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Sodium ferrocyanide: Difference between revisions

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{{chembox {{chembox
| Watchedfields = changed
| verifiedrevid = 396450798 | verifiedrevid = 440300753
| Reference = <ref></ref> | Reference = <ref> {{webarchive|url=https://web.archive.org/web/20100517032546/http://siri.org/msds/f2/bdn/bdnqc.html |date=2010-05-17 }}</ref>
| Name = Sodium ferrocyanide | Name = Sodium ferrocyanide
| ImageFile = sodium ferrocyanide.png | ImageFile = sodium ferrocyanide.png
| ImageSize = 200px | ImageSize = 200px
| IUPACName = Tetrasodium | IUPACName = Tetrasodium
| OtherNames = Yellow prussiate of soda (YPS), Tetrasodium hexacyanoferrate, Gelbnatron, Ferrocyannatrium | OtherNames = {{Unbulleted list|Yellow prussiate of soda (YPS)|Tetrasodium hexacyanoferrate|Gelbnatron|Ferrocyannatrium|sodium hexacyanoferrate(II)|Yellow blood salt{{citation needed|date=December 2015}}}}
| Section1 = {{Chembox Identifiers |Section1={{Chembox Identifiers
| CASNo_Ref = {{cascite|correct|??}}
| CASNo = 13601-19-9 | CASNo = 13601-19-9
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 5HT6X21AID
| EINECS = 237-081-9 | EINECS = 237-081-9
| PubChem = 26129 | PubChem = 26129
| RTECS = | RTECS =
| InChI = 1S/6CN.Fe.4Na/c6*1-2;;;;;/q6*-1;+2;4*+1
| SMILES = ..N#C(C#N)(C#N)(C#N)(C#N)C#N..
}} }}
| Section2 = {{Chembox Properties |Section2={{Chembox Properties
| Formula = Na<sub>4</sub>Fe(CN)<sub>6</sub> | Formula = Na<sub>4</sub>
| MolarMass = 303.91 g/mol | MolarMass = 303.91 g/mol
| Appearance = Yellow crystals | Appearance = pale yellow crystals
| Odor = odorless
| Density = 1.458 g/cm<sup>3</sup> | Density = 1.458 g/cm<sup>3</sup>
| Solubility = 18 g/100 mL | Solubility = 10.2 g/100 mL (10 °C) <br> 17.6 g/100 mL (20 °C) <br> 39.7 g/100 mL (96.6 °C)
| MeltingPt = 435 °C (decomposes) | MeltingPt = {{convert|435|C|F K}} (anhydrous) <br>{{convert|81.5|C|F K}} (decahydrate)
| MeltingPt_notes = (decomposes)
| BoilingPt = | BoilingPt =
| RefractIndex = 1.530
}} }}
| Section3 = {{Chembox Structure |Section3={{Chembox Structure
| Coordination = | Coordination =
| CrystalStruct = ] | CrystalStruct = ]
}} }}
| Section7 = {{Chembox Hazards |Section7={{Chembox Hazards
| MainHazards = | MainHazards =
| RPhrases = | GHSPictograms =
| GHSSignalWord =
| SPhrases = {{S22}} {{S24}} {{S25}}
| HPhrases = {{HPhrases|}}
| PPhrases = {{PPhrases|}}
| GHS_ref = <!-- NO DATA <ref>GHS: </ref> -->
}} }}
| Section8 = {{Chembox Related |Section8={{Chembox Related
| OtherAnions = Sodium ferricyanide (Red prussiate of soda) | OtherAnions = Sodium ] (Red prussiate of soda)
| OtherCations = ]
}} }}
}} }}


'''Sodium ferrocyanide''' is the sodium ] of the ] of formula {{chem2|(4-)}}. In its ] form, {{chem2|Na4Fe(CN)6*}}] (] ] ]), it is sometimes known as '''yellow ] of soda'''. It is a yellow ]line solid that is soluble in water and insoluble in ]. The yellow color is the color of ferrocyanide ]. Despite the presence of the ] ]s, sodium ferrocyanide has low ] (acceptable daily intake 0–0.025&nbsp;mg/kg body weight<ref name="toxic">{{cite web |year=1974 |title=Toxicological evaluation of some food additives including anticaking agents, antimicrobials, antioxidants, emulsifiers and thickening agents |url=http://www.inchem.org/documents/jecfa/jecmono/v05je02.htm |archive-url=https://web.archive.org/web/20101201064627/https://inchem.org/documents/jecfa/jecmono/v05je02.htm |archive-date=1 December 2010 |accessdate=18 May 2009 |website=inchem.org |publisher=]}}</ref>). The ]s are less toxic than many salts of cyanide, because they tend not to release free cyanide.<ref name=Holl>{{ cite book |author1=Holleman, A. F. |author2=Wiberg, E. | title = Inorganic Chemistry | publisher = Academic Press | location = San Diego | year = 2001 | isbn = 0-12-352651-5 }}</ref> However, like all ferrocyanide salt solutions, addition of an acid or exposure to UV light can result in the production of ] gas, which is extremely toxic.<ref>{{cite web |last= |title=PubChem Compound Summary for CID 26129, Sodium ferrocyanide |url=https://pubchem.ncbi.nlm.nih.gov/compound/26129 |url-status=live |archive-url=https://web.archive.org/web/20230213172049/https://pubchem.ncbi.nlm.nih.gov/compound/26129 |archive-date=2023-02-13 |access-date=2023-01-17 |website=National Center for Biotechnology Information |publisher=PubChem |language=en}}</ref><ref>{{cite web |last= |title=PubChem Compound Summary for CID 768, Hydrogen Cyanide |url=https://pubchem.ncbi.nlm.nih.gov/compound/768 |url-status=live |archive-url=https://web.archive.org/web/20230303074319/https://pubchem.ncbi.nlm.nih.gov/compound/768 |archive-date=2023-03-03 |access-date=2023-01-17 |website=National Center for Biotechnology Information |publisher=PubChem |language=en}}</ref>
'''Sodium ferrocyanide''', also known as '''tetrasodium hexacyanoferrate''' or '''sodium hexacyanoferrate(II)''', is a ] of formula Na<sub>4</sub>Fe(CN)<sub>6</sub> that forms semitransparent yellow ]s at ] and decomposes at its boiling point. It is soluble in water and insoluble in ]. Despite the presence of the cyanide ligands, sodium ferrocyanide is not especially toxic (acceptable daily intake 0–0.025&nbsp;mg/(kg body weight)<ref name=toxic/>) because the cyanides are tightly bound to the metal. However, as with all ferrocyanides, it can react with acid or photodecompose to release ] gas.

