SODIUM ACETATE

CAS No.: 127-09-3
EC No.: 204-823-8

Synonyms:
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Ph. Eur., anhydrous; Sodium acetate, anhydrous, BioUltra, for luminescence, for molecular biology, >=99.0% (NT); SODIUM ACETATE; sodium acetate; SODYUM ASETAT; sodyum asetat; Sodium acetate, anhydrous, free-flowing, Redi-Dri(TM), ACS reagent, >=99.0%; Mettler-Toledo Calibration substance ME 30130599, Sodium acetate anhydrous, tracable to primary standards (LGC); Sodium acetate solution, NMR reference standard, 50 mM in D2O (99.9 atom % D), water 1 %, NMR tube size 3 mm x 8 in.; SODIUM ACETATE; sodium acetate; SODYUM ASETAT; sodyum asetat; Sodium acetate, powder, BioReagent, for electrophoresis, suitable for cell culture, suitable for insect cell culture, >=99%; SODIUM ACETATE; sodium acetate; SODYUM ASETAT; sodyum asetat; sodium acetate; acetic acid; sodium salt; sodium acetate anhydrous; sodium acetate; anhydrous; acetic acid sodium salt; anhydrous sodium acetate; sodii acetas; sodium ethanoate; natrium aceticum; octan sodny czech

SODIUM ACETATE

Sodium acetate
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This article is about sodium acetate. For other uses of hot ice, see Hot ice (disambiguation).
Sodium acetate
Skeletal formula of sodium acetate
Sodium acetate
Names
IUPAC name
Sodium acetate
Systematic IUPAC name
Sodium ethanoate
Other names
Hot ice (sodium acetate trihydrate)
Identifiers
CAS Number    
anhydrous: 127-09-3 check
trihydrate: 6131-90-4 check
3D model (JSmol)    
anhydrous: Interactive image
Beilstein Reference    3595639
ChEBI    
anhydrous: CHEBI:32954 check
trihydrate: CHEBI:32138
ChEMBL    
anhydrous: ChEMBL1354 check
ChemSpider    
anhydrous: 29105 check
ECHA InfoCard    100.004.386 Edit this at Wikidata
EC Number    
anhydrous: 204-823-8
E number    E262 (preservatives)
Gmelin Reference    20502
KEGG    
trihydrate: D01779
PubChem CID    
anhydrous: 517045
trihydrate: 23665404
RTECS number    
anhydrous: AJ4300010 (anhydrous)
AJ4580000
UNII    
anhydrous: NVG71ZZ7P0 check
trihydrate: 4550K0SC9B
CompTox Dashboard (EPA)    
anhydrous: DTXSID2027044 Edit this at Wikidata
InChI[show]
SMILES[show]
Properties
Chemical formula    C2H3NaO2
Molar mass    82.034 g·mol−1
Appearance    White deliquescent powder
Odor    Vinegar (acetic acid) odor when heated to decomposition[1]
Density    1.528 g/cm3 (20 °C, anhydrous)
1.45 g/cm3 (20 °C, trihydrate)[2]
Melting point    324 °C (615 °F; 597 K)
(anhydrous)
58 °C (136 °F; 331 K)
(trihydrate)
Boiling point    881.4 °C (1,618.5 °F; 1,154.5 K)
(anhydrous)
122 °C (252 °F; 395 K)
(trihydrate) decomposes
Solubility in water    Anhydrous:
Solubility    Soluble in alcohol, hydrazine, SO2[4]
Solubility in methanol    16 g/100 g (15 °C)
16.55 g/100 g (67.7 °C)[4]
Solubility in ethanol    Trihydrate:
5.3 g/100 mL
Solubility in acetone    0.5 g/kg (15 °C)[4]
Acidity (pKa)    24 (20 °C)[4]
4.75 CH3COOH[5]
Basicity (pKb)    9.25
Magnetic susceptibility (χ)    −37.6·10−6 cm3/mol
Refractive index (nD)    1.464
Structure
Crystal structure    Monoclinic
Thermochemistry
Heat capacity (C)    100.83 J/mol·K (anhydrous)[6]
229 J/mol·K (trihydrate)[7]
Std molar
entropy (So298)    138.1 J/mol·K (anhydrous)[6]
262 J/mol·K (trihydrate)[2]
Std enthalpy of
formation (ΔfH⦵298)    −709.32 kJ/mol (anhydrous)[4]
−1604 kJ/mol (trihydrate)[2]
Gibbs free energy (ΔfG˚)    −607.7 kJ/mol (anhydrous)[4]
Pharmacology
ATC code    B05XA08 (WHO)
Hazards
Main hazards    Irritant
Safety data sheet    External MSDS
NFPA 704 (fire diamond)    
NFPA 704 four-colored diamond
110
Flash point    >250 °C (482 °F; 523 K) [5]
Autoignition
temperature    600 °C (1,112 °F; 873 K)[5]
Lethal dose or concentration (LD, LC):
LD50 (median dose)    3530 mg/kg (oral, rat)
Related compounds
Other anions    Sodium formate
Sodium propionate
Other cations    Potassium acetate
Calcium acetate
Related compounds    Sodium diacetate
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
Sodium acetate, NaCH3COO, also abbreviated NaOAc,[8] is the sodium salt of acetic acid. This colorless deliquescent salt has a wide range of uses.

