Potassium ferricyanide: Difference between revisions
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{{short description|Chemical compound}} |
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{{Distinguish|potassium ferrocyanide}} |
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{{redirect|Prussian red|pigment based on [[ferric oxide]]|Venetian red}} |
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{{chembox |
{{chembox |
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| Verifiedfields = changed |
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| verifiedrevid = 444993061 |
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| Watchedfields = changed |
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| Name = Potassium ferricyanide |
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| verifiedrevid = 451578816 |
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| ImageFile = Potassium ferricyanide crystals.jpg |
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| Name = Potassium ferricyanide |
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| ImageSize = 230px |
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| ImageFile = Potassium ferricyanide2.jpg |
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| ImageSize = |
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| ImageFile1 = Potassium-ferricyanide-sample.jpg |
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| ImageSize1 = |
| ImageSize1 = |
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| ImageFile1 = Structure of potassium ferricyanide.png |
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| ImageSize2 = |
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| IUPACName = Potassium hexacyanoferrate(III) |
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| ImageName2 = Crystals of potassium ferricyanide |
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| IUPACName = Potassium hexacyanoferrate(III) |
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| Section1 = {{Chembox Identifiers |
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| OtherNames = Red prussiate of Potash,<br/>Prussian red,<br/>Potassium ferricyanide |
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| Section1 = {{Chembox Identifiers |
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| CASNo = 13746-66-2 |
| CASNo = 13746-66-2 |
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| CASNo_Ref = {{cascite}} |
| CASNo_Ref = {{cascite|correct|CAS}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = U4MAF9C813 |
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| PubChem = 26250 |
| PubChem = 26250 |
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| RTECS = LJ8225000 |
| RTECS = LJ8225000 |
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| EC_number = 237-323-3 |
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| ChEBI = 30060 |
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| Gmelin = 21683 |
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| InChI = 1S/6CN.Fe.3K/c6*1-2;;;;/q6*-1;+3;3*+1 |
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| SMILES = [K+].[K+].N#C[Fe-3](C#N)(C#N)(C#N)(C#N)C#N.[K+] |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 24458 |
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| InChIKey = BYGOPQKDHGXNCD-UHFFFAOYAG |
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| StdInChI_Ref = {{stdinchicite|changed|chemspider}} |
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| StdInChI = 1S/6CN.Fe.3K/c6*1-2;;;;/q6*-1;+3;3*+1 |
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| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} |
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| StdInChIKey = BYGOPQKDHGXNCD-UHFFFAOYSA-N |
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}} |
}} |
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| Section2 = {{Chembox Properties |
| Section2 = {{Chembox Properties |
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| Formula = |
| Formula = K<sub>3</sub>[Fe(CN)<sub>6</sub>] |
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| MolarMass = 329.24 g/mol |
| MolarMass = 329.24 g/mol |
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| Appearance = deep red crystals |
| Appearance = deep red crystals, sometimes small pellets, orange to dark red powder |
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| Density = 1.89 g/cm<sup>3</sup>, solid |
| Density = 1.89 g/cm<sup>3</sup>, solid |
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| Solubility = 330 g/L ("cold water")<br />464 g/L (20°C)<br/>775 g/L ("hot water")<ref>Kwong, H.-L. |
| Solubility = 330 g/L ("cold water")<br />464 g/L (20 °C)<br/>775 g/L ("hot water")<ref>{{ cite encyclopedia | author = Kwong, H.-L. |title = Potassium Ferricyanide | encyclopedia = Encyclopedia of Reagents for Organic Synthesis | editor = Paquette, L. | year = 2004 | publisher = J. Wiley & Sons | location = New York | doi = 10.1002/047084289X| hdl = 10261/236866 |isbn = 9780471936237|url = https://hal.archives-ouvertes.fr/hal-02922790| hdl-access = free }}</ref> |
