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Sodium acetate

Sodium acetate, CH3COONa, also abbreviated NaOAc,[8] is the sodium salt of acetic acid. This colorless deliquescent salt has a wide range of uses.

Sodium acetate
Names
Preferred IUPAC name
Sodium acetate
Other names
Hot ice (sodium acetate trihydrate)
Identifiers
  • anhydrous: 127-09-3 Y
  • trihydrate: 6131-90-4 Y
3D model (JSmol)
  • anhydrous: Interactive image
3595639
ChEBI
  • anhydrous: CHEBI:32954 Y
  • trihydrate: CHEBI:32138
ChEMBL
  • anhydrous: ChEMBL1354 Y
ChemSpider
  • anhydrous: 29105 Y
DrugBank
  • anhydrous: DB09395
ECHA InfoCard 100.004.386
EC Number
  • anhydrous: 204-823-8
E number E262 (preservatives)
20502
KEGG
  • trihydrate: D01779
  • anhydrous: 517045
  • trihydrate: 23665404
RTECS number
  • anhydrous: AJ4300010 (anhydrous)
    AJ4580000
UNII
  • anhydrous: NVG71ZZ7P0 Y
  • trihydrate: 4550K0SC9B Y
  • anhydrous: DTXSID2027044
  • InChI=1S/C2H4O2.Na/c1-2(3)4;/h1H3,(H,3,4);/q;+1/p-1 Y
    Key: VMHLLURERBWHNL-UHFFFAOYSA-M Y
  • anhydrous: InChI=1/C2H4O2.Na/c1-2(3)4;/h1H3,(H,3,4);/q;+1/p-1
    Key: VMHLLURERBWHNL-REWHXWOFAT
  • anhydrous: [Na+].[O-]C(=O)C
Properties
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
Anhydrous:
119 g/100 mL (0 °C)
123.3 g/100 mL (20 °C)
125.5 g/100 mL (30 °C)
137.2 g/100 mL (60 °C)
162.9 g/100 mL (100 °C)
Trihydrate:
32.9 g/100 mL (-10 °C)
36.2 g/100 mL (0 °C)
46.4 g/100 mL (20 °C)
82 g/100 mL (50 °C)[3]
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) 51 (20 °C)[4]
4.75 (when mixed with CH3COOH as a buffer)[5]
Basicity (pKb) 9.25
−37.6·10−6 cm3/mol
1.464
Structure
Monoclinic
Thermochemistry
100.83 J/mol·K (anhydrous)[6]
229 J/mol·K (trihydrate)[7]
138.1 J/mol·K (anhydrous)[6]
262 J/mol·K (trihydrate)[2]
−709.32 kJ/mol (anhydrous)[4]
−1604 kJ/mol (trihydrate)[2]
−607.7 kJ/mol (anhydrous)[4]
Pharmacology
B05XA08 (WHO)
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Irritant
NFPA 704 (fire diamond)
1
1
0
Flash point >250 °C (482 °F; 523 K)[5]
600 °C (1,112 °F; 873 K)[5]
Lethal dose or concentration (LD, LC):
3530 mg/kg (oral, rat)
Safety data sheet (SDS) External MSDS
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).
N verify (what is YN ?)

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 flavour, and may be used as a substitute for vinegar itself on potato chips as it doesn't add moisture to the final product.[11] Sodium acetate (anhydrous) is widely used as a shelf-life extending agent, pH control agent[12] It is safe to eat at low concentration.[13]

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 58–58.4 °C (136.4–137.1 °F),[14][15] 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.[16] The latent heat of fusion is about 264–289 kJ/kg.[14] 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.[17]

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 the 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
2
O

Industrially, sodium acetate trihydrate is prepared by reacting acetic acid with sodium hydroxide using water as the solvent.

