Ammonium acetate

Ammonium acetate
Names
IUPAC name
Ammonium ethanoate
Identifiers
631-61-8 YesY
3D model (Jmol) Interactive image
ChEBI CHEBI:62947 N
ChemSpider 11925 YesY
ECHA InfoCard 100.010.149
PubChem 517165
RTECS number AF3675000
UNII RRE756S6Q2 YesY
Properties
C2H7NO2
Molar mass 77.08 g·mol−1
Appearance White solid crystals, deliquescent
Odor Slightly acetic
Density 1.17 g/cm3 (20 °C)[1]
1.073 g/cm3 (25 °C)
Melting point 113 °C (235 °F; 386 K) [2]
102 g/100 mL (0 °C)
148 g/100 mL (4 °C)[1]
143 g/100 mL (20 °C)
533 g/100 mL (80 °C)
Solubility Soluble in alcohol, SO2, acetone, liquid ammonia[3]
Solubility in methanol 7.89 g/100 mL (15 °C)[4][1]
131.24 g/100 g (94.2 °C)[3]
Solubility in dimethylformamide 0.1 g/100 g[3]
Structure
Orthorhombic
Thermochemistry
−615 kJ/mol[3]
Hazards
Main hazards Irritant
Safety data sheet JT Baker
GHS pictograms [4]
GHS signal word Warning
H303, H316, H320, H333[4]
P281, P335[4]
NFPA 704
Flash point 136 °C (277 °F; 409 K) [4]
Lethal dose or concentration (LD, LC):
386 mg/kg (mice, intravenous)[3]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Ammonium acetate is a chemical compound with the formula NH4CH3CO2. It is a white, hygroscopic solid and can be derived from the reaction of ammonia and acetic acid. It is available commercially.[5]

Uses

It is the main precursor to acetamide:[6]

NH4CH3CO2 → CH3C(O)NH2 + H2O

It is also used as a diuretic.[5]

Buffer

As the salt of a weak acid and a weak base, ammonium acetate is often used with acetic acid to create a buffer solution. Ammonium acetate is volatile at low pressures. Because of this, it has been used to replace cell buffers with non-volatile salts in preparing samples for mass spectrometry.[7] It is also popular as a buffer for mobile phases for HPLC with ELSD detection for this reason. Other volatile salts that have been used for this include ammonium formate.

Other

Food additive

Ammonium acetate is also used as a food additive as an acidity regulator; INS number 264. It is approved for usage in Australia and New Zealand.[8]

Production

Ammonium acetate is produced by the neutralization of acetic acid with ammonium carbonate or by saturating glacial acetic acid with ammonia.[9] Obtaining crystalline ammonium acetate is difficult on account of its aqueous solution giving off ammonia when evaporated.

References

  1. 1 2 3 Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. ISBN 0-07-049439-8.
  2. ↑ Davidson, Arthur W.; McAllister, Walter H. (1930). "SOLUTIONS OF SALTS IN PURE ACETIC ACID. II. SOLUBILITIES OF ACETATES1". Journal of the American Chemical Society. 52 (2): 507–519. doi:10.1021/ja01365a010. ISSN 0002-7863.
  3. 1 2 3 4 5 http://chemister.ru/Database/properties-en.php?dbid=1&id=354
  4. 1 2 3 4 5 6 "Safety Data Sheet of Ammonium Acetate" (PDF). http://www.tedia.com. Tedia Company Inc. 2011-08-12. Retrieved 2014-06-10. External link in |website= (help)
  5. 1 2 Hosea Cheung; Robin S. Tanke; G. Paul Torrence (2005), "Acetic Acid", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a01_045.pub2
  6. ↑ Coleman, G. H.; Alvarado, A. M. (1923). "Acetamide". Org. Synth. 3: 3.; Coll. Vol., 1, p. 3
  7. ↑ Berman et al., 2008. J Am Soc Mass Spectrom, 19:1230-1236.
  8. ↑ Australia New Zealand Food Standards Code "Standard 1.2.4 - Labelling of ingredients". Retrieved 2011-10-27.
  9. ↑ Brannt, William (1914). A practical treatise on the manufacture of vinegar. Lancaster, PA: Henry Carey Baird & Co. pp. 316–317.

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