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			{{Short description|Chemical compound}}
			{{Distinguish|potassium ferricyanide}}
	{{chembox		{{chembox
			| Verifiedfields = changed
	| verifiedrevid = 417486082
			| Watchedfields = changed
	| Name = Potassium ferrocyanide
			| verifiedrevid = 444997361
	| ImageFile = Potassium ferrocyanide.jpg
			| Name = Potassium hexacyanidoferrate(II)
	| ImageSize = 250px
			| ImageFile1 = Structure of potassium ferrocyanide.png
	| ImageName = Potassium ferrocyanide trihydrate
	| IUPACName = Potassium hexacyanidoferrate(II)		| ImageFile2 = Potassium Ferrocyanide.png
			| ImageFile3 = Potassium hexacyanidoferrate(II).jpg
	| OtherNames = Tetrapotassium ferrocyanide, trihydrate; Ferrate (4-), hexacyanido, tetrapotassium, trihydrate<ref>{{cite web |url=http://physchem.ox.ac.uk/MSDS/PO/potassium_ferrocyanide_trihydrate.html |title=Safety (MSDS) data for potassium ferrocyanide trihydrate |date=2006-02-17 |accessdate=2008-02-25 |work=}}</ref>
			| ImageSize3 = 150px
	| Section1 = {{Chembox Identifiers
			| ImageName3 = Potassium ferrocyanide trihydrate
	| CASNo = 13943-58-3
			| IUPACName = Potassium hexacyanidoferrate(II)
	| CASNo_Ref = {{cascite|correct|CAS}}
			| OtherNames = {{Unbulleted list
	| CASOther = (anhydrous)<br/>14459-95-1 (trihydrate)
			| (Yellow) Prussiate of Potash<ref>{{Cite book|url=https://play.google.com/books/reader?printsec=frontcover&output=reader&id=gXwPAAAAYAAJ&pg=GBS.PA8|title = Five Hundred Useful and Amusing Experiments in Chemistry, and in the Arts and Manufactures: With Observations on the Properties Employed, and Their Application to Useful Purposes|year = 1825|publisher = Thomas Tegg}}</ref>
	| PubChem = 161067
			| Potassium&nbsp;hexacyanoferrate&nbsp;(II) trihydrate
	| RTECS =
			| Tetrapotassium&nbsp;ferrocyanide trihydrate
			| Ferrate&nbsp;hexacyano tetrapotassium trihydrate<ref name=JTBaker/>
			}}
			| Section1 = {{Chembox Identifiers
			| CASNo = 13943-58-3
			| CASNo_Ref = {{cascite|correct|CAS}}
			| CASNo_Comment = (anhydrous)
			| CASNo2_Ref = {{cascite|correct|CAS}}
			| CASNo2 = 14459-95-1
			| CASNo2_Comment = (trihydrate)
			| ChemSpiderID = 20162028
			| EINECS = 237-722-2
			| UNII_Ref = {{fdacite|correct|FDA}}
			| UNII = GTP1P30292
			| UNII_Comment = (anhydrous)
			| UNII2 = 961WP42S65
			| UNII2_Comment = (trihydrate)
			| UNII2_Ref = {{fdacite|correct|FDA}}
			| PubChem = 161067
			| SMILES = ..N#C(C#N)(C#N)(C#N)(C#N)C#N..