CH3COOH + NaOH → CH3COONa + H2O

Structure

The crystal structure of anhydrous sodium acetate has been described as alternating sodium-carboxylate and methyl group layers.[18] Sodium acetate trihydrate's structure consists of distorted octahedral coordination at sodium. Adjacent octahedra share edges to form one-dimensional chains. Hydrogen bonding in two dimensions between acetate ions and water of hydration links the chains into a three-dimensional network.[19][20]

Comparison of anhydrous and trihydrate crystal structures
Degree of hydration Na coordination Strongly bonded aggregation Weakly bonded aggregation
Anhydrous[18]    
2D sheet
 
sheets stacked with
hydrophobic surfaces in contact
Trihydrate[19][20]    
1D chain
 
chains linked by hydrogen bonds
(one chain highlighted in light blue)

Reactions

Sodium acetate can be used to form an ester with an alkyl halide such as bromoethane:

CH3COONa + BrCH2CH3CH3COOCH2CH3 + 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. Cesium salts also catalyze this reaction.[citation needed]

References

  1. ^ "Sodium Acetate". International Chemical Safety Cards. National Institute of Occupational Safety and Health. 2018-09-18.
  2. ^ a b c "sodium acetate trihydrate". chemister.ru.
  3. ^ Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand.
  4. ^ a b c d e f "sodium acetate". chemister.ru.
  5. ^ a b c Sigma-Aldrich Co., Sodium acetate. Retrieved on 2014-06-07.
  6. ^ a b Acetic acid, sodium salt in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD) (retrieved 2014-05-25)
  7. ^ Acetic acid, sodium salt, hydrate (1:1:3) in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD) (retrieved 2014-05-25)
  8. ^ Clayden, Jonathan; Greeves, Nick; Warren, Stuart; Wothers, Peter (2001). Organic Chemistry (1st ed.). Oxford University Press. ISBN 978-0-19-850346-0.
  9. ^ "Potato Chip Flavoring Boosts Longevity Of Concrete". Science Daily. 8 August 2007.
  10. ^ AG, Jungbunzlauer Suisse. "Sodium Diacetate – Jungbunzlauer". www.jungbunzlauer.com.
  11. ^ Austen, Ian (2018-06-09). "The Secret Story of Salt and Vinegar Chips: the Canada Letter". The New York Times. ISSN 0362-4331. Retrieved 2021-11-23.
  12. ^ "Food Additive "Sodium Acetate (Anhydrous)" | Products". Mitsubishi Chemical Corporation. Retrieved 16 September 2020.
  13. ^ Mohammadzadeh-Aghdash, Hossein; Sohrabi, Yousef; Mohammadi, Ali; Shanehbandi, Dariush; Dehghan, Parvin; Ezzati Nazhad Dolatabadi, Jafar (15 August 2018). "Safety assessment of sodium acetate, sodium diacetate and potassium sorbate food additives". Food Chemistry. 257: 211–215. doi:10.1016/j.foodchem.2018.03.020. ISSN 0308-8146. PMID 29622200. S2CID 4596295. Retrieved 16 September 2020.
  14. ^ a b Ibrahim Dincer and Marc A. Rosen. Thermal Energy Storage: Systems and Applications, page 155
  15. ^ Courty JM, Kierlik E, Les chaufferettes chimiques, Pour la Science, décembre 2008, pp. 108–110
  16. ^ "Crystallization of Supersaturated Sodium Acetate". Journal of Chemical Education. 2015-07-19.
  17. ^ "How do sodium acetate heat pads work?". HowStuffWorks. April 2000. Retrieved 2007-09-03.
  18. ^ a b Hsu, Leh-Yeh; Nordman, C. E. (1983). "Structures of two forms of sodium acetate, Na+.C2H3O2". Acta Crystallogr. C. 39 (6): 690–694. doi:10.1107/S0108270183005946.
  19. ^ a b Cameron, T. S.; Mannan, K. M.; Rahman, M. O. (1976). "The crystal structure of sodium acetate trihydrate". Acta Crystallogr. B. 32: 87–90. doi:10.1107/S0567740876002367.
  20. ^ a b Wei, K.-T.; Ward, D. L. (1977). "Sodium acetate trihydrate: a redetermination". Acta Crystallogr. B. 33 (2): 522–526. doi:10.1107/S0567740877003975.

External links

  • Hot Ice – Instructions, Pictures, and Videos
  • How Sodium Acetate heating pads work
  • Lavars, Nick (2021-09-15). "Sodium acetate acts as a potential fountain of youth for aging bones". New Atlas. Retrieved 2021-09-16.{{cite web}}: CS1 maint: url-status (link)

