|Preferred IUPAC name
Potassium salt, E261
3D model (JSmol)
|E number||E261 (preservatives)|
CompTox Dashboard (EPA)
|Molar mass||98.142 g·mol−1|
|Appearance||White deliquescent crystalline powder|
|Density||1.8 g/cm3 (20 °C)|
1.57 g/cm3 (25 °C)
|Melting point||292 °C (558 °F; 565 K)|
|216.7 g/100 mL (0.1 °C)|
233.8 g/100 mL (10 °C)
268.6 g/100 mL (25 °C)
320.8 g/100 mL (40 °C)
390.7 g/100 mL (96 °C)
|Solubility||Soluble in alcohol, liquid ammonia|
Insoluble in ether, acetone
|Solubility in methanol||24.24 g/100 g (15 °C)|
53.54 g/100 g (73.4 °C)
|Solubility in ethanol||16.3 g/100 g|
|Solubility in sulfur dioxide||0.06 g/kg (0 °C)|
Heat capacity (C)
Std enthalpy of
|NFPA 704 (fire diamond)|
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|3250 mg/kg (oral, rat)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
what is ?)(
- CH3COOH + KOH → CH3COOK + H2O
This sort of reaction is known as an acid-base neutralization reaction.
The sesquihydrate in water solution (CH3COOK·1½H2O) begins to form semihydrate at 41.3 °C.
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 advantage of being less aggressive on soils and much less corrosive: for this reason, it is preferred for airport runways although it is more expensive.
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. Potassium hydrogen diacetate (CAS #4251-29-0 ) with formula KH(OOCCH3)2 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 diabetic ketoacidosis because of its ability to break down to bicarbonate to help neutralize the acidotic state.
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. This process was used to soak Lenin's corpse.
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.  In August 2017, the U.S. state of Florida executed Mark James Asay using a combination of etomidate, rocuronium bromide, and potassium acetate.
- "Potassium acetate".
- Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand.
- 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)
- http://chem.sis.nlm.nih.gov/chemidplus/rn/127-08-2[dead link]
- UK Food Standards Agency: "Current EU approved additives and their E Numbers". Retrieved 2011-10-27.
- US Food and Drug Administration: "Listing of Food Additives Status Part II". Food and Drug Administration. Retrieved 2011-10-27.
- Australia New Zealand Food Standards Code"Standard 1.2.4 - Labelling of ingredients". Retrieved 2011-10-27.
- Dale Ulmer (1994). "Fixation. The Key to Good Tissue Preservation" (PDF). Journal of the International Society for Plastination. 8 (1): 7–10. Archived from the original (PDF) on 2011-05-16. Retrieved 2017-09-08.
- Andrew Nagorski (2007). The Greatest Battle. Simon and Schuster. p. 53.
- "Oklahoma used wrong drug in Charles Warner's execution, autopsy report says".
- Eyder Peralta. "Oklahoma Used The Wrong Drug To Execute Charles Warner". NPR.
- Jason Dearon. "Florida executes convicted killer Mark Asay using new drug". Sun Sentinel.
- 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.