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Sodium acetate

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Sodium acetate Basic information
Sodium acetate Chemical Properties
  • Melting point:>300 °C (dec.)(lit.)
  • Density 1.01 g/mL at 20 °C
  • refractive index 1.4640
  • FEMA 3024 | SODIUM ACETATE
  • Flash point:>250 °C
  • storage temp. 2-8°C
  • solubility H2O: 3 M at 20 °C, clear, colorless
  • form powder
  • color white
  • PH8.9 (25℃, 100mg/mL in water, 0.1 M agueous sodium acetate solution)
  • Water Solubility 500 g/L (20 ºC)
  • Sensitive Hygroscopic
  • λmaxλ: 260 nm Amax: 0.03
    λ: 280 nm Amax: 0.02
  • Merck 14,8571
  • Boiling point:>400°C(decomposition)
  • BRN 3595639
  • Stability:Stable. Incompatible with strong oxidizing agents, halogens. Moisture sensitive.
  • InChIKeyVMHLLURERBWHNL-UHFFFAOYSA-M
  • CAS DataBase Reference127-09-3(CAS DataBase Reference)
  • NIST Chemistry ReferenceSodium ethanoate(127-09-3)
  • EPA Substance Registry SystemAcetic acid, sodium salt(127-09-3)
Safety Information
  • Safety Statements 22-24/25
  • WGK Germany 1
  • RTECS AJ4300010
  • 3
  • Autoignition Temperature607 °C
  • TSCA Yes
  • HS Code 29152200
  • Hazardous Substances Data127-09-3(Hazardous Substances Data)
  • ToxicityLD50 orally in Rabbit: 3530 mg/kg LD50 dermal Rabbit > 10000 mg/kg
MSDS
Sodium acetate Usage And Synthesis
  • DescriptionSodium acetate (CH3COONa) is the sodium salt of acetic acid. It appears as a colorless deliquescent salt with a wide range of applications. In industry, it can be used in textile industry to neutralize sulfuric acid waste streams and as a photoresist upon using aniline dyes. In concrete industry, it can be used as a concrete sealant to mitigate the water damage. In food, it can be used as a seasoning. It can also be used as a buffer solution in lab. In addition, it is also used in heating pads, hand warmers and hot ice. For laboratory use, it can be produced by the reaction between acetate with the sodium carbonate, sodium bicarbonate and sodium hydroxide. In industry, it is prepared from the glacial acetic acid and sodium hydroxide.
  • Chemical PropertiesAnhydrous salt is a colorless crystalline solid; density 1.528 g/cm3; melts at 324°C; very soluble in water; moderately soluble in ethanol. The colorless crystalline trihydrate has a density 1.45 g/cm3; decomposes at 58°C; is very soluble in water; pH of 0.1M aqueous solution is 8.9; moderately soluble in ethanol, 5.3 g/100mL.
  • Chemical PropertiesSodium acetate, CH3COONa, also abbreviated NaOAc , also sodium ethanoate, is the sodium salt of acetic acid. This colourless salt has a wide range of uses.
  • Chemical PropertiesSodium acetate is odorless or has a faint acetous odor. It effloresces in warm, dry air.
  • OccurrenceAcetic acid or acetates are present in most plant and animal tissues in small, but detectable amounts
  • UsesSodium Acetate is a source of acetic acid that is obtained as crystals or powder. it has a solubility of 1 g in 0.8 ml of water.
  • UsesSodium Acetate, Anhydrous is a source of acetic acid obtained as a granular powder. it has a solubility of 1 g in 2 ml of water.
  • UsesThis colorless crystal, also known as sodium ethanoate or acetate of soda, was made by the reaction of acetic acid with sodium carbonate. It is soluble in water but less so in alcohol. Sodium acetate was used as a pH modifier for toning baths.
  • UsesSodium acetate is a mordant in dyeing. Other applications are in photography, as an additive to food, in purification of glucose, in preservation of meat, in tanning, and as a dehydrating agent. In analytical chemistry it is used to prepare buffer solution.
    Sodium acetate can be used to preserve processed meats and it is often used in combination with other acid based preservatives like lactates and propionates. The typical inclusion level is 0.2 to 0.5%. Sodium acetate is also used in salad dressings and ready-to-eat meals.
  • UsesUsed as buffers.
    Acidity regulation (buffering)
    Sodium acetate mixed with acetic acid forms a pH buffer, which can be used to stabilise the pH of foods in the pH-range from 3 to 6. The table below gives indicative values of the composition needed to give a certain pH. The mixtures below can be diluted at least 10 times with minimum effect on pH, however, the stability decreases.
