| Revision as of 06:53, 23 September 2011 editCheMoBot (talk | contribs)Bots141,565 edits Updating {{chembox}} (no changed fields - added verified revid - updated 'ChemSpiderID_Ref', 'DrugBank_Ref', 'UNII_Ref', 'ChEMBL_Ref', 'ChEBI_Ref', 'KEGG_Ref', 'StdInChI_Ref', 'StdInChIKey_Ref', 'ChEBI_Ref') per [[WP:CHEMVALID|Chem/Drugbox validation← Previous edit |
Latest revision as of 13:22, 14 September 2024 edit undoPygos (talk | contribs)Extended confirmed users, New page reviewers2,306 editsNo edit summary |
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{{chembox |
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| verifiedrevid = 435209329 |
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| verifiedrevid = 451980637 |
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| ImageFileL1 = Sodium-3D.png |
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| ImageFileL1 = Sodium-3D.png |
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| ImageSizeL1 = 90px |
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| ImageNameL1 = The sodium cation |
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| ImageNameL1 = The sodium cation |
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| ImageFileR1 = Tetrafluoroborate-ion-3D-balls.png |
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| ImageFileR1 = Tetrafluoroborate-ion-3D-balls.png |
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| ImageSizeR1 = 110px |
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| ImageNameR1 = The tetrafluoroborate anion (ball-and-stick model) |
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| ImageNameR1 = The tetrafluoroborate anion (ball-and-stick model) |
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| OtherNames = sodium fluoroborate, NaBF4 |
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| OtherNames = sodium fluoroborate, NaBF4 |
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| Section1 = {{Chembox Identifiers |
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| Section1 = {{Chembox Identifiers |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo = 13755-29-8 |
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| CASNo = 13755-29-8 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = CFC805A5WR |
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| PubChem = 4343483 |
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| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} |
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| ChemSpiderID = 24462 |
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| InChI = 1S/BF4.Na/c2-1(3,4)5;/q-1;+1 |
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| SMILES = (F)(F)(F)F. |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| Formula = NaBF<sub>4</sub> |
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| Formula = NaBF<sub>4</sub> |
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| MolarMass = 109.79 |
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| MolarMass = 109.794 g/mol |
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| MeltingPt = 384 °C |
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| MeltingPtC = 384 |
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| Density = 2.47 g/cm<sup>3</sup> |
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| Section3 = {{Chembox Hazards |
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'''Sodium tetrafluoroborate''', also called '''sodium borofluoride''', is a ] with formula NaBF<sub>4</sub>. It forms colorless water-soluble ] crystals and is soluble in water (108 g/100 ml) and less soluble in organic solvents.<ref>{{Kirjaviite | Tekijä = George W. A. Milne | Nimeke =Gardner's commercially important chemicals | Vuosi =2005 |Sivu =564 |Julkaisija =John Wiley and Sons | Tunniste = ISBN 978-0-471-73518-2 | www =http://books.google.fi/books?id=oWdc2qcb3QsC&pg=PA564&dq=Sodium+tetrafluoroborate&cd=5#v=onepage&q=Sodium%20tetrafluoroborate&f=false | www-teksti =Kirja Googlen teoshaussa | Viitattu =16.01.2010 | Kieli ={{en}}}}</ref> |
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'''Sodium tetrafluoroborate''' is an ] with formula NaBF<sub>4</sub>. It is a salt that forms colorless or white ] crystals and is soluble in water (108 g/100 mL) but less soluble in organic solvents.<ref>{{cite book | url = https://books.google.com/books?id=oWdc2qcb3QsC&q=Sodium+tetrafluoroborate&pg=PA564 | title = Gardner's Commercially Important Chemicals: Synonyms, Trade Names, and Properties | isbn = 9780471735182 | last1 = Milne | first1 = G. W. A | date = 2005-07-11| publisher = John Wiley & Sons }}</ref> |