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| SolubleOther = slightly soluble in [[alcohol]] <br> soluble in [[acid]]<br />soluble in water |
| SolubleOther = slightly soluble in [[ethanol|alcohol]] <br> soluble in [[acid]]<br />soluble in water |
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| MeltingPtC = 300 |
| MeltingPtC = 300 |
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| BoilingPt = |
| BoilingPt = decomposes |
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| MagSus = +2290.0·10<sup>−6</sup> cm<sup>3</sup>/mol |
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}} |
}} |
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| Section3 = {{Chembox Structure |
| Section3 = {{Chembox Structure |
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| Coordination = [[octahedral]] at Fe |
| Coordination = [[octahedral]] at Fe |
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| CrystalStruct = [[monoclinic]] |
| CrystalStruct = [[monoclinic]] |
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}} |
}} |
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| Section7 = {{Chembox Hazards |
| Section7 = {{Chembox Hazards |
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| |
| ExternalSDS = [http://hazard.com/msds/mf/baker/baker/files/p5752.htm MSDS] |
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| MainHazards = |
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| EUIndex = Not listed |
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| |
| NFPA-F = 0 |
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| NFPA-H = 1 |
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| RPhrases = {{R20}}, {{R21}}, {{R22}}, {{R32}} |
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| NFPA-R = 0 |
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| SPhrases = {{S26}}, {{S36}} |
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| LD50 = 2970 mg/kg (mouse, oral) |
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| GHSPictograms = {{GHS07}} |
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| GHSSignalWord = Warning |
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| HPhrases = {{H-phrases|302|315|319|332|335}} |
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| PPhrases = {{P-phrases|261|264|270|271|280|301+312|302+352|304+312|304+340|305+351+338|312|321|330|332+313|337+313|362|403+233|405|501}} |
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| FlashPt = Non-flammable |
| FlashPt = Non-flammable |
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}} |
}} |
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| Section8 = {{Chembox Related |
| Section8 = {{Chembox Related |
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| OtherAnions = [[Potassium ferrocyanide]] |
| OtherAnions = [[Potassium ferrocyanide]] |
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| OtherCations = [[Prussian blue]] |
| OtherCations = [[Prussian blue]] |
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}} |
}} |
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}} |
}} |
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[[File:Красная кровяная соль растёртая.jpg|alt=Potassium ferricyanide milled|thumb|Potassium ferricyanide when milled has lighter color]] |
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'''Potassium ferricyanide''' is the [[chemical compound]] with the formula K<sub>3</sub>[Fe(CN)<sub>6</sub>]. This bright red salt contains the [[octahedral molecular geometry|octahedral]]ly [[coordination compound|coordinated]] [[ferricyanide|[Fe(CN)<sub>6</sub>]<sup>3−</sup>]] ion.<ref>{{ cite book | author = Sharpe, A. G. | title = The Chemistry of Cyano Complexes of the Transition Metals | publisher = Academic Press | location = London | year = 1976 }}</ref> It is soluble in water and its solution shows some green-yellow [[fluorescence]]. It was discovered in 1822 by [[Leopold Gmelin]].<ref>{{cite journal |last1=Gmelin |first1=Leopold |title=Ueber ein besonderes Cyaneisenkalium, and über eine neue Reihe von blausauren Eisensalzen |journal=Journal für Chemie und Physik |date=1822 |volume=34 |pages=325–346 |url=https://babel.hathitrust.org/cgi/pt?id=nyp.33433069069148&view=1up&seq=347 |trans-title=On a particular potassium iron cyanate, and on a new series of iron salts of cyanic acid |language=German}}</ref><ref>{{cite book|last1=Ihde|first1=A.J.|title=The Development of Modern Chemistry|date=1984|publisher=Dover Publications|location=New York|page=153|edition=2nd}}</ref> |
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'''Potassium ferricyanide''' is the [[chemical compound]] with the formula K<sub>3</sub>[Fe(CN)<sub>6</sub>]. This bright red salt contains the [[octahedral molecular geometry|octahedral]]ly [[coordination compound|coordinated]] [[ferricyanide|[Fe(CN)<sub>6</sub>]<sup>3−</sup>]] ion.<ref>Sharpe, A. G., The Chemistry of Cyano Complexes of the Transition Metals, Academic Press: London, 1976</ref> It is soluble in water and its solution shows some green-yellow [[fluorescence]]. |