			| StdInChI=1S/6CN.Fe.4K.3H2O/c6*1-2;;;;;;;;/h;;;;;;;;;;;3*1H2/q6*-1;+2;4*+1;;;
			| StdInChIKey = UTYXJYFJPBYDKY-UHFFFAOYSA-N
	}}		}}
	| Section2 = {{Chembox Properties		| Section2 = {{Chembox Properties
	| Formula = C<sub>6</sub>N<sub>6</sub>FeK<sub>4</sub>		| Formula = K<sub>4</sub>
	| MolarMass = 368.35 g/mol (anhydrous)<br/>422.388 g/mol (trihydrate)		| MolarMass = 368.35 g/mol (anhydrous)<br />422.388 g/mol (trihydrate)
	| Appearance = Light yellow, crystalline granules.		| Appearance = Light yellow, crystalline granules
	| Density = 1.85 g/cm<sup>3</sup> (trihydrate)		| Density = 1.85 g/cm<sup>3</sup> (trihydrate)
	| Solubility = ''trihydrate'' <br> 28.9 g/100 mL (20 °C)		| Solubility = ''trihydrate'' <br /> 28.9 g/100 mL (20&nbsp;°C)
	| SolubleOther = insoluble in ], ]		| SolubleOther = insoluble in ], ]
	| MeltingPt = 69-71°C		| MeltingPtC =
			| BoilingPtC =
	| BoilingPt = 400°C (decomp)
			| BoilingPt_notes = (decomposes)
			| MagSus = &minus;130.0·10<sup>−6</sup> cm<sup>3</sup>/mol
	}}		}}
	| Section7 = {{Chembox Hazards		| Section7 = {{Chembox Hazards
	| ExternalMSDS =		| ExternalSDS =
	| MainHazards =		| MainHazards =
			| FlashPt = Non-flammable
	| EUIndex = Not listed
			| GHSPictograms = {{GHS09}}
	| FlashPt = Non-flammable
			| GHSSignalWord = Warning
	| RPhrases = {{R32}}, {{R52}}, {{R53}}
	| SPhrases = {{S50}}(B), {{S61}}		| HPhrases = {{H-phrases|411}}
			| PPhrases = {{P-phrases|}}
	| NFPA-H = 1
	| NFPA-F = 0		| NFPA-H = 1
	| NFPA-R = 0		| NFPA-F = 0
	| NFPA-O =		| NFPA-R = 0
			| NFPA-S =
			| LD50 = 6400 mg/kg (oral, rat)<ref>https://chem.nlm.nih.gov/chemidplus/rn/13943-58-3 {{Dead link|date=March 2022}}</ref>
	}}		}}
	| Section8 = {{Chembox Related		| Section8 = {{Chembox Related
	| OtherAnions = ]		| OtherAnions = ]
	| OtherCations = ]<br/>]		| OtherCations = ]<br />]
	}}		}}
	}}		}}
	'''Potassium ferrocyanide''', also known as '''potassium prussiate''' or '''yellow prussiate of potash''' or '''potassium hexacyanidoferrate(II)''', is a ] of formula K<sub>4</sub>•3H<sub>2</sub>O, which forms lemon-yellow ] ]s at ], and which decomposes at its boiling point.
			'''Potassium hexacyanidoferrate(II)''' is the ] with formula K<sub>4</sub>·3H<sub>2</sub>O. It is the potassium salt of the ] <sup>4−</sup>. This salt forms lemon-yellow ] ]s.
