Potassium acetate

Potassium acetate
Names
Preferred IUPAC name
Potassium acetate
Other names
Potassium ethanoate
Identifiers
3D model (JSmol)
ChEMBL
ChemSpider
ECHA InfoCard 100.004.385
E number E261 (preservatives)
UNII
  • InChI=1S/C2H4O2.K/c1-2(3)4;/h1H3,(H,3,4);/q;+1/p-1 N
    Key: SCVFZCLFOSHCOH-UHFFFAOYSA-M N
  • InChI=1/C2H4O2.K/c1-2(3)4;/h1H3,(H,3,4);/q;+1/p-1
    Key: SCVFZCLFOSHCOH-REWHXWOFAA
  • CC(=O)[O-].[K+]
Properties
CH3COOK
Molar mass 98.142 g·mol−1
Appearance White deliquescent crystalline powder
Density 1.57 g/cm3 (25 °C (77 °F; 298 K))[1]
Melting point 303–307 °C (577–585 °F; 576–580 K)[1]
Boiling point Decomposes
  • 216.7 g/100 mL (0.1 °C (32.2 °F; 273.2 K))
  • 233.7 g/100 mL (10 °C (50 °F; 283 K))
  • 268.6 g/100 mL (25 °C (77 °F; 298 K))
  • 320.8 g/100 mL (40 °C (104 °F; 313 K))
  • 390.7 g/100 mL (96 °C (205 °F; 369 K))[2]
Solubility in methanol
  • 24.24 g/100g (15 °C (59 °F; 288 K))
  • 53.54 g/100g (73.4 °C (164.1 °F; 346.5 K))[3]
Solubility in ethanol 16.3 g/100g[2]
Solubility in acetic acid 20.95 g/100g (28.03 °C (82.45 °F; 301.18 K))[3][4]
Solubility in dimethylformamide 0.09 g/100g[3]
Solubility in sulfur dioxide 0.006 g/100g (0 °C (32 °F; 273 K))[3]
Solubility in liquid ammonia 1.026 g/100g (−33.9 °C (−29.0 °F; 239.2 K))[3]
Vapor pressure < 0.0000001 hPa[1]
Acidity (pKa) 4.76
Structure
Monoclinic
Thermochemistry[5]
109.38 J/(mol × K)
150.82 J/(mol × K)
−722.6 kJ⋅mol−1[3]
Enthalpy of fusion (ΔfH⦵fus)
 22 kJ⋅mol−1[3]
Pharmacology
B05XA17 (WHO)
Hazards[6]
GHS labelling:
Warning
NFPA 704 (fire diamond)
1
1
1
Lethal dose or concentration (LD, LC):
3250 mg/kg (oral, rat)
Related compounds
Other anions
Other cations
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Potassium acetate (also called potassium ethanoate), (CH3COOK) is the potassium salt of acetic acid. It is a hygroscopic solid at room temperature.

Preparation

It can be prepared by treating a potassium-containing base such as potassium hydroxide with acetic acid:

CH3COOH + KOH → CH3COOK + H2O

This sort of reaction is known as an acid-alkalai reaction.

At saturation, the sesquihydrate in water solution (2CH3COOK·3H2O) begins to form the semihydrate (2CH3COOK·H2O) at 41.3 °C (106.3 °F).[2]

Applications

Deicing

Potassium acetate (as a substitute for calcium chloride or magnesium chloride) can be used as a deicer to remove ice or prevent its formation. It offers the advantages over chlorides of being less aggressive on soils and much less corrosive: for this reason, it is one of the preferred substances for removal of ice from airplanes and airport runways.[7][8]

Fire extinguishing

Potassium acetate is the extinguishing agent used as a component in some Class K fire extinguishers[9] because of its ability to cool and form a crust over burning oils.

Food additive

Potassium acetate is used in processed foods as a preservative and acidity regulator. In the European Union, it is labeled by the E number E261; it is also approved for usage in the USA, Australia, and New Zealand.[10][11][12]

Medicine and biochemistry

In molecular biology, potassium acetate is used to precipitate Sodium dodecyl sulfate (SDS) and SDS-bound proteins to allow their removal from DNA.

