Sodium acetate - wikipedia Sodium acetate This article is about sodium acetate. For other uses of hot ice, see Hot ice ( disambiguation ). 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 trihydrate : 6131 - 90 - 4 3D model ( JSmol ) anhydrous : Interactive image Beilstein Reference 3595639 ChEBI anhydrous : CHEBI : 32954 trihydrate : CHEBI : 32138 ChEMBL anhydrous : ChEMBL1354 ChemSpider anhydrous : 29105 ECHA InfoCard 100.004. 386 EC Number 204 - 823 - 8 E number E262 ( preservatives ) Gmelin Reference 20502 KEGG trihydrate : D01779 PubChem CID anhydrous : 517045 trihydrate : 23665404 RTECS number AJ4300010 ( anhydrous ) AJ4580000 UNII anhydrous : NVG71ZZ7P0 trihydrate : 4550K0SC9B InChI InChI = 1S / C2H4O2.Na/c1-2 ( 3 ) 4 ; / h1H3, ( H, 3, 4 ) ; / q ; + 1 / p - 1 Key : VMHLLURERBWHNL - UHFFFAOYSA - M anhydrous : InChI = 1 / C2H4O2.Na/c1-2 ( 3 ) 4 ; / h1H3, ( H, 3, 4 ) ; / q ; + 1 / p - 1 Key : VMHLLURERBWHNL - REWHXWOFAT SMILES anhydrous : ( Na+ ). ( O - ) C ( = O ) C Properties Chemical formula C H Na O Molar mass 82.03 g mol Appearance White deliquescent powder Odor Vinegar ( acetic acid ) odor when heated to decomposition Density 1.528 g / cm ( 20 ° C, anhydrous ) 1.45 g / cm ( 20 ° C, trihydrate ) 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 : 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 ) Solubility Soluble in alcohol, hydrazine, SO Solubility in methanol 16 g / 100 g ( 15 ° C ) 16.55 g / 100 g ( 67.7 ° C ) Solubility in ethanol Trihydrate : 5.3 g / 100 mL Solubility in acetone 0.5 g / kg ( 15 ° C ) Acidity ( pK ) 24 ( 20 ° C ) 4.75 CH COOH Basicity ( pK ) 9.25 Magnetic susceptibility ( χ ) − 37.6 10 cm / mol Refractive index ( n ) 1.464 Structure Crystal structure Monoclinic Thermochemistry Specific heat capacity ( C ) 100.83 J / mol K ( anhydrous ) 229 J / mol K ( trihydrate ) Std molar entropy ( S ) 138.1 J / mol K ( anhydrous ) 262 J / mol K ( trihydrate ) Std enthalpy of formation ( Δ H ) − 709.32 kJ / mol ( anhydrous ) − 1604 kJ / mol ( trihydrate ) Gibbs free energy ( Δ G  ̊ ) − 607.7 kJ / mol ( anhydrous ) Pharmacology ATC code B05XA08 ( WHO ) Hazards Main hazards Irritant Safety data sheet External MSDS NFPA 704 0 Flash point > 250 ° C ( 482 ° F ; 523 K ) Autoignition temperature 600 ° C ( 1,112 ° F ; 873 K ) Lethal dose or concentration ( LD, LC ) : LD ( 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 ). verify ( what is ? ) Infobox references Sodium acetate, CH COONa, also abbreviated Na O Ac, is the sodium salt of acetic acid. This colorless deliquescent salt has a wide range of uses. Contents 1 Applications 1.1 Industrial 1.2 Concrete longevity 1.3 Food 1.4 Buffer solution 1.5 Heating pad 2 Preparation 3 Reactions 4 References 5 External links Applications 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. 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, given the E-number E262. It is often used to give potato chips a salt and vinegar flavor. 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 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 ( to 137.12 ° F / 58.4 ° C ), 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. The latent heat of fusion is about 264 -- 289 kJ / kg. 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. 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. CH COOH + NaHCO → CH COONa + H CO H CO → CO + H O Industrially, sodium acetate trihydrate is prepared by reacting acetic acid with sodium hydroxide using water as the solvent. CH COOH + NaOH → CH COONa + H O Reactions Sodium acetate can be used to form an ester with an alkyl halide such as bromoethane : CH COONa + BrCH CH → CH COOCH CH + NaBr Sodium acetate undergoes decarboxylation to form methane ( CH ) under forcing conditions ( pyrolysis in the presence of sodium hydroxide ) : CH COONa + NaOH → CH + Na CO Caesium salts catalyze this reaction. References Jump up ^ `` Sodium Acetate ''. International Chemical Safety Cards. National Institute of Occupational Safety and Health. ^ Jump up to : `` sodium acetate trihydrate ''. chemister.ru. Jump up ^ Seidell, Atherton ; Linke, William F. ( 1952 ). Solubilities of Inorganic and Organic Compounds. Van Nostrand. ^ Jump up to : `` sodium acetate ''. chemister.ru. ^ Jump up to : Sigma - Aldrich Co., Sodium acetate. Retrieved on 2014 - 06 - 07. ^ Jump up to : 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 ), http://webbook.nist.gov ( retrieved 2014 - 05 - 25 ) Jump up ^ 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 ), http://webbook.nist.gov ( retrieved 2014 - 05 - 25 ) Jump up ^ Clayden, Jonathan ; Greeves, Nick ; Warren, Stuart ; Wothers, Peter ( 2001 ). Organic Chemistry ( 1st ed. ). Oxford University Press. ISBN 978 - 0 - 19 - 850346 - 0. Jump up ^ `` Potato Chip Flavoring Boosts Longevity Of Concrete ''. Science Daily. 8 August 2007. Jump up ^ AG, Jungbunzlauer Suisse. `` Sodium Diacetate - Jungbunzlauer ''. www.jungbunzlauer.com. ^ Jump up to : Ibrahim Dincer and Marc A. Rosen. Thermal Energy Storage : Systems and Applications, page 155 Jump up ^ Courty JM, Kierlik E, Les chaufferettes chimiques, Pour la Science, décembre 2008, p 108 - 110 Jump up ^ `` Crystallization of Supersaturated Sodium Acetate ''. Journal of Chemical Education. Jump up ^ `` Fake latent heat and supersaturation ) ''. www.atmos.washington.edu. Jump up ^ `` How do sodium acetate heat pads work ? ''. HowStuffWorks. Retrieved 2007 - 09 - 03. External links Wikimedia Commons has media related to Sodium acetate. Hot Ice -- Instructions, Pictures, and Videos How Sodium Acetate heating pads work Sodium compounds NaAlO NaBH NaBH ( CN ) NaBO NaBiO NaBr NaBrO NaBrO NaCH COO NaC H CO NaC H ( OH ) CO NaCN NaCl NaClO NaClO NaClO NaClO NaF Na FeO NaH NaHCO NaH PO NaHSO NaHSO NaI NaIO NaIO Na IO NaMnO NaN NaNH NaNO NaNO NaOCN NaO NaO NaOH NaPO H NaReO NaSCN NaSH NaTcO NaVO Na CO Na C O Na CrO Na Cr O Na GeO Na MnO Na MnO Na MoO Na MoS Na N O Na O Na O Na O ( UO ) Na PO F Na S Na SO Na SO Na S O Na S O Na S O Na S O Na S O Na S O Na S O Na Se Na SeO Na SeO Na SiO Na Si O Na SiO Na Te Na TeO Na TeO Na Po Na Ti O Na U O Na WO Na Zn ( OH ) Na N Na P Na PO Na VO Na Fe ( CN ) Na P O Na P O Chemical formulas Acetyl halides and salts of the acetate ion AcOH He LiOAc Be ( OAc ) BeAcOH B ( OAc ) AcOAc ROAc NH OAc AcOOH FAc Ne NaOAc Mg ( OAc ) Al ( OAc ) ALSOL Al ( OAc ) OH Al SO ( OAc ) Si ClAc Ar KOAc Ca ( OAc ) Sc ( OAc ) Ti ( OAc ) VO ( OAc ) Cr ( OAc ) Mn ( OAc ) Mn ( OAc ) Fe ( OAc ) Fe ( OAc ) Co ( OAc ), Co ( OAc ) Ni ( OAc ) Cu ( OAc ) Zn ( OAc ) Ga ( OAc ) Ge As ( OAc ) Se BrAc Kr RbOAc Sr ( OAc ) Y ( OAc ) Zr ( OAc ) Nb Mo ( OAc ) Tc Ru ( OAc ) Ru ( OAc ) Ru ( OAc ) Rh ( OAc ) Pd ( OAc ) AgOAc Cd ( OAc ) In Sn ( OAc ) Sn ( OAc ) Sb ( OAc ) Te IAc Xe CsOAc Ba ( OAc ) Hf Ta Re Os Ir Pt ( OAc ) Au Hg ( OAc ), Hg ( OAc ) TlOAc Tl ( OAc ) Pb ( OAc ) Pb ( OAc ) Bi ( OAc ) Po At Rn Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og ↓ La ( OAc ) Ce ( OAc ) Pr Nd Pm Sm ( OAc ) Eu ( OAc ) Gd ( OAc ) Tb Dy ( OAc ) Ho ( OAc ) Er Tm Yb ( OAc ) Lu ( OAc ) Ac Th Pa UO ( OAc ) Np Pu Am Cm Bk Cf Es Fm Md No Lr Retrieved from `` https://en.wikipedia.org/w/index.php?title=Sodium_acetate&oldid=842423880 '' Categories : Acetates Organic sodium salts Food additives Photographic chemicals Hidden categories : Chemical articles with multiple compound IDs Chemicals using indexlabels Chemical articles with multiple CAS registry numbers Chemical articles with multiple PubChem CIDs Chemical articles with multiple ChEBIs Articles with changed CASNo identifier ECHA InfoCard ID from Wikidata E number from Wikidata Articles containing unverified chemical infoboxes Chembox image size set Talk Contents About Wikipedia تۆرکجه Български Bosanski Català Čeština Dansk Deutsch Eesti Español Esperanto فارسی Français 한국어 Hrvatski Bahasa Indonesia Italiano עברית Magyar Nederlands 日本 語 Norsk Polski Português Română Русский Scots Slovenčina Slovenščina Српски / srpski Srpskohrvatski / српскохрватски Suomi Svenska தமிழ் తెలుగు Türkçe Українська Tiếng Việt 中文 30 more Edit links This page was last edited on 22 May 2018, at 10 : 35. 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Question: what is the chemical name of ch3 c o o n a
Answer: Sodium acetate