View source for Chemistry:Potassium acetate

{{Short description|Colourless soluble salt of acetic acid}}
{{chembox
| Verifiedfields = changed
| Watchedfields  = changed
| verifiedrevid  = 404348953
| Name           = Potassium acetate
| ImageFile      = Potassium_acetate skeletal.png
| ImageFileL1    = Acetate-anion-3D-balls.png
| ImageFileR1    = Potassium-3D.png
| ImageSize      = 120px
| ImageName      = Skeletal formula of potassium acetate
| PIN            = Potassium acetate
| OtherNames     = Potassium ethanoate,  E261
| Section1       = {{Chembox Identifiers
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo = 127-08-2
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = M911911U02
| ChEMBL_Ref = {{ebicite|changed|EBI}}
| ChEMBL = 1201058
| PubChem = 31371
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| ChemSpiderID = 29104
| SMILES = CC(=O)[O-].[K+]
| InChI = 1/C2H4O2.K/c1-2(3)4;/h1H3,(H,3,4);/q;+1/p-1
| InChIKey = SCVFZCLFOSHCOH-REWHXWOFAA
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| StdInChI = 1S/C2H4O2.K/c1-2(3)4;/h1H3,(H,3,4);/q;+1/p-1
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| StdInChIKey = SCVFZCLFOSHCOH-UHFFFAOYSA-M
  }}
| Section2       = {{Chembox Properties
| C=2 | H=3 | O=2 | K=1
| Appearance = White deliquescent crystalline powder
| Density = 1.8{{nbsp}}g/cm<sup>3</sup> (20{{nbsp}}°C)<ref name=chemister /><br /> 1.57{{nbsp}}g/cm<sup>3</sup> (25{{nbsp}}°C)
| Solubility = 216.7{{nbsp}}g/100{{nbsp}}mL (0.1{{nbsp}}°C)<br /> 233.8{{nbsp}}g/100{{nbsp}}mL (10{{nbsp}}°C)<br /> 268.6{{nbsp}}g/100{{nbsp}}mL (25{{nbsp}}°C)<br /> 320.8{{nbsp}}g/100{{nbsp}}mL (40{{nbsp}}°C)<br /> 390.7{{nbsp}}g/100{{nbsp}}mL (96{{nbsp}}°C)<ref name=sioc>{{cite book|last1 = Seidell|first1 = Atherton|last2 = Linke|first2 = William F.|year = 1952|title = Solubilities of Inorganic and Organic Compounds|publisher = Van Nostrand}}</ref>
| SolubleOther = Soluble in [[Chemistry:Ethanol|alcohol]], liquid [[Chemistry:Ammonia|ammonia]]<br /> Insoluble in [[Chemistry:Diethyl ether|ether]], [[Chemistry:Acetone|acetone]]
| Solubility1 = 24.24{{nbsp}}g/100{{nbsp}}g (15{{nbsp}}°C)<br /> 53.54{{nbsp}}g/100{{nbsp}}g (73.4{{nbsp}}°C)<ref name=chemister />
| Solvent1 = methanol
| Solubility2 = 16.3{{nbsp}}g/100{{nbsp}}g<ref name=chemister/>
| Solvent2 = ethanol
| Solubility3 = 0.06{{nbsp}}g/kg (0{{nbsp}}°C)<ref name=chemister/>
| Solvent3 = sulfur dioxide
| MeltingPtC = 292
| BoilingPt = Decomposes
| pKa = 4.76
  }}
| Section3       = {{Chembox Structure
| CrystalStruct = Monoclinic
  }}
| Section4       = 
| Section5       = {{Chembox Thermochemistry
| DeltaHf = −722.6{{nbsp}}kJ/mol<ref name=chemister>{{Cite web|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=504|title=Potassium acetate}}</ref>
| HeatCapacity = 109.38{{nbsp}}J/mol·K<ref name=nist>{{nist|name=Acetic acid, potassium salt|id=C127082|accessdate=2014-05-18|mask=FFFF|units=SI}}</ref>
| DeltaGf = 
| Entropy = 150.82{{nbsp}}J/mol·K<ref name=nist />
}}
| Section6       = {{Chembox Pharmacology
| ATCCode_prefix = B05
| ATCCode_suffix = XA17
}}
| Section7       = {{Chembox Hazards
| NFPA-H = 1
| NFPA-F = 1
| NFPA-R = 0
| LD50 = 3250{{nbsp}}mg/kg (oral, rat)<ref>https://chem.nlm.nih.gov/chemidplus/rn/127-08-2 </ref>
  }}
}}
'''Potassium acetate''' (also called '''potassium ethanoate'''), (CH<sub>3</sub>COOK) is the [[Chemistry:Potassium|potassium]] [[Chemistry:Salt|salt]] of [[Chemistry:Acetic acid|acetic acid]]. It is a [[Biology:Hygroscopy|hygroscopic]] solid at room temperature.