In its ] form, Na<sub>4</sub>Fe(CN)<sub>6</sub>·10H<sub>2</sub>O (sodium ferrocyanide decahydrate), it is sometimes known as '''yellow prussiate of soda (YP Soda)'''. The yellow color is the color of ] anion.


==Uses== ==Uses==
Sodium ferrocyanide is a chemical additive known as '''E 535'''. It is added to road and food grade ] as an ].<ref name=toxic>{{cite web| url =http://www.inchem.org/documents/jecfa/jecmono/v05je02.htm|title = Toxicological evaluation of some food additives including anticaking agents, antimicrobials, antioxidants, emulsifiers and thickening agents| publisher = World Health Organization, Geneva| year = 1974|accessdate = 18 May 2009}}</ref> When combined with iron, it converts to a deep blue pigment, which is the main component of ].<ref>{{cite web| title = Prussian blue |publisher = Encyclopædia Britannica|accessdate =18 May. 2009 |url =http://www.britannica.com/EBchecked/topic/480982/Prussian-blue}}</ref> In photography, it is used for bleaching, toning, and fixing. It is used as a stabilizer for the coating on ] rods. In the ] industry, it is used for removal of ]s. When combined with a Fe(III) salt, it converts to a deep blue pigment called ], {{chem2|Fe4(3+)])6]3}}.<ref>{{cite web |title=Prussian blue |url=http://www.britannica.com/EBchecked/topic/480982/Prussian-blue |url-status=live |archive-url=https://web.archive.org/web/20150905235045/https://www.britannica.com/technology/Prussian-blue |archive-date=5 September 2015 |accessdate=18 May 2009 |publisher=Encyclopædia Britannica}}</ref> It is used as a stabilizer for the coating on ] rods. In the ] industry, it is used for removal of ]s.

In the EU, ferrocyanides (E 535–538) were, as of 2018, solely authorized as additives in ] and ]s, where they serve as ]. The ]s are the organ susceptible to ferrocyanide ], but according to the ], ferrocyanides are of no safety concern at the levels at which they are used.<ref>{{cite journal |last1=Peter Aggett, Fernando Aguilar, Riccardo Crebelli, Birgit Dusemund, Metka Filipič, Maria Jose Frutos, Pierre Galtier, David Gott, Ursula Gundert-Remy, Gunter Georg Kuhnle, Claude Lambré, Jean-Charles Leblanc, Inger Therese Lillegaard, Peter Moldeus, Alicja Mortensen, Agneta Oskarsson, Ivan Stankovic, Ine Waalkens-Berendsen, Rudolf Antonius Woutersen, Matthew Wright and Maged Younes. |title=Re-evaluation of sodium ferrocyanide (E 535), potassium ferrocyanide (E 536) and calcium ferrocyanide (E 538) as food additives |journal=EFSA Journal |date=2018 |volume=16 |issue=7 |page=5374 |doi=10.2903/j.efsa.2018.5374 |pmid=32626000 |pmc=7009536 |url=https://www.efsa.europa.eu/en/efsajournal/pub/5374|doi-access=free }}</ref>

==Production==
Sodium ferrocyanide is produced industrially from ], ], and ], the combination of which affords {{chem2|Ca2*11H2O}}. A solution of this salt is then treated with sodium salts to precipitate the mixed calcium-sodium salt {{chem2|CaNa22}}, which in turn is treated with ] to give the tetrasodium salt.<ref name=Ullmann>{{Ullmann |author1=Gail, E. |author2=Gos, S. |author3=Kulzer, R. |author4=Lorösch, J. |author5=Rubo, A. |author6=Sauer, M. |author7=Kellens, R. |author8=Reddy, J. |author9=Steier, N. |author10=Hasenpusch, W. | title = Cyano Compounds, Inorganic| year = 2011 | publisher = Wiley-VCH | location = Weinheim | doi = 10.1002/14356007.a08_159.pub3 }}</ref>


==References== ==References==
<references/> <references/>
http://www.sodium-ferrocyanide.com
{{Sodium compounds}} {{Sodium compounds}}
{{Med-toxic-stub}}
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