Ammonium hexacyanoferrate(II)
| Names | |
|---|---|
| IUPAC name
Ammonium hexacyanoferrate(II)
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Other names
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| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.034.963 |
| EC Number |
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| 46775 | |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| C6H16FeN10 | |
| Molar mass | 284.109 g·mol−1 |
| Appearance | green solid |
| Density | 1.423 g/cm3[1] |
| soluble | |
| Solubility | insoluble in ethanol |
| Structure[1] | |
| cubic (sesquihydrate) | |
| Ia3d (No. 230) | |
a = 18.261 Å α = 90°, β = 90°, γ = 90°
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Formula units (Z)
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16 units per cell |
| Hazards | |
| GHS labelling:[2] | |
| Warning | |
| H302, H312, H332 | |
| P261, P264, P270, P271, P280, P301+P317, P302+P352, P304+P340, P317, P321, P330, P362+P364, P501 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
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Ammonium hexacyanoferrate(II) is an inorganic compound with the chemical formula (NH4)4[Fe(CN)6]. A hygroscopic, yellowish-green monohydrate as well as a trihydrate exist.[3] A sesquihydrate has been characterized.[1] The compound loses NH3 on exposure to air and light.[3]
Synthesis
Ammonium hexacyanoferrate(II) can be prepared by the neutralization of ferrocyanic acid with ammonia solution followed by salting with ethanol:[4]
- H4Fe(CN)6 + 4NH3 → (NH4)4[Fe(CN)6]
Uses
It is of research interest as a catholyte in flow batteries.[5][6]
Reactions
The compound decomposes with the sequential formation of (NH4)3[FeIII(CN)6],
(NH4)3[FeII(CN)5], FeIII
4 [FeII(CN)6]3 (Prussian blue), and finally Fe2O3.[7] Prussian blue nanoparticles as well as amorphous Fe2O3 nanoparticles can be prepared using this method.
Related compounds
Double salts such as ammonium barium hexacyanoferrate(II) trihydrate (Ba(NH4)2[Fe(CN)6]·3H2O) have been characterized.[8]
References
- ^ a b c Morosin, B. (1978-12-01). "The hydrate of ammonium ferrocyanide and possible ionic transport mechanism". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry. 34 (12): 3730–3731. doi:10.1107/S056774087801198X. ISSN 0567-7408.
- ^ PubChem. "Ammonium ferrocyanide". pubchem.ncbi.nlm.nih.gov. Retrieved 2026-05-05.
- ^ a b Perry, Dale L. (19 April 2016). Handbook of Inorganic Compounds. CRC Press. p. 24. ISBN 978-1-4398-1462-8. Retrieved 18 September 2024.
- ^ Brauer, Georg (2 December 2012). Handbook of Preparative Inorganic Chemistry V2. Elsevier. p. 1509. ISBN 978-0-323-16129-9. Retrieved 18 September 2024.
- ^ Luo, Jian; Hu, Bo; Debruler, Camden; Bi, Yujing; Zhao, Yu; Yuan, Bing; Hu, Maowei; Wu, Wenda; Liu, T. Leo (January 2019). "Unprecedented Capacity and Stability of Ammonium Ferrocyanide Catholyte in pH Neutral Aqueous Redox Flow Batteries". Joule. 3 (1): 149–163. doi:10.1016/j.joule.2018.10.010. ISSN 2542-4351.
- ^ Mouselly, Maryam; Alawadhi, Hussain; Senthilkumar, Sirugaloor Thangavel (2024-12-01). "Current status of ferro-/ferricyanide for redox flow batteries". Current Opinion in Electrochemistry. 48 101581. doi:10.1016/j.coelec.2024.101581. ISSN 2451-9103.
- ^ Machala, Libor; Zbořil, Radek (2016). "Thermal decomposition of ammonium ferrocyanide, (NH4)4[Fe(CN)6], in air": 020005. doi:10.1063/1.4966001.
{{cite journal}}: Cite journal requires|journal=(help) - ^ Córdoba, Lucrecia Medina; Echeverría, Gustavo A.; Piro, Oscar E.; Gómez, M. Inés (June 2015). "Ammonium, barium hexacyanoferrate(II) trihydrate: Synthesis, crystal structure, thermal decomposition and spectroscopic study". Journal of Thermal Analysis and Calorimetry. 120 (3): 1827–1834. doi:10.1007/s10973-015-4492-5. hdl:11336/49979. ISSN 1388-6150.