==Preparation==
It can be prepared by treating a potassium-containing base such as [[Chemistry:Potassium hydroxide|potassium hydroxide]] or [[Chemistry:Potassium carbonate|potassium carbonate]] with [[Chemistry:Acetic acid|acetic acid]]:

:CH<sub>3</sub>COOH + KOH → CH<sub>3</sub>COOK + H<sub>2</sub>O
This sort of reaction is known as an acid-base neutralization reaction.

The sesquihydrate in water solution (CH<sub>3</sub>COOK·1½H<sub>2</sub>O) begins to form semihydrate at 41.3&nbsp;°C.<ref name=sioc/>

==Applications==

===Deicing===
Potassium acetate (as a substitute for [[Chemistry:Calcium chloride|calcium chloride]] or [[Chemistry:Magnesium chloride|magnesium chloride]]) can be used as a [[Chemistry:Deicing|deicer]] to remove ice or prevent its formation. It offers the advantage of being less aggressive on soils and much less corrosive:<ref>{{cite journal |last1=Gruber |first1=Michael R. |last2=Hofko |first2=Bernhard |last3=Hoffmann |first3=Markus |last4=Stinglmayr |first4=David |last5=Seifried |first5=Teresa M. |last6=Grothe |first6=Hinrich |title=Deicing performance of common deicing agents for winter maintenance with and without corrosion-inhibiting substances |journal=Cold Regions Science and Technology |date=April 2023 |volume=208 |pages=103795 |doi=10.1016/j.coldregions.2023.103795|doi-access=free }}</ref> for this reason, it is preferred for airport runways although it is more expensive.<ref>{{cite book |last1=Harrington-Hughes |first1=Kathryn |title=Handbook of test methods for evaluating chemical deicers. |date=1992 |publisher=Transportation Research Board |isbn=9789994805839}}</ref>

===Fire extinguishing===
Potassium acetate is the extinguishing agent used in [[Engineering:Fire extinguisher#United States|Class K]] [[Engineering:Fire extinguisher|fire extinguisher]]s because of its ability to cool and form a crust over burning oils.

===Food additive===
Potassium acetate is used in processed foods as a [[Chemistry:Preservative|preservative]] and acidity regulator.  In the European Union, it is labeled by the [[Chemistry:E number|E number]] E261;<ref>UK Food Standards Agency: {{cite web |url=http://www.food.gov.uk/safereating/chemsafe/additivesbranch/enumberlist |title=Current EU approved additives and their E Numbers |access-date=2011-10-27}}</ref> it is also approved for usage in the USA,<ref>US Food and Drug Administration: {{cite web |url=https://www.fda.gov/Food/FoodIngredientsPackaging/FoodAdditives/ucm191033.htm#ftnT |title=Listing of Food Additives Status Part II |website=[[Organization:Food and Drug Administration|Food and Drug Administration]] |access-date=2011-10-27}}</ref> Australia, and New Zealand.<ref>Australia New Zealand Food Standards Code{{cite web |url=http://www.comlaw.gov.au/Details/F2011C00827 |title=Standard 1.2.4 - Labelling of ingredients |access-date=2011-10-27}}</ref> Potassium hydrogen diacetate (CAS #{{CAS|4251-29-0}}) with formula KH(OOCCH<sub>3</sub>)<sub>2</sub> is a related food additive with the same E number as potassium acetate.

===Medicine and biochemistry===
In medicine, potassium acetate is used as part of electrolyte replacement protocols in the treatment of [[Medicine:Diabetic ketoacidosis|diabetic ketoacidosis]] because of its ability to break down to [[Chemistry:Bicarbonate|bicarbonate]] to help neutralize the acidotic state.

In [[Biology:Molecular biology|molecular biology]], potassium acetate is used to precipitate [[Chemistry:Sodium dodecyl sulfate|dodecyl sulfate]] (DS) and DS-bound proteins to extract ethanol from DNA.