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<div style="float:right;margin-left:0.5em;"> |
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<big>3 K<sup>+</sup></big> [[File:HexacyanidoferratIII 2.svg|175px]] |
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</div> |
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==Preparation== |
==Preparation== |
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Potassium ferricyanide is manufactured by passing [[chlorine]] through a [[solution]] of [[potassium ferrocyanide]]. Potassium ferricyanide separates from the solution: |
Potassium ferricyanide is manufactured by passing [[chlorine]] through a [[Solution (chemistry)|solution]] of [[potassium ferrocyanide]]. Potassium ferricyanide separates from the solution: |
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:2 K<sub>4</sub>[Fe(CN)<sub>6</sub>] + Cl<sub>2</sub> → 2 K<sub>3</sub>[Fe(CN)<sub>6</sub>] + 2 KCl |
:2 K<sub>4</sub>[Fe(CN)<sub>6</sub>] + Cl<sub>2</sub> → 2 K<sub>3</sub>[Fe(CN)<sub>6</sub>] + 2 KCl |
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==Structure== |
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Like other metal cyanides, solid potassium ferricyanide has a complicated polymeric structure. The polymer consists of octahedral [Fe(CN)<sub>6</sub>]<sup>3−</sup> centers crosslinked with K<sup>+</sup> ions that are bound to the CN [[ligand]]s.<ref>{{cite journal | doi=10.1098/rspa.1969.0031 | title=The crystallography and paramagnetic anisotropy of potassium ferricyanide | journal=Proceedings of the Royal Society of London. A. Mathematical and Physical Sciences | year=1969 | volume=309 | issue=1496 | pages=91–118 | bibcode=1969RSPSA.309...91F | last1=Figgis | first1=B. N. | last2=Gerloch | first2=M. | last3=Mason | first3=R. | s2cid=96689342 }}</ref> The K<sup>+</sup>---NCFe linkages break when the solid is dissolved in water. |
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==Applications== |
==Applications== |
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The compound is also used to [[case hardening|harden]] [[iron]] and [[steel]], in [[electroplating]], [[dye]]ing [[wool]], as a [[laboratory]] [[reagent]], and as a mild [[oxidizing agent]] in [[organic chemistry]]. |
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In 19th century, it was used for reading [[palimpsest]]s and old manuscripts.<ref>[http://www.skypoint.com/~waltzmn/ShortDefs.html#Chemicals Chemicals at the Encyclopedia of Textual Criticism]</ref> |
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===Photography=== |
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The compound has widespread use in [[blueprint]] drawing and in [[photography]] ([[Cyanotype]] process). [[Iron]] and [[copper]] [[Lightness (color)|toning]] involve the use of potassium ferricyanide. Potassium ferricyanide is used as an [[oxidizing agent]] to remove [[silver]] from negatives and positives, a process called dot etching. In [[color photography]], potassium ferricyanide is used to reduce the size of color dots without reducing their number, as a kind of manual color correction. The compound is also used to [[case hardening|harden]] [[iron]] and [[steel]], in [[electroplating]], [[dye]]ing [[wool]], as a [[laboratory]] [[reagent]], and as a mild [[oxidizing agent]] in [[organic chemistry]]. |
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==== Blueprint, cyanotype, toner ==== |
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It is also used in black-and-white photography with [[sodium thiosulfate]] (hypo)<ref>{{cite book|author1=Leslie Stroebel|author2=Richard D. Zakia|title=The Focal encyclopedia of photography|url=http://books.google.com/books?id=CU7-2ZLGFpYC&pg=PA297|accessdate=1 June 2011|year=1993|publisher=Focal Press|isbn=9780240514178|pages=297–}}</ref> to reduce the density of a [[Negative (photography)|negative]] or [[gelatin silver print]] where the mixture is known as Farmer's reducer; this can help offset problems from [[Exposure (photography)|overexposure]] of the negative, or brighten the highlights in the print. |
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The compound has widespread use in [[blueprint]] drawing and in [[photography]] ([[Cyanotype]] process). Several [[photographic print toning]] processes involve the use of potassium ferricyanide.It is often used as a mild bleach in a concentration of 10g/L to reduce film or print density. |
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==== Bleaching ==== |
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Potassium ferricyanide is also one of two compounds present in [[ferroxyl indicator solution]] (along with [[phenolphthalein]]) which turns blue ([[Prussian blue]]) in the presence of Fe<sup>2+</sup> ions, and which can therefore be used to detect metal oxidation that will lead to rust. It is possible to calculate the number of moles of Fe<sup>2+</sup> ions by using a [[colorimeter]], because of the very intense color of [[Prussian blue]] Fe<sub>4</sub>[Fe(CN)<sub>6</sub>]<sub>3</sub>. |