Contents
1    Applications
1.1    Biotechnological
1.2    Industrial
1.3    Concrete longevity
1.4    Food
1.5    Buffer solution
1.6    Heating pad
2    Preparation
3    Reactions
4    References
5    External links
Applications
Biotechnological
Sodium acetate is used as the carbon source for culturing bacteria. Sodium acetate is also useful for increasing yields of DNA isolation by ethanol precipitation.

Industrial
Sodium acetate is used in the textile industry to neutralize sulfuric acid waste streams and also as a photoresist while using aniline dyes. It is also a pickling agent in chrome tanning and helps to impede vulcanization of chloroprene in synthetic rubber production. In processing cotton for disposable cotton pads, sodium acetate is used to eliminate the buildup of static electricity.

Concrete longevity
Sodium acetate is used to mitigate water damage to concrete by acting as a concrete sealant, while also being environmentally benign and cheaper than the commonly used epoxy alternative for sealing concrete against water permeation.[9]

Food
Sodium acetate may be added to food as a seasoning, sometimes in the form of sodium diacetate, a one-to-one complex of sodium acetate and acetic acid,[10] given the E-number E262. It is often used to give potato chips a salt and vinegar flavor.[citation needed] Sodium acetate (anhydrous) is widely used as a shelf-life extending agent, pH control agent[11] It is safe to eat at low concentration.[12]

Buffer solution
A solution of sodium acetate (a basic salt of acetic acid) and acetic acid can act as a buffer to keep a relatively constant pH level. This is useful especially in biochemical applications where reactions are pH-dependent in a mildly acidic range (pH 4–6).

Heating pad

A hand warmer containing a supersaturated solution of sodium acetate which releases heat upon crystallization
Sodium acetate is also used in heating pads, hand warmers, and hot ice. Sodium acetate trihydrate crystals melt at 136.4 °F/58 °C[13] (to 137.12 °F/58.4 °C),[14] dissolving in their water of crystallization. When they are heated past the melting point and subsequently allowed to cool, the aqueous solution becomes supersaturated. This solution is capable of cooling to room temperature without forming crystals. By pressing on a metal disc within the heating pad, a nucleation center is formed, causing the solution to crystallize back into solid sodium acetate trihydrate. The bond-forming process of crystallization is exothermic.[15] The latent heat of fusion is about 264–289 kJ/kg.[13] Unlike some types of heat packs, such as those dependent upon irreversible chemical reactions, a sodium acetate heat pack can be easily reused by immersing the pack in boiling water for a few minutes, until the crystals are completely dissolved, and allowing the pack to slowly cool to room temperature.[16]

Preparation

A crystal of sodium acetate trihydrate (length 1.7 centimetres)
For laboratory use, sodium acetate is inexpensive and usually purchased instead of being synthesized. It is sometimes produced in a laboratory experiment by the reaction of acetic acid, commonly in the 5–8% solution known as vinegar, with sodium carbonate ("washing soda"), sodium bicarbonate ("baking soda"), or sodium hydroxide ("lye", or "caustic soda"). Any of these reactions produce sodium acetate and water. When a sodium and carbonate ion-containing compound is used as the reactant, the carbonate anion from sodium bicarbonate or carbonate, reacts with hydrogen from the carboxyl group (-COOH) in acetic acid, forming carbonic acid. Carbonic acid readily decomposes under normal conditions into gaseous carbon dioxide and water. This is the reaction taking place in the well-known "volcano" that occurs when the household products, baking soda and vinegar, are combined.

CH3COOH + NaHCO3 → CH3COONa + H2CO
3
H2CO
3 → CO
2 + H
2O
Industrially, sodium acetate trihydrate is prepared by reacting acetic acid with sodium hydroxide using water as the solvent.

CH3COOH + NaOH → CH3COONa + H2O
Reactions
Sodium acetate can be used to form an ester with an alkyl halide such as bromoethane:

CH3COONa + BrCH2CH3 → CH3COOCH2CH3 + NaBr
Sodium acetate undergoes decarboxylation to form methane (CH4) under forcing conditions (pyrolysis in the presence of sodium hydroxide):

CH3COONa + NaOH → CH4 + Na2CO3
Calcium oxide is the typical catalyst used for this reaction. Caesium salts also catalyze this reaction

What is Sodium acetate (anhydrous) （CH3COONa）？    [close]
Acetic acid has been said to prevent bacteria cultivation and therefore has been used not only to add sour taste but to preserve food.
Sodium acetate is a food additive obtained by neutralization of acetic acid. When used as a food additive, sodium acetate can be indicated by its group name, substance name, or abbreviated name according to the purpose of use.

Purpose    Group name or abbreviated name
Keep the pH level of food within the appropriate level    pH regulator
Improve taste by adding or enhancing sour taste    Sour agent
Improve taste by adding or controlling taste    Seasoning (Organic acid)
Other purposes (shelf-life extension, combined use with preservative, etc.    Sodium acetate
What is a shelf-life extending agent？    [close]
A sanitizer, antioxidant, and preservative are used to maintain the quality of food. As specified in the regulation in regard to food labeling, an antioxidant and preservative are indicated with the application name as “preservative, etc.” The use of many of these agents is restricted so they are not available to some food.
A shelf-life extending agent, indicated only with its name (sodium acetate), functions like these agents, giving slightly moderate effects. It is highly safe and its use is not restricted.
Sodium acetate can prevent bacteria cultivation in a wide range of acidic region. It also functions as a buffer as well. When used to add sour taste to food, acetic acid is generally selected, but combination of sodium acetate and acetic acid can make the taste mild.