Potassium acetate is used in mixtures applied for tissue preservation, fixation, and mummification. Most museums today use a [[Physics:Formaldehyde|formaldehyde]]-based method recommended by Kaiserling in 1897 which contains potassium acetate.<ref>{{cite journal | url = https://www.uqtr.ca/plast-journal/vol8/Ulmer_7a10.pdf | author = Dale Ulmer | title = Fixation. The Key to Good Tissue Preservation | journal = Journal of the International Society for Plastination | volume = 8 | issue = 1 | pages = 7–10 | date = 1994 | access-date = 2017-09-08 | archive-url = https://web.archive.org/web/20110516150018/http://www.uqtr.ca/plast-journal/vol8/Ulmer_7a10.pdf | archive-date = 2011-05-16 | url-status = dead }}</ref> This process was used to soak Lenin's corpse.<ref>{{Cite book | author = Andrew Nagorski | title = The Greatest Battle | publisher = Simon and Schuster | date = 2007 | page = 53}}</ref>

===Use in executions===

Potassium acetate was incorrectly used in place of [[Chemistry:Potassium chloride|potassium chloride]] when [[Social:Capital punishment|putting a prisoner to death]] in Oklahoma in January 2015.<ref>{{cite news|title=Oklahoma used wrong drug in Charles Warner's execution, autopsy report says|url=https://www.theguardian.com/us-news/2015/oct/08/oklahoma-wrong-drug-execution-charles-warner}}</ref> Charles Frederick Warner was executed on January 15, 2015 with potassium acetate; this was not public knowledge until the scheduled execution of Richard Glossip was called off. <ref>{{cite news|url= https://www.npr.org/sections/thetwo-way/2015/10/08/446862121/oklahoma-used-the-wrong-drug-to-execute-charles-warner|title=Oklahoma Used The Wrong Drug To Execute Charles Warner|author=Eyder Peralta|publisher=NPR}}</ref> In August 2017, the U.S. state of Florida executed Mark James Asay using a combination of [[Chemistry:Etomidate|etomidate]], [[Chemistry:Rocuronium bromide|rocuronium bromide]], and potassium acetate.<ref>{{cite news|url=http://www.sun-sentinel.com/news/florida/fl-reg-florida-execution-asay-20170824-story.html|title=Florida executes convicted killer Mark Asay using new drug|author=Jason Dearon|publisher=Sun Sentinel}}</ref> The drug was also used in the February 2023 execution of Donald Dillbeck, once again in combination with etomidate and rocuronium bromide. <ref>{{cite news|url=https://www.tallahassee.com/story/news/2023/02/23/donald-dillbeck-florida-execution-latest-updates/69904871007/|title=Convicted murderer Donald Dillbeck has been executed. Here's the latest.|author=Kathryn Varn|publisher=Tallahassee Democrat}}</ref>

===Industry===
Potassium acetate is used as a [[Chemistry:Catalysis|catalyst]] in the production of [[Chemistry:Polyurethane|polyurethane]]s.<ref>Hosea Cheung, Robin S. Tanke, G. Paul Torrence "Acetic Acid" in ''Ullmann's Encyclopedia of Industrial Chemistry'', 2005 Wiley-VCH, Weinheim.  {{doi|10.1002/14356007.a01_045}}.</ref>

==Historical==
It is used as a [[Chemistry:Diuretic|diuretic]] and urinary alkalizer. Before modern chemistry, it was variously called ''terra foliata tartari'', ''sal Sennerti'', ''tartarus regeneratus,'' ''arcanum tartari'' and ''sal diureticus''.<ref>{{Cite book |last=Crosland |first=Maurice P. |url=https://books.google.com/books?id=kwQQaltqByAC&pg=PA104 |title=Historical Studies in the Language of Chemistry |date=2004-01-01 |publisher=Courier Corporation |isbn=978-0-486-43802-3 |language=en}}</ref> In 1760 it was used in the preparation of [[Chemistry:Cadet's fuming liquid|Cadet's fuming liquid]] ((CH<sub>3</sub>)<sub>2</sub>As)<sub>2</sub>O, the first organometallic compound ever produced.

==References==
{{reflist}}

==External links==

{{Potassium compounds}}
{{clear}}
{{Acetates}}


[[Category:Acetates]]
[[Category:Potassium compounds]]
[[Category:Lethal injection components]]
[[Category:E-number additives]]

{{Sourceattribution|Potassium acetate}}