| Revision as of 13:50, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 475776710 of page Sodium_acetate for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 13:20, 1 January 2025 edit 2403:a080:c06:db7a:c0c6:2203:6ef1:8832 (talk)No edit summary |
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{{Short description|Chemical compound}} |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{Redirect|Hot ice}} |
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{{chembox |
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{{chembox |
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| Verifiedfields = changed |
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| verifiedrevid = 464392486 |
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| Watchedfields = changed |
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| Name = Sodium acetate |
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| verifiedrevid = 477003809 |
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| ImageFile = Sodium-acetate-2D-skeletal.png |
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| Name = Sodium acetate |
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| ImageSize = 150px |
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| ImageName = Sodium acetate |
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| ImageFile = Sodium-acetate-2D-skeletal.png |
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| IUPACName = Sodium acetate |
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| ImageName = Skeletal formula of sodium acetate |
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| ImageSize = 150px |
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| ImageFileL1 = Acetate-anion-3D-balls.png |
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| ImageFile1 = Sodium-acetate-form-I-xtal-sheet-3D-bs-17.png |
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| ImageSizeL1 = 120px |
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| ImageSize1 = |
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| ImageNameL1 = Ball-and-stick model of the acetate anion |
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| ImageFile2 = Octan sodný.JPG |
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| ImageFileR1 = Sodium-3D.png |
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| ImageName2 = Sodium acetate |
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| ImageSizeR1 = 90px |
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| PIN = Sodium acetate |
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| ImageNameR1 = The sodium cation |
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| SystematicName = Sodium ethanoate |
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| ImageFile2 = Acetate de sodium hydraté.jpg |
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| OtherNames = Hot ice (sodium acetate trihydrate) |
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| SystematicName = Sodium ethanoate |
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|Section1={{Chembox Identifiers |
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| OtherNames = Hot ice (Sodium acetate trihydrate) |
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| index_label = anhydrous |
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| Section1 = {{Chembox Identifiers |
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| index1_label = trihydrate |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = NVG71ZZ7P0 |
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| UNII = NVG71ZZ7P0 |
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| UNII1_Ref = {{fdacite|correct|FDA}} |
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| UNII1 = 4550K0SC9B |
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| ChEMBL_Ref = {{ebicite|correct|EBI}} |
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| ChEMBL_Ref = {{ebicite|correct|EBI}} |
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| ChEMBL = 1354 |
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| ChEMBL = 1354 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI = 32954 |
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| ChEBI = 32954 |
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| ChEBI1 = 32138 |
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| DrugBank = DB09395 |
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| KEGG1 = D01779 |
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| SMILES = .C(=O)C |
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| SMILES = .C(=O)C |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo = 127-09-3 |
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| CASNo = 127-09-3 |
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| CASNo1_Ref = {{cascite|correct|CAS}} |
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| CASNo1 = 6131-90-4 |
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| CASNo1 = 6131-90-4 |
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| CASNo1_Comment = (trihydrate) |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 29105 |
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| ChemSpiderID = 29105 |
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| PubChem = 517045 |
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| PubChem = 517045 |
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| PubChem1 = 23665404 |
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| RTECS = AJ4300010 (anhydrous) <br> AJ4580000 |
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| RTECS = AJ4300010 (anhydrous)<br />AJ4580000 |
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| ATCCode_prefix = B05 |
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| EINECS = 204-823-8 |
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| ATCCode_suffix = XA08 |
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| Gmelin = 20502 |
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| Beilstein = 3595639 |
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}} |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Na = 1 | C = 2| H = 3 | O = 2 |
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| Na=1 | C=2 | H=3 | O=2 |
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| Appearance = White deliquescent powder or crystals |
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| MolarMass = 82.0343 g/mol (anhydrous) <br> 136.0799 g/mol (trihydrate) |