    Acidity regulation (Sodium acetate buffering)
  • PreparationSodium acetate is prepared by reacting sodium hydroxide or sodium carbonate with acetic acid in aqueous solution. The solution is evaporated to obtain hydrated crystals of sodium acetate.
    NaOH + CH3COOH → CH3COONa + H2O
    Na2CO3 + CH3COOH → 2CH3COONa + CO2 + H2O
  • DefinitionA white solid prepared by the neutralization of ethanoic acid with either sodium carbonate or sodium hydroxide. Sodium ethanoate reacts with sulfuric acid to form sodium hydrogensulfate and ethanoic acid; with sodium hydroxide it gives rise to sodium carbonate and methane. Sodium ethanoate is used in the dyeing industry.
  • Application2 - 1 - Industrial
    Sodium acetate is used in the textile industry to neutralize sulfuric acid waste streams, and as a photoresist while using aniline dyes. It is also a pickling agent in chrome tanning, and it helps to retard 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.
    2 - 2 - Concrete longevity
    Sodium acetate is used to reduce the damage water can potentially do to concrete by acting as a concrete sealant, while also being environmentally benign and cheaper than the epoxy alternative that is usually employed for sealing concrete against water permeation.
    2 - 3 - Food
    Sodium acetate may be added to foods as a seasoning. It may be used in the form of sodium diacetate — a 1:1 complex of sodium acetate and acetic acid, given the E-number E262. A frequent use is to impart a salt and vinegar flavor to potato chips.
    2 - 4 - Buffer solution
    As the conjugate base of acetic acid, a solution of sodium acetate and acetic acid can act as a buffer to keep a relatively constant pH.
    2 - 5 - Heating pad
    Sodium acetate is also used in consumer heating pads or hand warmers and is also used in hot ice. Sodium acetate trihydrate crystals melt at 58.4°C , (to 58°C ) dissolving in their water of crystallization. When they are heated to around 100°C, and subsequently allowed to cool, the aqueous solution becomes supersaturated. This solution is capable of cooling to room temperature with out forming crystals.
  • PreparationFor laboratory use, sodium acetate is very inexpensive, and is usually purchased instead of being synthesized. It is sometimes produced in a laboratory experiment by the reaction of acetic acid (ethanoic acid) with sodium carbonate, sodium bicarbonate, or sodium hydroxide. These reactions produce aqueous sodium acetate and water. Carbon dioxide is produced in the reaction with sodium carbonate and bicarbonate, and it leaves the reaction vessel as a gas (unless the reaction vessel is pressurized). This is the well-known "volcano" reaction between baking soda (sodium bicarbonate) and vinegar.
    CH3COOH + NaHCO3 → CH3COONa + H2O + CO2
    Industrially, sodium acetate is prepared from glacial acetic acid and sodium hydroxide.
    CH3COOH + NaOH → CH3COONa + H2O .
  • ReactionsSodium acetate can be used to form an ester with an alkyl halide such as bromo ethane:
    CH3COONa + Br CH2CH3→ CH3COOCH2CH3+ NaBr
    Caesium salts catalyze this reaction.
  • Reactivity ProfileWhen sodium acetate reacts with strong acids, irritating, noxious vapors of acetic acid are usually produced. Sodium acetate is sufficiently basic to catalyze the violent polymerization of diketene, perhaps as well as other reactive dimers that are susceptible to polymerization in the presence of a mild base.
  • Biological ActivityCommonly used laboratory reagent
  • Safety ProfilePoison by intravenous route. Moderately toxic by ingestion. A skin and eye irritant. Migrates to food from packagmg materials. Violent reaction with F2, m03, diketene. When heated to decomposition it emits toxic fumes of Na2O.
  • Chemical SynthesisAcetic acid plus sodium bicarbonate makes sodium acetate plus carbonic acid. Produced by the neutralization of acetic acid with sodium bicarbonate, or by treating calcium acetate with sodium sulfate and sodium bicarbonate.
  • Purification MethodsCrystallise it from acetic acid and keep it under vacuum for 10hours at 120o. Alternatively, it is crystallised from aqueous EtOH, as the trihydrate. This material can be converted to anhydrous salt by heating slowly in a porcelain, nickel or iron dish, so that the salt liquefies. Steam is evolved and the mass again solidifies. Heating is now increased so that the salt melts again. (NB: if it is heated too strongly, the salt can char; avoid this.) After several minutes, the salt is allowed to solidify and is cooled to a convenient temperature (in a desiccator) before being powdered and bottled. The water content should now be less than 0.02%. [Beilstein 2 II 113, 2 III 184, 2 IV 109.]
Sodium acetate Preparation Products And Raw materials
Sodium acetate(127-09-3)Related Product Information
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