sodium, acetate, redirects, here, other, uses, disambiguation, ch3coona, also, abbreviated, naoac, sodium, salt, acetic, acid, this, colorless, deliquescent, salt, wide, range, uses, namespreferred, iupac, name, other, names, sodium, acetate, trihydrate, ident. Hot ice redirects here For other uses see Hot ice disambiguation Sodium acetate CH3COONa also abbreviated NaOAc 8 is the sodium salt of acetic acid This colorless deliquescent salt has a wide range of uses Sodium acetate NamesPreferred IUPAC name Sodium acetateOther names Hot ice sodium acetate trihydrate IdentifiersCAS Number anhydrous 127 09 3 Ytrihydrate 6131 90 4 Y3D model JSmol anhydrous Interactive imageBeilstein Reference 3595639ChEBI anhydrous CHEBI 32954 Ytrihydrate CHEBI 32138ChEMBL anhydrous ChEMBL1354 YChemSpider anhydrous 29105 YDrugBank anhydrous DB09395ECHA InfoCard 100 004 386EC Number anhydrous 204 823 8E number E262 preservatives Gmelin Reference 20502KEGG trihydrate D01779PubChem CID anhydrous 517045trihydrate 23665404RTECS number anhydrous AJ4300010 anhydrous AJ4580000UNII anhydrous NVG71ZZ7P0 Ytrihydrate 4550K0SC9B YCompTox Dashboard EPA anhydrous DTXSID2027044InChI InChI 1S C2H4O2 Na c1 2 3 4 h1H3 H 3 4 q 1 p 1 YKey VMHLLURERBWHNL UHFFFAOYSA M Yanhydrous InChI 1 C2H4O2 Na c1 2 3 4 h1H3 H 3 4 q 1 p 1Key VMHLLURERBWHNL REWHXWOFATSMILES anhydrous Na O C O CPropertiesChemical formula C 2H 3Na O 2Molar mass 82 034 g mol 1Appearance White deliquescent powderOdor 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 decomposesSolubility in water Anhydrous 119 g 100 mL 0 C 123 3 g 100 mL 20 C 125 5 g 100 mL 30 C 137 2 g 100 mL 60 C 162 9 g 100 mL 100 C Trihydrate 32 9 g 100 mL 10 C 36 2 g 100 mL 0 C 46 4 g 100 mL 20 C 82 g 100 mL 50 C 3 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 mLSolubility in acetone 0 5 g kg 15 C 4 Acidity pKa 51 20 C 4 4 75 when mixed with CH3COOH as a buffer 5 Basicity pKb 9 25Magnetic susceptibility x 37 6 10 6 cm3 molRefractive index nD 1 464StructureCrystal structure MonoclinicThermochemistryHeat capacity C 100 83 J mol K anhydrous 6 229 J mol K trihydrate 7 Std molarentropy S 298 138 1 J mol K anhydrous 6 262 J mol K trihydrate 2 Std enthalpy offormation DfH 298 709 32 kJ mol anhydrous 4 1604 kJ mol trihydrate 2 Gibbs free energy DfG 607 7 kJ mol anhydrous 4 PharmacologyATC code B05XA08 WHO HazardsOccupational safety and health OHS OSH Main hazards IrritantNFPA 704 fire diamond 110Flash point gt 250 C 482 F 523 K 5 Autoignitiontemperature 600 C 1 112 F 873 K 5 Lethal dose or concentration LD LC LD50 median dose 3530 mg kg oral rat Safety data sheet SDS External MSDSRelated compoundsOther anions Sodium formate Sodium propionateOther cations Potassium acetate Calcium acetateRelated compounds Sodium diacetateExcept where otherwise noted data are given for materials in their standard state at 25 C 77 F 100 kPa N verify what is Y N Infobox references 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 Structure 4 Reactions 5 References 6 External linksApplications EditBiotechnological Edit 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 Edit 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 Edit 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 Edit 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 flavour and may be used as a substitute for vinegar itself on potato chips as it doesn t add moisture to the final product 11 Sodium acetate anhydrous is widely used as a shelf life extending agent pH control agent 12 It is safe to eat at low concentration 13 Buffer solution Edit 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 Edit 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 58 58 4 C 136 4 137 1 F 14 15 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 16 The latent heat of fusion is about 264 289 kJ kg 14 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 17 Preparation Edit 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 the 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 H2CO3 H2CO3 CO2 H2 OIndustrially sodium acetate trihydrate is prepared by reacting acetic acid with sodium hydroxide using water as the solvent CH3COOH NaOH CH3COONa H2OStructure EditThe crystal