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Potassium ferricyanide was used as an [[oxidizing agent]] to remove [[silver]] from color negatives and positives during processing, a process called bleaching. Because potassium ferricyanide bleaches are environmentally unfriendly, short-lived, and capable of releasing hydrogen cyanide gas if mixed with high concentrations and volumes of acid, bleaches using ferric [[EDTA]] have been used in color processing since the 1972 introduction of the Kodak [[C-41 process]]. In [[color lithography]], potassium ferricyanide is used to reduce the size of color dots without reducing their number, as a kind of manual color correction called dot etching. |
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==== Farmer's reducer ==== |
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Ferricyanide is also used in black-and-white photography with [[sodium thiosulfate]] (hypo) to reduce the density of a [[Negative (photography)|negative]] or [[gelatin silver print]] where the mixture is known as Farmer's reducer; this can help offset problems from [[Exposure (photography)|overexposure]] of the negative, or brighten the highlights in the print.<ref>{{ cite encyclopedia | author1 = Stroebel, L. | author2 = Zakia, R. D. | title = Farmer's Reducer | encyclopedia = The Focal Encyclopedia of Photography | url = https://books.google.com/books?id=CU7-2ZLGFpYC&pg=PA297 | year = 1993 | publisher = Focal Press | isbn = 978-0-240-51417-8 | page = 297 }}</ref> |
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===Reagent in organic synthesis=== |
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Potassium ferricyanide is often used in physiology experiments as a means of increasing a solution's [[redox potential]] (E°' ~ 436 mV at pH 7). [[Sodium dithionite]] is usually used as a reducing chemical in such experiments (E°' ~ −420 mV at pH 7). |
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Potassium ferricyanide is a used as an oxidant in organic chemistry.<ref>{{cite journal|first1=E. A.|last1=Prill|first2=S. M.|last2=McElvain |doi=10.15227/orgsyn.015.0041|title=1-Methyl-2-Pyridone|journal=Organic Syntheses|year=1935|volume=15|page=41}}</ref><ref>{{cite journal |first1=Hendryk|last1=Würfel|first2= Dörthe|last2=Jakobi|doi=10.15227/orgsyn.095.0177|title=Syntheses of Substituted 2-Cyano-benzothiazoles|year=2018|journal=Organic Syntheses|volume=95|pages=177–191|doi-access=free}}</ref> It is an oxidant for catalyst regeneration in [[Sharpless dihydroxylation]]s.<ref>{{cite journal|first1=Javier|last1=Gonzalez|first2= Christine|last2=Aurigemma|first3=Larry|last3=Truesdale|doi=10.15227/orgsyn.079.0093|title= Synthesis of (+)-(1S,2R)- and (−)-(1R,2S)-''trans''-2-Phenylcyclohexanol via Sharpless Asymmetric Dihydroxylation (AD)|journal=Organic Syntheses|year=2002|volume=79|page=93}}</ref><ref>{{cite journal|first1=Ryu|last1=Oi|first2=K. Barry|last2=Sharpless |doi=10.15227/orgsyn.073.0001|title=3-[(1S)-1,2-Dihydroxyethyl]-1,5-Dihydro-3H-2,4-Benzodioxepine|journal=Organic Syntheses|year=1996|volume=73|page=1}}</ref> |
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===Sensors and indicators=== |
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Potassium ferricyanide is used in many amperometric [[biosensor]]s as an [[electron transfer]] agent replacing an enzyme's natural electron transfer agent such as [[oxygen]] as with the [[enzyme]] [[glucose oxidase]]. It is used as this ingredient in many commercially available blood [[glucose meter]]s for use by [[diabetics]]. |
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Potassium ferricyanide is also one of two compounds present in [[ferroxyl indicator solution]] (along with [[phenolphthalein]]) that turns blue ([[Prussian blue]]) in the presence of Fe<sup>2+</sup> ions, and which can therefore be used to detect metal oxidation that will lead to rust. It is possible to calculate the number of moles of Fe<sup>2+</sup> ions by using a [[Colorimeter (chemistry)|colorimeter]], because of the very intense color of [[Prussian blue]]. |
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In physiology experiments potassium ferricyanide provides a means increasing a solution's [[redox potential]] (E°' ~ 436 mV at pH 7). As such, it can oxidize reduced cytochrome c (E°' ~ 247 mV at pH 7) in isolated mitochondria. [[Sodium dithionite]] is usually used as a reducing chemical in such experiments (E°' ~ −420 mV at pH 7). |
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Potassium ferricyanide is the main component of Murakami's etchant for cemented carbides. |
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Potassium ferricyanide is used to determine the ferric reducing power potential of a sample (extract, chemical compound, etc.).<ref>Nakajima, Y., Sato, Y., & Konishi, T. (2007). Antioxidant Small Phenolic Ingredients in |
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==Prussian blue== |