	==Synthesis==		==Synthesis==
			In 1752, the French chemist ] (1718–1784) first reported the preparation of Potassium hexacyanidoferrate(II), which he achieved by reacting ] (iron(III) ferrocyanide) with ].<ref>{{cite journal |last1=Macquer |title=Éxamen chymique de bleu de Prusse |journal=Histoire de l'Académie Royale des Sciences …, § Mémoires de l'Académie royale des Sciences |date=1752 |pages=60–77 |url=https://www.biodiversitylibrary.org/item/88112#page/250/mode/1up |trans-title=Chemical examination of Prussian blue |language=fr}}
	Potassium ferrocyanide is the product of the reaction between hydrogen ] and ]:
			From pp. 63-64: ''"Après avoir essayé ainsi inutilement de décomposer le bleu de Prusse par les acides, … n'avoit plus qu'une couleur jaune un peu rousse."'' (After having tried so vainly to decompose Prussian blue by acids, I made recourse to alkalies. I put a half ounce of this blue in a flask, and I poured on it ten ounces of a solution of nitre fixed by tartar ] (''nitre'') which is mixed with crude ] and then ignited, producing potassium carbonate]. As soon as these two substances had been mixed together, I saw with astonishment that, without the aid of heat, the blue color had entirely disappeared; the powder at the bottom of the flask had only a rather gray color: having put this vessel on a ] in order to heat the solution until it simmered, this gray color also disappeared entirely, and all that was contained in the flask, both the powder and the solution, had only a yellow color a little red.)</ref><ref>{{cite journal |last1=Munroe |first1=Charles E. |last2=Chatard |first2=Thomas M. |title=Manufactures: Chemicals and Allied Products |journal=Twelfth Census of the United States: Bulletins |date=1902 |issue=210 |pages=1–306 |url=https://books.google.com/books?id=8UIUAQAAMAAJ&pg=RA1-PA31}}; see p. 31.</ref>
			===Modern production===
	:H<sub>4</sub> + KOH → K<sub>4</sub>•3H<sub>2</sub>O<ref name="Wageningen">{{cite web |url= http://www.food-info.net/uk/e/e536.htm |title=Food-Info |author=Wageningen University |date=2009-02-24 |accessdate=2009-04-30 |work=}}</ref>
			Potassium hexacyanidoferrate(II) is produced industrially from ], ], and ], the combination of which affords Ca<sub>2</sub>·11H<sub>2</sub>O. This solution is then treated with potassium salts to precipitate the mixed calcium-potassium salt CaK<sub>2</sub>, which in turn is treated with ] to give the tetrapotassium salt.<ref name=Ullmann>{{ cite encyclopedia |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 | encyclopedia = Ullmann's Encyclopedia of Industrial Chemistry |date=October 2011 | publisher = Wiley-VCH | location = Weinheim | doi = 10.1002/14356007.a08_159.pub3 |isbn=978-3527306732 }}</ref>
			===Historical production===
	The reaction forms a stable compound that is neither combustible nor ].<ref name="JTBaker">{{cite web |url=http://hazard.com/msds/mf/baker/baker/files/p5763.htm |title=Potassium ferrocyanide MSDS |author=JT Baker, Inc. |date=2006-02-13 |accessdate=2009-04-30 |work=}}</ref> This compound is a strong reducing agent and is thus incompatible with oxidizing agents.<ref>{{cite web |url=http://pubs.acs.org/doi/abs/10.1021/ac50094a018 |title=Employment of Potassium Ferrocyanide in Standardization of Dilute Potassium Permanganate |author=Edwin J. deBeer, Axel M. Hjort |date=1935-03 |accessdate=2009-04-30 |format= |work=}}</ref> Addition of ], ], ], or ] to a solution of carefully prepared and otherwise stable potassium ferrocyanide may result in a large explosion.<ref name="JTBaker" />
			Historically, the compound was manufactured from nitrogenous organic material, iron filings, and potassium carbonate.<ref name=Wagner>{{cite book|last=Von Wagner|first=Rudolf|title=Manual of chemical technology|year=1897|publisher=D. Appleton & Co.|location=New York|page=474 & 477|url=https://archive.org/details/manualofchemical00wagnuoft}}</ref> Common ] and ] sources were ] horn, leather scrap, ], or dried blood. It was also obtained commercially from gasworks spent oxide (purification of city gas from hydrogen cyanide).
