127-09-3 Usage
Chemical Description
Different sources of media describe the Chemical Description of 127-09-3 differently. You can refer to the following data:
1. Sodium acetate is a salt commonly used as a buffer in biochemistry.
2. Sodium acetate is a salt commonly used in the textile industry.
3. Sodium acetate is a white crystalline powder that is used in the textile industry.
Description
Sodium 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 Properties
Different sources of media describe the Chemical Properties of 127-09-3 differently. You can refer to the following data:
1. Anhydrous 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.
2. Sodium acetate, CH3COONa, also abbreviated NaOAc , also sodium ethanoate, is the sodium salt of acetic acid, was made by the reaction of acetic acid with sodium carbonate. It is soluble in water but less so in alcohol. This colourless salt has a wide range of uses. Sodium acetate was used as a pH modifier for toning baths.
3. Sodium acetate is odorless or has a faint acetous odor. It effloresces in warm, dry air.
Physical properties
Anhydrous 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.
Occurrence
Acetic acid or acetates are present in most plant and animal tissues in small, but detectable amounts
Uses
Different sources of media describe the Uses of 127-09-3 differently. You can refer to the following data:
1. Sodium 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.
2. Sodium 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.
3. Used 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.
Preparation
Sodium 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
Definition
A 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.
Application
2 - 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.
Synthesis
Different sources of media describe the Synthesis of 127-09-3 differently. You can refer to the following data:
1. For 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.
2. Acetic 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.
Reactions
Sodium 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.
General Description
Sodium Acetate is reported to inhibit the growth of Listeria monocytogenes.
Reactivity Profile
When 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.
Flammability and Explosibility
Nonflammable
Biological Activity
Commonly used laboratory reagent
Safety Profile
Poison 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.
Purification Methods
Crystallise 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.]
Check Digit Verification of cas no
The CAS Registry Mumber 127-09-3 includes 6 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 3 digits, 1,2 and 7 respectively; the second part has 2 digits, 0 and 9 respectively.
Calculate Digit Verification of CAS Registry Number 127-09:
(5*1)+(4*2)+(3*7)+(2*0)+(1*9)=43
43 % 10 = 3
So 127-09-3 is a valid CAS Registry Number.
InChI:InChI=1/C2H4O2.Na.3H2O/c1-2(3)4;;;;/h1H3,(H,3,4);;3*1H2/q;+1;;;/p-1
127-09-3Relevant articles and documents
Depree,Closson
, p. 2311 (1958)
A new, more efficient procedure for the preparation of potassium tris(malonto)cobaltate(III) dihydrate
Miodragovic, Zoran M.,Vuckovic, Gordana
, p. 1451 - 1461 (1999)
A new, very efficient and elegant procedure for the preparation of potassium tris(malonato)cobaltate(III) dihydrate, starting from Co(OH)3 and potassium hydrogenmalonate, is presented. The most important advantages of this procedure, in comparison to the previously reported ones, are: a relatively short time required, saving of the reagents and solvents, and a very good yield of pure product. The identification of the obtained complex was carried out by elemental analyses, electronic absorption and IR spectroscopy. The spectral data are in accordance with the previously reported literature data. Analogous procedure was also preliminary tested for the preparation of the corresponding tris(oxalato)-and tris(succinato)cobaltate(III). Finally, the described complex can be used as a starting material for the preparation of one mixed ligand Co(III) complex.
Efficient Iridium Catalysts for Formic Acid Dehydrogenation: Investigating the Electronic Effect on the Elementary β-Hydride Elimination and Hydrogen Formation Steps
Liu, Hong,Wang, Wan-Hui,Xiong, Huatian,Nijamudheen,Ertem, Mehmed Z.,Wang, Mei,Duan, Lele
, p. 3410 - 3417 (2021)
We report herein a series of Cp*Ir complexes containing a rigid 8-aminoquinolinesulfonamide moiety as highly efficient catalysts for the dehydrogenation of formic acid (FA). The complex [Cp*Ir(L)Cl] (HL = N-(quinolin-8-yl)benzenesulfonamide) displayed a high turnover frequency (TOF) of 2.97 × 104 h-1 and a good stability (>100 h) at 60 °C. Comparative studies of [Cp*Ir(L)Cl] with the rigid ligand and [Cp*Ir(L′)Cl] (HL′ = N-propylpypridine-2-sulfonamide) without the rigid aminoquinoline moiety demonstrated that the 8-aminoquinoline moiety could dramatically enhance the stability of the catalyst. The electron-donating ability of the N,N′-chelating ligand was tuned by functionalizing the phenyl group of the L ligand with OMe, Cl, and CF3 to have a systematical perturbation of the electronic structure of [Cp*Ir(L)Cl]. Experimental kinetic studies and density functional theory (DFT) calculations on this series of Cp*Ir complexes revealed that (i) the electron-donating groups enhance the hydrogen formation step while slowing down the β-hydride elimination and (ii) the electron-withdrawing groups display the opposite effect on these reaction steps, which in turn leads to lower optimum pH for catalytic activity compared to the electron-donating groups.
Synthesis and characterization of complexes of some hydroxyaryltellurium trichlorides with N-donor ligands
Verma,Dahiya, Reena,Soni, Daya
, p. 1033 - 1052 (1999)
Twenty new complexes of hydroxyaryltellurium trichlorides derived from isomeric cresols and ortho-chlorophenol with pyridine (Py), 2,2′-bipyridyl (Bipy) and piperidine (Pip) have been synthesized and characterized by elemental analyses, conductance, cryoscopy, infrared and proton magnetic resonance studies. Pyridine and piperidine form RTeCl3.L and RTeCl3.2L complexes, whereas 2,2′-bipyridyl which acts as a bidentate ligand and gives only RTeCl3.L complexes. Conductance and cryoscopic measurements reflect their weak or 1:1 electrolytic behaviour in solution of nitrobenzene, acetonitrile and acetone. Spectral studies indicate the linkage of these ligand molecules to the tellurium atom of the hydroxyaryltellurium group through nitrogen atoms. A square-pyramidal structure is suggested for RTeCl3.Py and RTeCl3.Pip, whereas 1:2 complexes of pyridine and piperidine along with RTeCl3.Bipy, have octahedral stereochemistry.