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| Odor = Vinegar (acetic acid) odor when heated to decomposition<ref>{{cite web |url = https://www.cdc.gov/niosh/ipcsneng/neng0565.html |title = Sodium Acetate |work = International Chemical Safety Cards | publisher = National Institute of Occupational Safety and Health|date = 2018-09-18 }}</ref> |
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| Appearance = White deliquescent powder <br> odorless |
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| Density = 1.528 g/cm<sup>3</sup> <br> 1.45 g/cm<sup>3</sup> (trihydrate) |
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| Density = 1.528 g/cm<sup>3</sup> (20 °C, anhydrous)<br/> 1.45 g/cm<sup>3</sup> (20 °C, trihydrate)<ref name=chemister2>{{cite web |url=http://chemister.ru/Database/properties-en.php?dbid=1&id=1510 |title=sodium acetate trihydrate |website=chemister.ru}}</ref> |
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| Solubility = Anhydrous:<br/> 119 g/100 mL (0 °C)<br/> 123.3 g/100 mL (20 °C)<br/> 125.5 g/100 mL (30 °C)<br/> 137.2 g/100 mL (60 °C)<br/> 162.9 g/100 mL (100 °C)<br/> Trihydrate:<br/> 32.9 g/100 mL (-10 °C)<br/> 36.2 g/100 mL (0 °C)<br/> 46.4 g/100 mL (20 °C)<br/> 82 g/100 mL (50 °C)<ref name=sioc>{{cite book |last1 = Seidell |first1 = Atherton |last2 = Linke |first2 = William F. |year = 1952 |title = Solubilities of Inorganic and Organic Compounds |publisher = Van Nostrand}}</ref> |
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| Solubility = 36.2 g/100 ml (0°C) <br> 46.4 g/100 mL (20°C) <br> 139 g/100 mL (60°C) <br> 170.15 g/100 mL (100°C) |
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| SolubleOther = soluble in ] (5.3 g/100 mL (trihydrate) |
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| SolubleOther = Soluble in ], ], ]<ref name=chemister /> |
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| Solubility1 = 16 g/100 g (15 °C)<br/> 16.55 g/100 g (67.7 °C)<ref name=chemister /> |
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| MeltingPt = 324 °C (anhydrous) <br> 58 °C (trihydrate) |
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| Solvent1 = methanol |
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| BoilingPt = 881.4 °C (anhydrous) <br> 122 °C (trihydrate)(decomposes) |
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| Solubility2 = Trihydrate:<br/> 5.3 g/100 mL |
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| pKb = 9.25 |
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| Solvent2 = ethanol |
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| RefractIndex = 1.464 |
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| Solubility3 = 0.5 g/kg (15 °C)<ref name=chemister>{{cite web |url=http://chemister.ru/Database/properties-en.php?dbid=1&id=172 |title=sodium acetate |website=chemister.ru}}</ref> |
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| Solvent3 = acetone |
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| MeltingPtC = 324 |
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| MeltingPt_notes = <br/> (anhydrous)<br/> {{convert|58|C|F K}}<br/> (trihydrate) |
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| BoilingPtC = 881.4 |
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| BoilingPt_notes = <br/> (anhydrous)<br/> {{convert|122|C|F K}}<br/> (trihydrate) decomposes |
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| pKb = 9.25 |
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| RefractIndex = 1.464 |
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| pKa = 24 (20 °C)<ref name=chemister /><br/> 4.75 (when mixed with ] as a buffer)<ref name="sigma">{{Sigma-Aldrich|id=229873|name=Sodium acetate|accessdate=2014-06-07}}</ref> |
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| MagSus = −37.6·10<sup>−6</sup> cm<sup>3</sup>/mol |
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}} |
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| Section3 = {{Chembox Structure |
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|Section3={{Chembox Structure |
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| CrystalStruct = ] |
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| CrystalStruct = ] |
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| Dipole = |
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| Dipole = |
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}} |
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| Section7 = {{Chembox Hazards |
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|Section5={{Chembox Thermochemistry |
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| DeltaHf = −709.32 kJ/mol (anhydrous)<ref name=chemister /><br/> −1604 kJ/mol (trihydrate)<ref name=chemister2 /> |
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| ExternalMSDS = |
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| DeltaGf = −607.7 kJ/mol (anhydrous)<ref name=chemister /> |
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| MainHazards = Irritant |
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| Entropy = 138.1 J/(mol·K) (anhydrous)<ref name=nist>{{nist|name=Acetic acid, sodium salt|id=C127093|accessdate=2014-05-25|mask=FFFF|units=SI}}.</ref><br/> 262 J/(mol·K) (trihydrate)<ref name=chemister2 /> |
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| NFPA-H = 1 |
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| HeatCapacity = 100.83 J/(mol·K) (anhydrous)<ref name=nist /><br/> 229 J/(mol·K) (trihydrate)<ref name=nist2>{{nist|name=Acetic acid, sodium salt, hydrate (1:1:3)|id=C6131904|accessdate=2014-05-25|mask=FFFF|units=SI}}.</ref> |
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}} |
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|Section6={{Chembox Pharmacology |
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| ATCCode_prefix = B05 |
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| ATCCode_suffix = XA08 |
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}} |
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|Section7={{Chembox Hazards |
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| ExternalSDS = |
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| MainHazards = Irritant |
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| NFPA-H = 0 |
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| NFPA-F = 1 |