	== Properties ==		==Chemical reactions==
			Treatment of potassium hexacyanidoferrate(II) with ] gives H<sub>2</sub>. After neutralization of this intermediate with ], red crystals of ] can be selectively crystallized.<ref>{{cite encyclopedia | author = Seel, F. | title = Sodium nitrosyl cyanoferrate | encyclopedia = Handbook of Preparative Inorganic Chemistry | edition = 2nd | editor = Brauer, G. | publisher = Academic Press | year = 1965 | location = New York | volume = 2 | page = 1768 | lccn = 63-14307 | url = https://www.scribd.com/doc/27443280/Handbook-of-Preparative-Inorganic-Chemistry-Vol-2-2d-Ed-George-Brauer | access-date = 2017-09-10 | archive-date = 2010-03-07 | archive-url = https://web.archive.org/web/20100307011411/http://www.scribd.com/doc/27443280/Handbook-of-Preparative-Inorganic-Chemistry-Vol-2-2d-Ed-George-Brauer | url-status = dead }}</ref>
	===Physical characteristics===
			Upon treatment with ] gas, potassium hexacyanidoferrate(II) converts to ]:
	Although it is insoluble in ], a liter of water can dissolve just under three hundred ]s of the crystals, and the solution can react with acid to release toxic ] (HCN) gas. The resulting HCN gas boils at 26 °] and, being ] (with a gaseous density of 0.94), quickly ] clear of the release point.
			:2 K<sub>4</sub> + Cl<sub>2</sub> → 2 K<sub>3</sub> + 2 KCl
			This reaction can be used to remove potassium hexacyanidoferrate(II) from a solution.{{citation needed|date=April 2012}}
			A famous reaction involves treatment with ferric salts, most commonly ], to give ]. In the reaction with Iron(III) chloride, producing ] as a side-product:
	=== Chemical reactions ===
			3 K<sub>4</sub> + 4 FeCl<sub>3</sub> → Fe<sub>4</sub><sub>3</sub> + 12 KCl
	When ] gas is bubbled through a solution of this compound, ] is formed in the reaction:
			With the composition Fe{{su|p=III|b=4}}]){{su|b=6}}]{{su|b=3}}, this insoluble but deeply coloured material is the blue of ]ing, as well as on many famous paintings such as ] and ].
	:2 K<sub>4</sub> + Cl<sub>2</sub> → 2 K<sub>3</sub> + 2 KCl<ref>{{cite web |url=http://ntp.niehs.nih.gov/ntp/htdocs/Chem_Background/ExSumPdf/PotassiumFerriCyanide.pdf | title=Summary of Data for Chemical Selection |author=NIH |date= |accessdate=2009-04-30 |format= |work=}}</ref>
			==Applications==
	This reaction can be used to remove potassium ferrocyanide from a solution.<ref>{{cite web |url=http://www.jbc.org/cgi/content/citation/240/11/4264 | title=Deamino-oxytocin. Its Isolation by Partition Chromatography on Sephadex and Crystallization from Water, and its Biological Activities. |author=Barbara M. Ferrier, Derek Jarvis, and Vincent Du Vigneaud |date=1965-11 |accessdate=2009-04-30 |format= |work=}}</ref> When the two are combined, the product is ]. Potassium ferrocyanide, potassium ferricyanide, and Prussian blue account for over 97% of cyanides in the environment.<ref name="YuXZ">{{cite journal |author=Yu XZ, Gu JD, Li TP |title=Availability of ferrocyanide and ferricyanide complexes as a nitrogen source to cyanogenic plants |journal=Archives of Environmental Contamination and Toxicology |volume=55 |issue=2 |pages=229–37 |year=2008 |month=August |pmid=18180862 |doi=10.1007/s00244-007-9101-6}}</ref>
			Potassium hexacyanidoferrate(II) finds many niche applications in industry. It and ] are widely used as anticaking agents for both road salt and table salt. The potassium and sodium hexacyanidoferrates(II) are also used in the purification of tin and the separation of copper from molybdenum ores. Potassium hexacyanidoferrate(II) is used in the production of wine and citric acid.<ref name=Ullmann/>
			In the EU, hexacyanidoferrates(II) (E 535–538) were, as of 2017, solely authorised in two food categories as salt additives.