Interaction of cobalt(II) and copper(II) with polyoxometallates. Structure of Na3Co[IMo6O24]. 14H2O
Rosu, Cristina,Gomez-Garcia, Carlos Jose,Dickman, Michael H.,Rusu, Mariana
, p. 1123 - 1131 (1999)
Cobalt(II) and copper(II) complexes with the ligand anion [IMo6O24]5- (periodate 6-molybdoanion) of the general formula Na3M[IMo6O24].nH2O (where M = Co, Cu) have been prepared by the reaction of the corresponding metal salts with the ligand in aqueous media (pH = 6). The complexes were characterised by elemental and thermogravimetric analyses, spectral data (IR, UV-vis). The EPR spectrum of a copper(II) powder sample was recorded at both room temperature and 12 K indicating a weakly distorted octahedral copper(II) stereochemistry. The crystal structure of Na3CO[IMo6O24]. 14H2O has been determined by single-crystal X-ray diffraction technique.
Seyb, E.,Kleinberg, J.
, p. 115 - 117 (1951)
Selective formation of lactate by oxidation of 1,2-propanediol using gold palladium alloy supported nanocrystals
Dimitratos, Nikolaos,Lopez-Sanchez, Jose Antonio,Meenakshisundaram, Sankar,Anthonykutty, Jinto Manjaly,Brett, Gemma,Carley, Albert F.,Taylor, Stuart H.,Knight, David W.,Hutchings, Graham J.
, p. 1209 - 1216 (2009)
The use of bio-renewable resources, such as glycerol, a by-product from bio-diesel manufacture, can provide a viable way to make valuable products using greener technology. In particular, glycerol can be reduced to give 1,2-propanediol that can then be se
No contribution of an inductive effect to secondary deuterium isotope effects on acidity
Perrin, Charles L.,Flach, Agnes
, p. 7674 - 7676 (2011)
Effect and cause: Secondary deuterium isotope effects on the acidity of the deuterated compounds 1-4 were measured by using an NMR titration method applicable to a mixture and capable of very high accuracy. Variable-temperature experiments show that these isotope effects are due only to changes in vibrational frequencies. These findings refute an inductive origin for these isotope effects. Copyright
MECHANISM OF CHLORAMINE-T OXIDATION OF METHYL VINYL KETONE AND ISOPROPYL METHYL KETONE IN AQUEOUS ALKALINE MEDIA
Singh, Bharat,Samant, A. K.,Saxena, B. B. L.
, p. 2591 - 2594 (1982)
The oxidation kinetics of methyl vinyl ketone and isopropyl methyl ketone by chloramine-T in aqueous alkaline solutions show first-order dependence on chloramine-T, both substrates and alkali.No effect of p-toluenesulphonamide was evident.Observed stoichiometry, negligible effect of ionic strength and a positive dielectric effect point to a mechanism involving interaction of enolate anions with chloramine-T in the rate determining step.Activation parameters and the isolation of the product formaldehyde are in agreement with the proposed mechanism.
Photoluminescence as a valuable tool in the optical characterization of acetaminophen and the monitoring of its photodegradation reactions
Baibarac, Mihaela,Daescu, Monica,Ion, Alina C.,Matea, Adelina,Negrila, Catalin,Serbschi, Constantin
, (2020/10/22)
In this work, new evidence for the photodegradation reactions of acetaminophen (AC) is reported by photoluminescence (PL), Raman scattering and FTIR spectroscopy. Under excitation wavelength of 320 nm, AC shows a PL band in the spectral range of 340–550 nm, whose intensity decreases by exposure to UV light. The chemical interaction of AC with the NaOH solutions, having the concentration ranging between 0.001 and 0.3 M, induces a gradual enhancement of the photoluminescence excitation (PLE) and PL spectra, when the exposure time of samples at the UV light increases until 140 min, as a result of the formation of p-aminophenol and sodium acetate. This behavior is not influenced by the excipients or other active compounds in pharmaceutical products as demonstrated by PLE and PL studies. Experimental arguments for the obtaining of p-aminophenol and sodium acetate, when AC has interacted with NaOH, are shown by Raman scattering and FTIR spectroscopy.
Br?nsted and Lewis Base Behavior of Sodium Amidotrihydridoborate (NaNH2BH3)
Chen, Xi-Meng,Li, Huizhen,Yang, Qiu-Yu,Wang, Rui-Rui,Hamilton, Ewan J. M.,Zhang, Jie,Chen, Xuenian
, p. 4541 - 4545 (2017/09/28)
The reactivity of sodium amidoborane (NaNH2BH3) as a Br?nsted and Lewis base was studied systematically. The [NH2BH3]– anion can act as a proton acceptor or a hydride donor in different types of reactions. In reactions with very weak Br?nsted acids such as cyclopentadiene, ammonia, and pyrazole, the [NH2BH3]– anion acts as a proton acceptor through the lone pair on N. The reactions of [NH2BH3]– with stronger Br?nsted acids are complicated. In the reaction with ammonium chloride or acetic acid, [NH2BH3]– accepts a proton, reforming NH3BH3. However, in the reaction with HCl or methanol, N–B bond cleavage occurs. [NH2BH3]– can also donate hydride in some reactions. The possible mechanisms of these reactions are discussed.