Potassium acetate is used in mixtures applied for tissue preservation, fixation, and mummification. Most museums today use a formaldehyde-based method recommended by Kaiserling in 1897 which contains potassium acetate.[13] This process was used to soak Lenin's corpse.[14]

Industry

Potassium acetate is used as a catalyst in the production of polyurethanes.[15]

Use in executions

Potassium acetate was incorrectly used in place of potassium chloride when putting a prisoner to death in Oklahoma in January 2015. 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.[16][17]

In August 2017, the U.S. state of Florida used potassium acetate (intentionally) in the execution of Mark James Asay.[18]

Historical

Potassium acetate is used as a diuretic and urinary alkalizer. Before modern chemistry, it was variously called terra foliata tartari, sal Sennerti, tartarus regeneratus, arcanum tartari and sal diureticus.[19] In 1760 it was used in the preparation of Cadet's fuming liquid ((CH3)2As)2 + ((CH3)2As)2O, the first organometallic compound ever produced.

References

  1. ^ a b c Sigma-Aldrich Co., Potassium acetate.
  2. ^ a b c Seidell, Atherton; Linke, William F. (1919). "Potassium - Potassium acetate". Solubilities of Inorganic and Organic Compounds (2nd ed.). New York: Van Nostrand. p. 500. Retrieved 31 October 2025.
  3. ^ a b c d e f g "Potassium acetate". chemister.ru. Chemister. Retrieved 31 October 2025.
  4. ^ Davidson, Arthur W.; McAllister, Walter H. (1 February 1930). "Solutions of salts in pure acetic acid. II. Solubilities of acetates". Journal of the American Chemical Society. 52 (2): 507–519. Bibcode:1930JAChS..52..507D. doi:10.1021/ja01365a010.
  5. ^ Acetic acid, potassium salt in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD) (retrieved 2014-05-18)
  6. ^ "SDS - Potassium acetate". fishersci.com. Thermo Fisher Scientific. Retrieved 31 October 2025.
  7. ^ Gruber, Michael R.; Hofko, Bernhard; Hoffmann, Markus; Stinglmayr, David; Seifried, Teresa M.; Grothe, Hinrich (April 2023). "Deicing performance of common deicing agents for winter maintenance with and without corrosion-inhibiting substances". Cold Regions Science and Technology. 208 103795. doi:10.1016/j.coldregions.2023.103795.
  8. ^ Chappelo, C.C.; McElroy, A.D.; Blackburn, R.R.; Darwin, D.; de Noyelles, F.G.; Locke, C.E. (1992). Handbook of test methods for evaluating chemical deicers (PDF). Washington, DC: Strategic Highway Research Program, National Research Council. p. 73. ISBN 9789994805839. SHRP-H-332.
  9. ^ "SDS - Class K liquid agent for extinguishers" (PDF). Amerex. May 2016. p. 2. Retrieved 31 October 2025.
  10. ^ "Current EU approved additives and their E Numbers". UK Food Standards Agency. Retrieved 2011-10-27.
  11. ^ "Listing of Food Additives Status Part II". Food and Drug Administration. US Food and Drug Administration. Archived from the original on January 8, 2010. Retrieved 2011-10-27.
  12. ^ "Standard 1.2.4 - Labelling of ingredients". Australia-New Zealand Food Standards Code. 8 September 2011. Retrieved 2025-06-14.
  13. ^ Dale Ulmer (1994). "Fixation. The Key to Good Tissue Preservation" (PDF). Journal of the International Society for Plastination. 8 (1): 7–10. doi:10.56507/OEVY7072. Archived from the original (PDF) on 2011-05-16. Retrieved 2017-09-08.
  14. ^ Nagorski, Andrew (18 September 2007). The Greatest Battle: Stalin, Hitler, and the Desperate Struggle for Moscow That Changed the Course of World War II (1st ed.). Simon and Schuster. p. 53. ISBN 978-0743281102.
  15. ^ Cheung, H.; Tanke, R. S.; Torrence, G. P. "Acetic Acid". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a01_045. ISBN 978-3-527-30673-2.
  16. ^ Gajanan, Mahita (8 October 2015). "Oklahoma used wrong drug in Charles Warner's execution, autopsy report says". The Guardian.
  17. ^ Peralta, Eyder (8 October 2015). "Oklahoma Used The Wrong Drug To Execute Charles Warner". NPR.
  18. ^ Dearon, Jason (3 June 2018) [24 August 2017]. "Florida executes convicted killer Mark Asay using new drug". Sun Sentinel.
  19. ^ Crosland, Maurice P. (2004-01-01). Historical Studies in the Language of Chemistry. Courier Corporation. ISBN 978-0-486-43802-3.
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