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Inonotus obliquus (persoon) Pilat (Chaga). Chemical & Pharmaceutical Bulletin, 55(8), 1222–1276.</ref> Such a measurement is used to determine of the [[antioxidant]] property of a sample. |
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[[Prussian blue]], the deep blue pigment in blue printing, is generated by the reaction of K<sub>3</sub>[Fe(CN)<sub>6</sub>] with ferrous (Fe<sup>2+</sup>) ions.<ref>Dunbar, K. R.; Heintz, R. A., "Chemistry of Transition Metal Cyanide Compounds: Modern Perspectives", Progress in Inorganic Chemistry, 1997, volume 45, pp. 283–391 {{doi|10.1002/9780470166468.ch4}}.</ref> |
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Potassium ferricyanide is a component of amperometric [[biosensor]]s as an [[electron transfer]] agent replacing an enzyme's natural electron transfer agent such as [[oxygen]] as with the [[enzyme]] [[glucose oxidase]]. It is an ingredient in commercially available blood [[glucose meter]]s for use by [[diabetics]]. |
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In [[histology]], potassium ferricyanide is used to detect ferrous iron in biological tissue, as the stain [[Perls' Prussian blue]]. In this reaction, potassium ferricyanide reacts with ferrous iron in acidic solution to produce an insoluble blue pigment, and both the stain and the pigment are commonly referred to as [[Prussian blue|Turnbull's blue]]. To detect ferric (Fe<sup>3+</sup>) iron, potassium ''ferrocyanide'' is used instead; the stain and pigment produced are commonly known as Prussian blue.<ref>Carson, Freida L. (1997). ''Histotechnology: A Self-Instructional Text'' (2nd ed.), pp. 209–211. Chicago: American Society of Clinical Pathologists. ISBN 0-89189-411-X.</ref> It has been found that the compound formed in the Turnbull's blue reaction and the compound formed in the Prussian blue reaction are the same unique compound, [[Prussian blue]].<ref>{{cite journal|doi=10.3390/i4060362|author=Tafesse, F. |year=2003|url=http://www.mdpi.org/ijms/papers/i4060362.pdf|title= Comparative studies on Prussian blue or diaquatetraamine-cobalt(III) promoted hydrolysis of 4-nitrophenylphosphate in microemulsions|journal=International Journal of Molecular Sciences|volume=4|issue=6|pages=362–370}}</ref><ref>{{cite journal|author=Verdaguer, M., Galvez, N., Garde, R., and Desplanches, C. |year=2002|title= Electrons at work in Prussian blue analogues|journal=Electrochemical Society Interface|volume=11|issue=3|pages=28–32|doi=10.1002/chin.200304218|url=http://www.electrochem.org/dl/interface/fal/fal02/IF8-02-Pages28-32.pdf}}</ref> |
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== |
===Other=== |
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Potassium ferricyanide is combined with [[potassium hydroxide]] (or [[sodium hydroxide]] as a substitute) and water to formulate Murakami's etchant. This etchant is used by metallographers to provide contrast between binder and carbide phases in cemented carbides. |
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==Prussian blue== |
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Potassium ferricyanide has very low toxicity, its main hazard being that it is a mild irritant to the eyes and skin. However, under very strongly acidic conditions, highly toxic [[hydrogen cyanide]] gas is evolved, according to the equation: |
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[[Prussian blue]], the deep blue pigment in blue printing, is generated by the reaction of K<sub>3</sub>[Fe(CN)<sub>6</sub>] with ferrous (Fe<sup>2+</sup>) ions as well as K<sub>4</sub>[Fe(CN)<sub>6</sub>] with ferric salts.<ref>{{ cite book |author1=Dunbar, K. R. |author2=Heintz, R. A. | chapter = Chemistry of Transition Metal Cyanide Compounds: Modern Perspectives | title = Progress in Inorganic Chemistry | year = 1997 | volume = 45 | pages = 283–391 | doi = 10.1002/9780470166468.ch4 |series=Progress in Inorganic Chemistry |isbn=9780470166468 }}</ref> |
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In [[histology]], potassium ferricyanide is used to detect ferrous iron in biological tissue. Potassium ferricyanide reacts with ferrous iron in acidic solution to produce the insoluble blue pigment, commonly referred to as Turnbull's blue or [[Prussian blue]]. To detect ferric (Fe<sup>3+</sup>) iron, potassium ''ferrocyanide'' is used instead in the [[Perls' Prussian blue]] staining method.<ref>{{ cite book | author = Carson, F. L. | year = 1997 | title = Histotechnology: A Self-Instructional Text | edition = 2nd | pages = 209–211 | location = Chicago | publisher = American Society of Clinical Pathologists | isbn = 978-0-89189-411-7 }}</ref> The material formed in the Turnbull's blue reaction and the compound formed in the Prussian blue reaction are the same.<ref>{{ cite journal | author = Tafesse, F. | title = Comparative Studies on Prussian Blue or Diaquatetraamine-Cobalt(III) Promoted Hydrolysis of 4-Nitrophenylphosphate in Microemulsions | journal = International Journal of Molecular Sciences | year = 2003 | volume = 4 | issue = 6 | pages = 362–370 | doi = 10.3390/i4060362 | url = http://www.mdpi.org/ijms/papers/i4060362.pdf | doi-access = free }}</ref><ref>{{ cite journal |author1=Verdaguer, M. |author2=Galvez, N. |author3=Garde, R. |author4=Desplanches, C. | title = Electrons at Work in Prussian Blue Analogues | journal = Electrochemical Society Interface | year = 2002 | volume = 11 | issue = 3 | pages = 28–32 | doi = 10.1002/chin.200304218 | url = http://www.electrochem.org/dl/interface/fal/fal02/IF8-02-Pages28-32.pdf }}</ref> |
