O|10|5−}}:
It is found in nature as a rock in [[Morocco]], [[Israel]], [[Egypt]], and [[Kola peninsula|Kola]] ([[Russia]]) and in smaller quantities in some other countries. The natural form is not completely pure, and there are some other components like sand and lime which can change the composition. In terms of P<sub>2</sub>O<sub>5</sub>, most calcium phosphate rocks have a content of 30 % to 40 % P<sub>2</sub>O<sub>5</sub> in weight.
* [[Dicalcium diphosphate]] (CAS#7790-76-3]: Ca<sub>2</sub>P<sub>2</sub>O<sub>7</sub>
* [[Calcium triphosphate]] (CAS# 26158-70-3): Ca<sub>5</sub>(P<sub>3</sub>O<sub>10</sub>)<sub>2</sub>


==Hydroxy- and oxo-phosphates==
The skeletons and teeth of [[vertebrate]] animals are composed of calcium phosphate, mainly [[hydroxylapatite]].
These materials contain other anions in addition to phosphate:{{cn|date=May 2023}}
* [[Hydroxyapatite]] Ca<sub>5</sub>(PO<sub>4</sub>)<sub>3</sub>(OH)
* [[Apatite]] Ca<sub>10</sub>(PO<sub>4</sub>)<sub>6</sub>(OH,F,Cl,Br)<sub>2</sub>
* [[Tetracalcium phosphate]] (CAS#1306-01-0): Ca<sub>4</sub>(PO<sub>4</sub>)<sub>2</sub>O


==Clinical significance==
==Uses==
Calcium phosphate stones account for approximately 15% of [[kidney stone disease]]. Calcium phosphate stones tend to grow in alkaline urine, especially when [[Proteus (bacterium)|''Proteus'' bacteria]] are present. It is the most common type in pregnant women.<ref name=Frassetto2011>{{cite journal| author=Frassetto L, Kohlstadt I| title=Treatment and prevention of kidney stones: an update. | journal=Am Fam Physician | year= 2011 | volume= 84 | issue= 11 | pages= 1234–42 | pmid=22150656 | doi= | pmc= | url=https://pubmed.ncbi.nlm.nih.gov/22150656 }}</ref>
Calcium phosphate is an important raw material for the production of [[phosphoric acid]] and [[fertilizer]]s, for example in the [[Odda process]].


Calcium phosphate is the usual constitution of [[microcalcification]]s of the [[breast]], particularly [[dystrophic calcification]]s. 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.
Calcium phosphate is also a raising agent (food additives) E341. Is a mineral salt found in rocks and bones, it is used in cheese products. No known side effects.
<ref>{{cite journal |last1=Nalawade |first1=Yojana V |title=Evaluation of breast calcifications |journal=The Indian Journal of Radiology & Imaging |date=November 2009 |volume=19 |issue=4 |pages=282–286 |doi=10.4103/0971-3026.57208 |pmid=19881103 |issn=0971-3026|pmc=2797739 |doi-access=free }}</ref>
<gallery heights=160 widths=200>
File:Urine crystals comparison.png|Urine crystals comparison, with calcium phosphate crystal depicted at top center.
File:Histopathology of dystrophic microcalcifications in ductal carcinoma in situ.jpg|Histopathology of dystrophic calcium phosphate microcalcifications in [[ductal carcinoma in situ]] (DCIS) of the breast, H&E stain.
</gallery>


==References==
Another practical application of the compound is its use in [[gene transfection]]. The Calcium [[ions]] can make a [[Cell (biology)|cell]] [[competent]] (a [[euphemism]] for "rip holes in its [[membrane]]") to allow exogenous [[genes]] to enter the cell by [[diffusion]]. A [[heat shock]] afterwards then invokes the cell to repair itself. This is a quick and easy method for [[transfection]], albeit a rather inefficient one.
{{Reflist}}


{{Calcium compounds}}
{{Phosphates}}

{{DEFAULTSORT:Calcium Phosphate}}
[[Category:Calcium compounds]]
[[Category:Calcium compounds]]
[[Category:Phosphates]]
[[Category:Phosphates]]
[[Category:Excipients]]
[[Category:E-number additives]]

Latest revision as of 22:27, 8 December 2023

For the function of calcium phosphate in organisms, see Calcium metabolism.
Calcium phosphate

Calcium Phosphate nanowires seen in SEM
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 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[edit]

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

Di- and polyphosphates[edit]

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

Hydroxy- and oxo-phosphates[edit]

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

Clinical significance[edit]

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.
    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[edit]

  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. ^ Frassetto L, Kohlstadt I (2011). "Treatment and prevention of kidney stones: an update". Am Fam Physician. 84 (11): 1234–42. PMID 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. PMC 2797739. PMID 19881103.
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