	Potassium ferrocyanide is also used to test for protein. ] and {{chem|K|3|Fe(CN)|6}} are added to an aqueous solution of the substance being tested. The formation of a white precipitate confirms the presence of protein.<ref>{{cite book
	| title = Methods of Organic Analysis
	| first1 = Henry Clapp
	| last1 = Sherman
	| publisher = READ BOOKS
	| year = 2007
	| page = 313
	| isbn = 1408628023
	}}</ref>
			It can also be used in animal feed.<ref>{{cite web |title=EuSalt Expert Meeting on E 535 and E 536 as Feed Additives |url=https://eusalt.com/events/eusalt-expert-meeting-e-535-and-e-536-feed-additives |publisher=EUSalt |access-date=2018-12-06 |archive-date=2019-05-12 |archive-url=https://web.archive.org/web/20190512013808/https://eusalt.com/events/eusalt-expert-meeting-e-535-and-e-536-feed-additives |url-status=dead }}</ref>
	===Toxicity===
			In the laboratory, potassium hexacyanidoferrate(II) is used to determine the concentration of ], a compound often used in ]s based on ] reactions. Potassium hexacyanidoferrate(II) is used in a mixture with potassium ferricyanide and phosphate buffered solution to provide a buffer for ], which is used to cleave ], giving a bright blue visualization where an antibody (or other molecule), conjugated to Beta-gal, has bonded to its target. On reacting with Fe(3) it gives a Prussian blue colour. Thus it is used as an identifying reagent for iron in labs.
	Potassium ferrocyanide itself is only slightly toxic,<ref name="JTBaker" /> although adding acid to its aqueous solution releases toxic hydrogen cyanide gas. While it is not ], it may cause irritation if it is ingested, inhaled, or if it comes into contact with skin.<ref>{{cite journal |author=Nishioka H |title=Mutagenic activities of metal compounds in bacteria |journal=Mutation Research |volume=31 |issue=3 |pages=185–9 |year=1975 |month=June |pmid=805366}}</ref> The best solution in these situations is to remove the victim to fresh air or wash the affected area thoroughly with water. It causes harm in aqueous environments and is especially toxic to aquatic organisms. The ] (LD50) in rats is 6400&nbsp;mg/kg.<ref name="JTBaker" />
			Potassium hexacyanidoferrate(II) can be used as a fertilizer for plants.{{citation needed|date=April 2012}}
	== Uses ==
	* Naturally, potassium ferrocyanide can be used as an alternate ] source for plants. It is often used as a gardening technique.<ref name="MelindaH">{{cite news |url=http://www.nytimes.com/2002/02/21/world/a-nation-challenged-suspects-4-arrested-in-plot-against-us-embassy-in-rome.html?n=Top/Reference/Times%20Topics/People/H/Henneberger,%20Melinda|title=A NATION CHALLENGED: SUSPECTS; 4 Arrested in Plot Against U.S. Embassy in Rome |author=Melinda Henneberger |date=2002-02-21 |accessdate=2009-04-30 |format= |work=The New York Times}}</ref> In an experiment to test this aim, plants were either deprived of nitrogen or given a nitrogen-rich environment while all were exposed to either potassium ferrocyanide or its product, potassium ferricyanide. The plants were unable to sustain themselves solely on the cyanides, but the uptake of the cyanides did increase in the absence of nitrogen. Furthermore, the plants appeared to have different methods for the uptake of the two cyanides.<ref name="YuXZ" />
			Prior to 1900, before the invention of the ], potassium hexacyanidoferrate(II) was the most important source of ] ].<ref name=Ullmann /> In this historical process, ] was produced by decomposing potassium hexacyanidoferrate(II):<ref name=Wagner />
	* Industrially, this complex is used in metal extraction and to make adhesives, computer electronics, fire retardants, cosmetics, dyes, nylon, paints, inks, plexiglass, pharmaceuticals, and rocket propellant.<ref name="YuXZ" /> It is also used in low doses in some food preparation. It works as an anti-caking agent and it removes copper from red wine, as copper is used as a fungicide on grapes.<ref name="Wageningen" />
			K<sub>4</sub> → 4 KCN + FeC<sub>2</sub> + N<sub>2</sub>
	* In the laboratory, potassium ferrocyanide is used to determine the concentration of ], a compound often used in ]s based on ]reactions.