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:6 H<sup>+</sup> + [Fe(CN)<sub>6</sub>]<sup>3−</sup> → 6 HCN + Fe<sup>3+</sup><ref>[http://www.labchem.net/msds/75436.pdf MSDS for potassium ferricyanide]</ref> |
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==Safety== |
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The reaction with [[hydrochloric acid]] is as follows: |
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Potassium ferricyanide has low toxicity, its main hazard being that it is a mild irritant to the eyes and skin. However, under very strongly acidic conditions, highly toxic [[hydrogen cyanide]] gas is evolved, according to the equation: |
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:6 |
:6 H<sup>+</sup> + [Fe(CN)<sub>6</sub>]<sup>3−</sup> → 6 HCN + Fe<sup>3+</sup><ref>{{ cite web | url = http://www.labchem.com/tools/msds/msds/LC19040.pdf | title = MSDS for potassium ferricyanide }}</ref> |
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==See also== |
==See also== |
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==References== |
==References== |
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{{reflist |
{{reflist}} |
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== Further reading == |
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* [https://phadkeinstruments.com/study-of-ferricyanide-by-cyclic-voltammetry-using-phadkestat-20/ Studying redox reaction of Ferricyanide using Potentiostat] Effect of different parameters using [[Cyclic voltammetry|Cyclic Voltammetry]] |
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==External links== |
==External links== |
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*[http://www.inchem.org/documents/icsc/icsc/eics1132.htm International Chemical Safety Card 1132] |
*[http://www.inchem.org/documents/icsc/icsc/eics1132.htm International Chemical Safety Card 1132] |
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* [http://www.npi.gov.au/database/substance-info/profiles/29.html National Pollutant Inventory – Cyanide compounds fact sheet] |
* [https://web.archive.org/web/20060517035532/http://www.npi.gov.au/database/substance-info/profiles/29.html National Pollutant Inventory – Cyanide compounds fact sheet] |
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{{Potassium compounds}} |
{{Potassium compounds}} |
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{{DEFAULTSORT:Potassium Ferricyanide}} |
{{DEFAULTSORT:Potassium Ferricyanide}} |
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[[Category:Potassium compounds]] |
[[Category:Potassium compounds]] |
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[[Category:Iron compounds]] |
[[Category:Iron(III) compounds]] |
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[[Category: |
[[Category:Cyano complexes]] |
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[[Category: |
[[Category:Iron complexes]] |
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[[Category:Photographic chemicals]] |
[[Category:Photographic chemicals]] |
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[[Category:Oxidizing agents]] |
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[[ca:Ferricianur de potassi]] |
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[[cs:Hexakyanoželezitan draselný]] |
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[[de:Kaliumhexacyanidoferrat(III)]] |
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[[el:Σιδηρικυανιούχο κάλιο]] |
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[[es:Ferricianuro de potasio]] |
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[[fr:Ferricyanure de potassium]] |
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[[it:Ferricianuro di potassio]] |
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[[nl:Kaliumhexacyanoferraat(III)]] |
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[[ja:フェリシアン |
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[[pl:Żelazicyjanek potasu]] |
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[[pt:Ferricianeto de potássio]] |
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[[ru:Гексацианоферрат(III) калия]] |
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[[sk:Hexakyanoželezitan draselný]] |
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[[sv:Kaliumferricyanid]] |
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[[uk:Гексаціаноферат(III) калію]] |
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[[zh:铁氰 |