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| NFPA-F = 1 |
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| NFPA-R = 0 |
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| NFPA-R = 1 |
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| NFPA-O = |
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| NFPA-S = |
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| FlashPt = 250 °C |
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| FlashPt = >{{convert|250|C|F K}} |
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| FlashPt_ref = <ref name="sigma" /> |
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| Autoignition = 607 °C |
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| AutoignitionPtC = 607 |
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| AutoignitionPt_ref = <ref name="sigma" /> |
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| LD50 = 3530 mg/kg (oral, rat)<br/> >10000 mg/kg (rabbit, dermal) |
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| LC50 = >30 g/m<sup>3</sup> (rat, 1 h) |
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| Section8 = {{Chembox Related |
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|Section8={{Chembox Related |
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| OtherAnions = ]<br/>] |
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| OtherAnions = ]<br/> ] |
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| OtherCations = ]<br/>] |
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| OtherCations = ]<br/> ] |
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| OtherCompounds = ] |
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'''Sodium acetate''', CH<sub>3</sub>COONa, also abbreviated ]]],<ref>{{Clayden}}</ref> is the ] ] of ]. This salt is colorless ], and ]. |
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==Applications== |
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===Biotechnological=== |
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Sodium acetate is used as the ] source for culturing ]. Sodium acetate can also be useful for increasing yields of ]. |
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===Industrial=== |
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Sodium acetate is used in the ] industry to neutralize ] waste streams and also as a ] while using ]. It is also a ] agent in chrome ] and helps to impede ] of ] in ] production. It is also used to reduce static electricity during production of disposable cotton pads. |
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===Concrete longevity=== |
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Sodium acetate is used to mitigate water damage to concrete by acting as a ] ], while also being environmentally benign and cheaper than the commonly used ] alternative for sealing concrete against water ].<ref>{{cite news |url=https://www.sciencedaily.com/releases/2007/08/070806101941.htm |title=Potato Chip Flavoring Boosts Longevity Of Concrete |date=8 August 2007 |work=]}}</ref> |
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===Food=== |
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Sodium acetate (anhydrous) is widely used as a shelf-life extending agent and pH-control agent.<ref>{{cite web |title=Food Additive "Sodium Acetate (Anhydrous)" |url=https://www.m-chemical.co.jp/en/products/departments/mcc/emulsifier/product/1206177_8006.html |website=Mitsubishi Chemical Corporation |access-date=16 September 2020 |language=en}}</ref> It is safe to eat at low concentration.<ref>{{cite journal |last1=Mohammadzadeh-Aghdash |first1=Hossein |last2=Sohrabi |first2=Yousef |last3=Mohammadi |first3=Ali |last4=Shanehbandi |first4=Dariush |last5=Dehghan |first5=Parvin |last6=Ezzati Nazhad Dolatabadi |first6=Jafar |title=Safety assessment of sodium acetate, sodium diacetate and potassium sorbate food additives |journal=Food Chemistry |date=15 August 2018 |volume=257 |pages=211–215 |doi=10.1016/j.foodchem.2018.03.020 |pmid=29622200 |s2cid=4596295 |url=https://www.sciencedirect.com/science/article/pii/S0308814618304370 |access-date=16 September 2020 |language=en |issn=0308-8146}}</ref> |
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===Buffer solution=== |
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A solution of sodium acetate (a basic salt of acetic acid) and acetic acid can act as a ] 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). |
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===Heating pad=== |
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] contains a ] of sodium acetate which releases heat upon ]]] |
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Sodium acetate is also used in ]s, ]s, and hot ice. A ] solution of sodium acetate in water is supplied with a device to initiate crystallization, a process that releases substantial heat. |
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] |
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Sodium acetate trihydrate crystals melt at {{Convert|58-58.4|°C|°F}},<ref name="IDMA" /><ref name="Température">{{cite web |author=Courty J.-M., Kierlik É. |title=Les chaufferettes chimiques |lang=fr |work=Pour la Science |date=2008-12-01 |pages=108–110 |url=https://www.pourlascience.fr/sd/physique/les-chaufferettes-chimiques-892.php}}</ref> and the liquid sodium acetate dissolves in the released ]. When heated past the melting point and subsequently allowed to cool, the aqueous solution becomes ]. This solution is capable of cooling to room temperature without forming crystals. By pressing on a metal disc within the heating pad, a ] center is formed, causing the solution to crystallize back into solid sodium acetate trihydrate. The process of crystallization is ].<ref>{{cite web | publisher = ] | url = http://jchemed.chem.wisc.edu/JCESoft/CCA/CCA3/MAIN/ACETATE/PAGE1.HTM | title = Crystallization of Supersaturated Sodium Acetate| date = 2015-07-19 }}</ref> The ] is about 264–289 kJ/kg.<ref name=IDMA>Ibrahim Dincer and Marc A. Rosen. , page 155.</ref> 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.<ref>{{cite web | title = How do sodium acetate heat pads work? | publisher = ] | access-date = 2007-09-03 | url = http://www.howstuffworks.com/question290.htm| date = April 2000 }}</ref> |
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==Preparation== |
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{{Unreferenced section|date=November 2023}} |
