Ammonium ferric citrate (also known as ferric ammonium citrate or ammoniacal ferrous citrate) has the formula [NH4]y[Fex(C6H4O7)]. The iron in this compound is trivalent. All three carboxyl groups and the central hydroxyl group of citric acid are deprotonated. A distinguishing feature of this compound is that it is very soluble in water, in contrast to ferric citrate which is not very soluble.[3]
-citrat_V7.svg) Structure of ammonium ferric citrate
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 Crystal structure of [NH4]5[Fe(C6H4O7)2]·2H2O[1]
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| Names | |
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| IUPAC name
2-Hydroxypropane-1,2,3-tricarboxylate, ammonium iron(3 ) salt
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| Other names
Ferric ammonium citrate
Ammonium iron(III) citrate Ammonium ferric citrate Iron ammonium citrate FerriSeltz | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChEMBL | |
| ChemSpider | |
| ECHA InfoCard | 100.013.351 |
| EC Number |
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| E number | E381 (antioxidants, ...) |
| KEGG | |
PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| C6H8O7⋅xFe3 ⋅yNH3 | |
| Appearance | yellow crystals |
| Pharmacology | |
| V08CA07 (WHO) | |
| Hazards | |
| Safety data sheet (SDS) | [1] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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In its crystal structure each moiety of citric acid has lost four protons. The deprotonated hydroxyl group and two of the carboxylate groups ligate to the ferric center, while the third carboxylate group coordinates with the ammonium.[1]
Uses
editAmmonium ferric citrate has a range of uses, including:
- As a food ingredient, it has an INS number 381, and is used as an acidity regulator.[4] Most notably used in the Scottish beverage Irn-Bru.
- Water purification[5]
- As a reducing agent of metal salts of low activity like gold and silver[5]
- With potassium ferricyanide as part of the cyanotype photographic process
- Used in Kligler's Iron Agar (KIA) test to identify enterobacteriaceae bacteria by observing their metabolism of different sugars, producing hydrogen sulfide[6]
- In medical imaging, ammonium ferric citrate is used as a contrast medium.
- As a hematinic[7]
See also
editReferences
edit- ^ a b Matzapetakis, M.; Raptopoulou, C. P.; Tsohos, A.; Papaefthymiou, V.; Moon, N.; Salifoglou, A. (1998). "Synthesis, Spectroscopic and Structural Characterization of the First Mononuclear, Water Soluble Iron−Citrate Complex, (NH4)5Fe(C6H4O7)2·2H2O". J. Am. Chem. Soc. 120 (50): 13266–13267. doi:10.1021/ja9807035.13266-13267&rft.date=1998&rft_id=info:doi/10.1021/ja9807035&rft.aulast=Matzapetakis&rft.aufirst=M.&rft.au=Raptopoulou, C. P.&rft.au=Tsohos, A.&rft.au=Papaefthymiou, V.&rft.au=Moon, N.&rft.au=Salifoglou, A.&rfr_id=info:sid/en.wikipedia.org:Ammonium ferric citrate" class="Z3988">
- ^ "KEGG DRUG: Ferric ammonium citrate".
- ^ PubChem. "Ammonium ferric citrate". pubchem.ncbi.nlm.nih.gov. Retrieved 4 October 2022.
- ^ "AMMONIUM FERRIC CITRATE". World Health Organization. Retrieved 21 September 2022.
- ^ a b "Ammonium Ferric Citrate Properties, Molecular Formula, Applications – WorldOfChemicals". worldofchemicals.com. Retrieved 17 October 2022.
- ^ Aryal, Sagar (28 November 2018). "Kligler's Iron Agar Test – Procedure, Uses and Interpretation". MicrobiologyInfo.com. Retrieved 5 November 2021.
- ^ Budavari, Susan, ed. (2001). The Merck Index: An Encyclopedia of Chemicals, Drugs, and Biologicals (13th ed.). Merck. ISBN 0911910131.