	== History ==		==Structure==
			Like other metal cyanides, solid potassium hexacyanidoferrate(II), both as the hydrate and anhydrous salts, has a complicated polymeric structure. The polymer consists of octahedral <sup>4−</sup> centers crosslinked with K<sup>+</sup> ions that are bound to the CN ]s.<ref>{{Cite journal |last1=Willans |first1=Mathew J. |last2=Wasylishen |first2=Roderick E. |last3=McDonald |first3=Robert |date=2009-05-18 |title=Polymorphism of Potassium Ferrocyanide Trihydrate as Studied by Solid-State Multinuclear NMR Spectroscopy and X-ray Diffraction |url=https://pubs.acs.org/doi/10.1021/ic802134j |journal=Inorganic Chemistry |language=en |volume=48 |issue=10 |pages=4342–4353 |doi=10.1021/ic802134j |pmid=19425611 |issn=0020-1669}}</ref> The K<sup>+</sup>---NC linkages break when the solid is dissolved in water.{{clarify|date=May 2020}}{{citation needed|date=May 2020}}
	This specific cyanide was part of an alleged terrorist attempt in ]. On February 21, 2002 four ] Nationalists were arrested with nine pounds of potassium ferrocyanide and a map pinpointing the exact water pipes leading to the ] Embassy in ]. The presumed plan was that the cyanide would be dumped into the water to poison the Embassy. Whether or not the men were planning an attack, the potassium ferrocyanide mixed with the water would not have been enough to make it toxic. As aforementioned, it is only extremely toxic when mixed with strong acids due to the resulting ].<ref name="MelindaH" />
	== See also ==		===Toxicity===
			The toxicity in rats is low, with ] (LD<sub>50</sub>) at 6400&nbsp;mg/kg.<ref name=JTBaker>{{cite web | url = http://hazard.com/msds/mf/baker/baker/files/p5763.htm | title = POTASSIUM FERROCYANIDE MSDS Number: P5763 - Effective Date: 12/08/96 | publisher = J. T. Baker Inc. | access-date = 2012-04-08 | url-status = dead | archive-date = 2015-11-21 | archive-url = https://web.archive.org/web/20151121093949/http://hazard.com/msds/mf/baker/baker/files/p5763.htm }}</ref>{{Better source needed|date=July 2024}} The kidneys are the organ for ferrocyanide toxicity.<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>
			==See also==
	*]		*]
			*]<ref>{{Cite journal |last1=Kosugi |first1=Nobuhiro |last2=Yokoyama |first2=Toshihiko |last3=Kuroda |first3=Haruo |date=May 1986 |title=Polarization dependence of XANES of square-planar Ni(CN)2−4 ion. A comparison with octahedral Fe(CN)4−6 and Fe(CN)3−6 ions |url=http://dx.doi.org/10.1016/0301-0104(86)85034-0 |journal=Chemical Physics |volume=104 |issue=3 |pages=449–453 |doi=10.1016/0301-0104(86)85034-0 |issn=0301-0104}}</ref>
	*]
	*]		*]
	== References ==		==References==
	{{Reflist}}		{{Reflist}}
	==External links==		==External links==
	*		* {{ cite web | url = http://www.npi.gov.au/substances/cyanide/index.html | publisher = National Pollutant Inventory Australia | title = Cyanide (inorganic) compounds fact sheet }}
			* {{cite web | url = http://blogs.rediff.com/thinko/2019/07/31/customers-can-rely-on-tata-salt-as-report-says-it-is-safe-to-consume/ | work = rediff.com | title = Potassium Ferrocyanide in Salt Is Entirely Safe To Consume }}{{Dead link|date=October 2022 |bot=InternetArchiveBot |fix-attempted=yes }}
	{{Potassium compounds}}		{{Potassium compounds}}
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	{{DEFAULTSORT:Potassium Ferrocyanide}}		{{DEFAULTSORT:Potassium Ferrocyanide}}
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