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Sodium tetrafluoroborate is used in some ] used for ] and to produce ].<ref name="Georg">{{cite book|last=Brauer|first=Georg|title=Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed.|date=1963|publisher=Academic Press|location=New York|isbn=978-0121266011|page=220 & 222|url=https://books.google.com/books?id=TLYatwAACAAJ&q=Handbook+of+Preparative+Inorganic+Chemistry}}</ref> |
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It is a source of ] anion. It is used in ] for ] reactions and as a ], and for lab-scale preparation of ]. |
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==Preparation== |
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Sodium tetrafluoroborate is used in some ] used for ]. |
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Sodium tetrafluoroborate can be prepared by neutralizing ] with ] or ].<ref name ="concise">{{cite book | url = https://books.google.com/books?id=Owuv-c9L_IMC&q=Sodium+tetrafluoroborate&pg=PA1001 | title = Concise Encyclopedia Chemistry | isbn = 9783110114515 | last1 = Eagleson | first1 = Mary | year = 1994| publisher = Walter de Gruyter }}</ref> |
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:NaOH + HBF<sub>4</sub> → NaBF<sub>4</sub> + H<sub>2</sub>O |
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:Na<sub>2</sub>CO<sub>3</sub> + 2 HBF<sub>4</sub> → 2 NaBF<sub>4</sub> + H<sub>2</sub>O + CO<sub>2</sub> |
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Alternatively the chemical can be synthesized from ], ], and sodium carbonate:<ref name="Georg" /> |
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:2H<sub>3</sub>BO<sub>3</sub> + 8HF + Na<sub>2</sub>CO<sub>3</sub> → 2NaBF<sub>4</sub> + 7H<sub>2</sub>O + CO<sub>2</sub> |
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Sodium tetrafluoroborate can be prepared by neutralizing ] with ] or ]. <ref name ="concise">{{Kirjaviite | Tekijä =Thomas Scott, Mary Eagleson | Nimeke =Concise encyclopedia chemistry | Vuosi =1994 |Sivu =1001 |Julkaisija =Walter de Gruyter | Tunniste = ISBN 978-3110114515 | www =http://books.google.fi/books?id=Owuv-c9L_IMC&pg=PA1001&dq=Sodium+tetrafluoroborate&lr=&cd=19#v=onepage&q=Sodium%20tetrafluoroborate&f=false | www-teksti =Kirja Googlen teoshaussa | Viitattu =16.01.2010 | Kieli ={{en}}}}</ref> |
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:Na<sub>2</sub>O + 2 HBF<sub>4</sub> → 2 NaBF<sub>4</sub> + H<sub>2</sub>O |
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:NaOH + HBF<sub>4</sub> → NaBF<sub>4</sub> + H<sub>2</sub>O |
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:Na<sub>2</sub>CO<sub>3</sub> + 2 HBF<sub>4</sub> → 2 NaBF<sub>4</sub> + H<sub>2</sub>O + CO<sub>2</sub> |
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==Reactions and uses== |
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Sodium tetrafluoroborate can be used to prepare ], an ], by reacting with ].<ref>http://books.google.fi/books?id=J55D3HcgPuoC&pg=PA76&dq=%22Sodium+tetrafluoroborate%22&hl=fi&ei=TNCoTZbDIov3sgbc5aWXCA&sa=X&oi=book_result&ct=result&resnum=5&ved=0CEcQ6AEwBA</ref> |
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On heating to its melting point, sodium tetrafluoroborate decomposes to ] and ]:<ref>{{cite book | url = https://books.google.com/books?id=LkIWiNg4FGEC&q=%22Sodium+tetrafluoroborate%22&pg=PA1271 | title = Hazardous Chemicals Desk Reference | isbn = 9780470334454 | last1 = Richard J. Lewis | first1 = Sr | date = 2008-07-14| publisher = Wiley }}</ref> |
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:NaBF<sub>4</sub> → NaF + BF<sub>3</sub> |
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On heating, sodium tetrafluoroborate decomposes to ] and ].<ref>http://books.google.fi/books?id=LkIWiNg4FGEC&pg=PA1271&dq=%22Sodium+tetrafluoroborate%22&hl=fi&ei=TNCoTZbDIov3sgbc5aWXCA&sa=X&oi=book_result&ct=result&resnum=6&ved=0CEwQ6AEwBQ</ref> |
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It is a source of ] anion, which is used in ] for the preparation of salts. Sodium tetrafluoroborate can be used for synthesis of ]s, where tetrafluoroborate is the anion. |
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Sodium tetrafluoroborate can be used for synthesis of ]s, where the tetrafluoroborate often plays the role of the product's anion. |
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==References== |
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==References== |
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{{sodium compounds}} |
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{{Tetrafluoroborates}} |
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