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] |
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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 ], commonly in the 5–18% solution known as ], with ] ("washing soda"), ] ("baking soda"), or ] ("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 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. |
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:CH<sub>3</sub>COOH + NaHCO<sub>3</sub> → CH<sub>3</sub>COONa + {{chem|H<sub>2</sub>CO|3}} |
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:{{chem|H<sub>2</sub>CO|3}} → {{chem|CO|2}} + {{chem|H|2|O}} |
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Industrially, sodium acetate trihydrate is prepared by reacting ] with ] using ] as the ]. |
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:CH<sub>3</sub>COOH + NaOH → CH<sub>3</sub>COONa + H<sub>2</sub>O. |
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To manufacture anhydrous sodium acetate industrially, the Niacet Process is used. Sodium metal ingots are extruded through a die to form a ribbon of ] metal, usually under an inert gas atmosphere such as N<sub>2</sub> then immersed in anhydrous ]. |
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:2 CH<sub>3</sub>COOH + 2 Na →2 CH<sub>3</sub>COONa + H<sub>2</sub>. |
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The ] gas is normally a valuable byproduct. |
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==Structure== |
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The ] of ] sodium acetate has been described as alternating sodium-carboxylate and ] layers.<ref name="Hsu&Nordman">{{ cite journal | journal = ] | year = 1983 | volume = 39 | pages = 690–694 | first1 = Leh-Yeh | last1 = Hsu | first2 = C. E. | last2 = Nordman | title = Structures of two forms of sodium acetate, Na<sup>+</sup>.C<sub>2</sub>H<sub>3</sub>O<sub>2</sub><sup>−</sup> | issue = 6 | doi = 10.1107/S0108270183005946 | bibcode = 1983AcCrC..39..690H }}</ref> Sodium acetate ]'s structure consists of distorted octahedral coordination at sodium. Adjacent octahedra share edges to form one-dimensional chains. ] in two dimensions between acetate ions and ] links the chains into a three-dimensional network.<ref name="CameronMannanRahman">{{ cite journal | journal = ] | year = 1976 | volume = 32 | pages = 87–90 | first1 = T. S. | last1 = Cameron | first2 = K. M. | last2 = Mannan | first3 = M. O. | last3 = Rahman | title = The crystal structure of sodium acetate trihydrate | issue = 1 | doi = 10.1107/S0567740876002367 | bibcode = 1976AcCrB..32...87C }}</ref><ref name="Wei&Ward">{{ cite journal | journal = ] | year = 1977 | volume = 33 | pages = 522–526 | first1 = K.-T. | last1 = Wei | first2 = D. L. | last2 = Ward | title = Sodium acetate trihydrate: a redetermination | issue = 2 | doi = 10.1107/S0567740877003975 | bibcode = 1977AcCrB..33..522W }}</ref> |
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{| class="wikitable" style="margin:1em auto; text-align:center;" |
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|+Comparison of anhydrous and trihydrate crystal structures |
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|- |
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! Degree of hydration |
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! Anhydrous<ref name="Hsu&Nordman" /> |
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! Trihydrate<ref name="CameronMannanRahman" /><ref name="Wei&Ward" /> |
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! Na coordination |
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| ] |
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| ] |
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! Strongly bonded aggregation |
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| ]<br />2D sheet |
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| ]<br />1D chain |
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|- |
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! Weakly bonded aggregation |
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| ]<br />sheets stacked with<br />hydrophobic surfaces in contact |
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| ]<br />chains linked by hydrogen bonds<br />(one chain highlighted in light blue) |
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|- |
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==Reactions== |
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Sodium acetate can be used to form an ] with an alkyl halide such as ]: |
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: CH<sub>3</sub>COONa + BrCH<sub>2</sub>CH<sub>3</sub> → ] + ] |
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Sodium acetate undergoes decarboxylation to form methane (CH<sub>4</sub>) under forcing conditions (pyrolysis in the presence of sodium hydroxide): |
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: CH<sub>3</sub>COONa + NaOH → CH<sub>4</sub> + Na<sub>2</sub>CO<sub>3</sub> |
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Calcium oxide is the typical catalyst used for this reaction. |
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Cesium salts also catalyze this reaction.{{citation needed|date=January 2020}} |
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==References== |
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{{Reflist}} |
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==External links== |
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{{Commons category|Sodium acetate}} |
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* |
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* |
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*{{cite web|last=Lavars|first=Nick|date=2021-09-15|title=Sodium acetate acts as a potential fountain of youth for aging bones|url=https://newatlas.com/medical/sodium-acetate-potential-fountain-youth-aging-bones/|access-date=2021-09-16|website=New Atlas|language=en-US}} |
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{{Sodium compounds}} |
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{{Acetates}} |
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{{Authority control}} |
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] |
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] |
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] |