structure of anhydrous sodium acetate has been described as alternating sodium carboxylate and methyl group layers 18 Sodium acetate trihydrate s structure consists of distorted octahedral coordination at sodium Adjacent octahedra share edges to form one dimensional chains Hydrogen bonding in two dimensions between acetate ions and water of hydration links the chains into a three dimensional network 19 20 Comparison of anhydrous and trihydrate crystal structures Degree of hydration Na coordination Strongly bonded aggregation Weakly bonded aggregationAnhydrous 18 2D sheet sheets stacked withhydrophobic surfaces in contactTrihydrate 19 20 1D chain chains linked by hydrogen bonds one chain highlighted in light blue Reactions EditSodium acetate can be used to form an ester with an alkyl halide such as bromoethane CH3COONa BrCH2CH3 CH3COOCH2CH3 NaBrSodium acetate undergoes decarboxylation to form methane CH4 under forcing conditions pyrolysis in the presence of sodium hydroxide CH3COONa NaOH CH4 Na2CO3Calcium oxide is the typical catalyst used for this reaction Cesium salts also catalyze this reaction citation needed References Edit Sodium Acetate International Chemical Safety Cards National Institute of Occupational Safety and Health 2018 09 18 a b c sodium acetate trihydrate chemister ru Seidell Atherton Linke William F 1952 Solubilities of Inorganic and Organic Compounds Van Nostrand a b c d e f sodium acetate chemister ru a b c Sigma Aldrich Co Sodium acetate Retrieved on 2014 06 07 a b Acetic acid sodium salt in Linstrom Peter J Mallard William G eds NIST Chemistry WebBook NIST Standard Reference Database Number 69 National Institute of Standards and Technology Gaithersburg MD retrieved 2014 05 25 Acetic acid sodium salt hydrate 1 1 3 in Linstrom Peter J Mallard William G eds NIST Chemistry WebBook NIST Standard Reference Database Number 69 National Institute of Standards and Technology Gaithersburg MD retrieved 2014 05 25 Clayden Jonathan Greeves Nick Warren Stuart Wothers Peter 2001 Organic Chemistry 1st ed Oxford University Press ISBN 978 0 19 850346 0 Potato Chip Flavoring Boosts Longevity Of Concrete Science Daily 8 August 2007 AG Jungbunzlauer Suisse Sodium Diacetate Jungbunzlauer www jungbunzlauer com Austen Ian 2018 06 09 The Secret Story of Salt and Vinegar Chips the Canada Letter The New York Times ISSN 0362 4331 Retrieved 2021 11 23 Food Additive Sodium Acetate Anhydrous Products Mitsubishi Chemical Corporation Retrieved 16 September 2020 Mohammadzadeh Aghdash Hossein Sohrabi Yousef Mohammadi Ali Shanehbandi Dariush Dehghan Parvin Ezzati Nazhad Dolatabadi Jafar 15 August 2018 Safety assessment of sodium acetate sodium diacetate and potassium sorbate food additives Food Chemistry 257 211 215 doi 10 1016 j foodchem 2018 03 020 ISSN 0308 8146 PMID 29622200 S2CID 4596295 Retrieved 16 September 2020 a b Ibrahim Dincer and Marc A Rosen Thermal Energy Storage Systems and Applications page 155 Courty JM Kierlik E Les chaufferettes chimiques Pour la Science decembre 2008 pp 108 110 Crystallization of Supersaturated Sodium Acetate Journal of Chemical Education 2015 07 19 How do sodium acetate heat pads work HowStuffWorks April 2000 Retrieved 2007 09 03 a b Hsu Leh Yeh Nordman C E 1983 Structures of two forms of sodium acetate Na C2H3O2 Acta Crystallogr C 39 6 690 694 doi 10 1107 S0108270183005946 a b Cameron T S Mannan K M Rahman M O 1976 The crystal structure of sodium acetate trihydrate Acta Crystallogr B 32 87 90 doi 10 1107 S0567740876002367 a b Wei K T Ward D L 1977 Sodium acetate trihydrate a redetermination Acta Crystallogr B 33 2 522 526 doi 10 1107 S0567740877003975 External links Edit Wikimedia Commons has media related to Sodium acetate Hot Ice Instructions Pictures and Videos How Sodium Acetate heating pads work Lavars Nick 2021 09 15 Sodium acetate acts as a potential fountain of youth for aging bones New Atlas Retrieved 2021 09 16 a href Template Cite web html title Template Cite web cite web a CS1 maint url status link Retrieved from https en wikipedia org w index php title Sodium acetate amp oldid 1121732946, wikipedia, wiki, book, books, library,

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