Ammonium acetate

Ammonium acetate
Names
	IUPAC name Ammonium ethanoate
Identifiers
CAS Number	631-61-8 ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:62947 ;
ChemSpider	11925 ;
ECHA InfoCard	100.010.149
PubChem CID	517165;
RTECS number	AF3675000;
UNII	RRE756S6Q2 ;
CompTox Dashboard (EPA)	DTXSID5023873 ;
	InChI InChI=1S/C2H4O2.H3N/c1-2(3)4;/h1H3,(H,3,4);1H3 Key: USFZMSVCRYTOJT-UHFFFAOYSA-N ; InChI=1/C2H4O2.H3N/c1-2(3)4;/h1H3,(H,3,4);1H3 Key: USFZMSVCRYTOJT-UHFFFAOYAY;
	SMILES O=C(O)C.N;
Properties
Chemical formula	C2H7NO2
Molar mass	77.083 g·mol−1
Appearance	White solid crystals, deliquescent
Odor	Slightly acetic
Density	1.17 g/cm3 (20 °C); 1.073 g/cm3 (25 °C)
Melting point	113 °C (235 °F; 386 K)
Solubility in water	102 g/100 mL (0 °C); 148 g/100 mL (4 °C); 143 g/100 mL (20 °C); 533 g/100 mL (80 °C)
Solubility	Soluble in alcohol, SO2, acetone, liquid ammonia
Solubility in methanol	7.89 g/100 mL (15 °C); 131.24 g/100 g (94.2 °C)
Solubility in dimethylformamide	0.1 g/100 g
Structure
Crystal structure	Orthorhombic
Thermochemistry
Std enthalpy of; formation (ΔfH⦵298)	−615 kJ/mol
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Irritant
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H303, H316, H320, H333
Precautionary statements	P281, P335
NFPA 704 (fire diamond)	1 1 1
Flash point	136 °C (277 °F; 409 K)
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	386 mg/kg (mice, intravenous)
Safety data sheet (SDS)	JT Baker
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) 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

NH₄C₂H₃O₂ is occasionally employed as a biodegradable de-icing agent.
Ammonium acetate is useful as a catalyst in the Knoevenagel condensation and as a source of ammonia in the Borch reaction in organic synthesis.
a protein precipitating reagent.
In dialysis as part of a protein purification step to remove contaminants via diffusion.
In agricultural chemistry used as reagent for determination of soil CEC (Cation Exchange Capacity ) and determination of available potassium in soil, ammonium ion is act as an replacement cation.

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

^ ^a ^b ^c Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. ISBN 0-07-049439-8.
^ ^a ^b ^c ^d ^e http://chemister.ru/Database/properties-en.php?dbid=1&id=354
^ ^a ^b ^c ^d ^e ^f "Safety Data Sheet of Ammonium Acetate" (PDF). http://www.tedia.com. Tedia Company Inc. 2011-08-12. Retrieved 2014-06-10. {{cite web}}: External link in |website= (help)
^ 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.
^ ^a ^b Hosea Cheung; Robin S. Tanke; G. Paul Torrence. "Acetic Acid". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a01_045.pub2. ISBN 978-3527306732.
^ Coleman, G. H.; Alvarado, A. M. (1923). "Acetamide". Organic Syntheses. 3: 3; Collected Volumes, vol. 1, p. 3.
^ Berman et al., 2008. J Am Soc Mass Spectrom, 19:1230-1236.
^ Australia New Zealand Food Standards Code "Standard 1.2.4 - Labelling of ingredients". Retrieved 2011-10-27.
^ Brannt, William (1914). A practical treatise on the manufacture of vinegar. Lancaster, PA: Henry Carey Baird & Co. pp. 316–317.

External links

[pphoic-1] Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. ISBN 0-07-049439-8.

[chemister-2] ttp://chemister.ru/Database/properties-en.php?dbid=1&id=354

[tedia-3] ^ ^a ^b ^c ^d ^e ^f "Safety Data Sheet of Ammonium Acetate" (PDF). http://www.tedia.com. Tedia Company Inc. 2011-08-12. Retrieved 2014-06-10. {{cite web}}: External link in |website= (help)

[0-4] 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.

[Ullmann-5] Hosea Cheung; Robin S. Tanke; G. Paul Torrence. "Acetic Acid". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a01_045.pub2. ISBN 978-3527306732.

[6] Coleman, G. H.; Alvarado, A. M. (1923). "Acetamide". Organic Syntheses. 3: 3; Collected Volumes, 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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