| Revision as of 16:37, 10 January 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 467429472 of page Zinc_nitrate for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 13:43, 19 June 2024 edit Marbletan (talk | contribs)Extended confirmed users5,340 edits No longer a stub |
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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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| verifiedrevid = 454732144 |
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| verifiedrevid = 470636543 |
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| Name = Zinc nitrate |
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| Name = Zinc nitrate |
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| ImageFile = zinc nitrate.png |
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| ImageFile = zinc nitrate.png |
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| ImageSize = 200px |
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| ImageSize = |
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| ImageName = Zinc nitrate |
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| ImageName = Zinc nitrate |
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| ImageFile1 = Dusičnan zinečnatý.JPG |
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| ImageFile1 = Dusičnan zinečnatý.JPG |
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| IUPACName = Zinc nitrate |
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| IUPACName = Zinc nitrate |
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| OtherNames = |
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| OtherNames = Zinc dinitrate |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 22926 |
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| ChemSpiderID = 22926 |
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| ChEBI = 231504 |
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| PubChem = 24518 |
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| PubChem = 24518 |
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| InChI = 1/2NO3.Zn/c2*2-1(3)4;/q2*-1;+2 |
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| InChI = 1/2NO3.Zn/c2*2-1(3)4;/q2*-1;+2 |
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| StdInChIKey = ONDPHDOFVYQSGI-UHFFFAOYSA-N |
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| StdInChIKey = ONDPHDOFVYQSGI-UHFFFAOYSA-N |
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| CASNo = 7779-88-6 |
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| CASNo = 7779-88-6 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo2_Ref = {{cascite|changed|??}} |
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| CASOther = <br> 19154-63-3 (tetrahydrate) <br> 10196-18-6 (hexahydrate) |
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| EINECS = 231-943-8 |
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| CASNo2 = 19154-63-3 |
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| CASNo2_Comment = (tetrahydrate) |
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| UNNumber = 1514 |
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| CASNo3_Ref = {{cascite|changed|??}} |
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| RTECS = ZH4772000 |
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| CASNo3 = 10196-18-6 |
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| CASNo3_Comment = (hexahydrate) |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = EDO66F5U49 |
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| EINECS = 231-943-8 |
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| UNNumber = 1514 |
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| RTECS = ZH4772000 |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = Zn(NO<sub>3</sub>)<sub>2</sub> |
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| Formula = {{chem2|Zn(NO3)2}} |
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| MolarMass = 189.36 g/mol (anhydrous) <br> 297.49 g/mol (hexahydrate) |
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| MolarMass = 189.36 g/mol (anhydrous)<br>297.49 g/mol (hexahydrate) |
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| Appearance = colorless, ] crystals |
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| Appearance = colorless, ] crystals |
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| Density = 2.065 g/cm<sup>3</sup> (hexahydrate) |
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| Density = 2.065 g/cm<sup>3</sup> (hexahydrate) |
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| Solubility = 327 g/100 mL, 40 °C (trihydrate) <br> 184.3 g/100 ml, 20 °C (hexahydrate) |
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| Solubility = 327 g/(100 mL), 40 °C (trihydrate)<br>184.3 g/(100 mL), 20 °C (hexahydrate) |
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| SolubleOther = very soluble in ] |
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| SolubleOther = very soluble in ] |
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| MeltingPtC = 110 |
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| MeltingPt = 110 °C (anhydrous) <br> 45.5 °C (trihydrate) <br> 36.4 °C (hexahydrate) |
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| BoilingPt = ~125 °C, decomp (hexahydrate) |
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| MeltingPt_notes = (anhydrous)<br>45.5 °C (trihydrate)<br>36.4 °C (hexahydrate) |
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| BoilingPt= ~ |
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| BoilingPtC = 125 |
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| BoilingPt_notes = decomposes (hexahydrate) |
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| MagSus = −63.0·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Section7 = {{Chembox Hazards |
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|Section7={{Chembox Hazards |
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| ExternalMSDS = |
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| ExternalSDS = |
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| GHSPictograms = {{GHS03}}{{GHS07}} |
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| EUIndex = Not listed |
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| MainHazards = Oxidant, may explode on heating |
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| MainHazards = Oxidant, may explode on heating |
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| FlashPt = Non-flammable |
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| FlashPt = Non-flammable |
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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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| OtherCpds = ] |
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| OtherCompounds = ] |
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'''Zinc nitrate''' is an inorganic chemical compound with the ] {{chem2|Zn(NO3)2}}. This colorless, crystalline salt is highly ]. It is typically encountered as a ] {{chem2|Zn(NO3)2*6H2O}}. It is soluble in both water and alcohol. |
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==Synthesis== |
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Zinc nitrate is usually prepared by dissolving zinc metal, ], or related materials in ]: |
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:{{chem2|Zn + 2 HNO3 → Zn(NO3)2 + H2}} |
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:{{chem2|ZnO + 2 HNO3 → Zn(NO3)2 + H2O}} |
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These reactions are accompanied by the hydration of the zinc nitrate. |
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The anhydrous salt arises by the reaction of anhydrous ] with ]:<ref name=G&E>{{Greenwood&Earnshaw2nd|page=455}}</ref> |
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:{{chem2|ZnCl2 + 4 NO2 → Zn(NO3)2 + 2 NOCl}} |
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==Reactions== |
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Treatment of zinc nitrate with ] gives zinc acetate.<ref>{{cite book|author1=O. F. Wagenknecht|author2=R. Juza|chapter=Zinc Acetate|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY, NY|volume=2|page=1087}}</ref> |
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On heating, zinc nitrate undergoes ] to form ], ] and ]: |
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:{{chem2|2 Zn(NO3)2 → 2 ZnO + 4 NO2 + 1 O2}} |
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Aqueous zinc nitrate contains ]es {{chem2|(2+) and (2+)}}.<ref>Sze, Yu-Keung, and Donald E. Irish. "Vibrational spectral studies of ion-ion and ion-solvent interactions. I. Zinc nitrate in water." Journal of Solution Chemistry 7.6 (1978): 395-415.</ref> and, thus, this reaction may be better written as the reaction of the aquated ion with hydroxide through donation of a proton, as follows. |
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==Applications== |
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Zinc nitrate has no large scale application but is used on a laboratory scale for the synthesis of ]s.<ref>{{cite journal|last1=Barnett|first1=Sarah A|last2=Champness|first2=Neil R|title=Structural diversity of building-blocks in coordination framework synthesis—combining M(NO3)2 junctions and bipyridyl ligands|journal=Coordination Chemistry Reviews|date=November 2003|volume=246|issue=1–2|pages=145–168|doi=10.1016/S0010-8545(03)00121-8}}</ref> Its controlled decomposition to ] has also been used for the generation of various ZnO based structures, including nanowires.<ref>{{cite journal|last1=Greene|first1=Lori E.|last2=Yuhas|first2=Benjamin D.|last3=Law|first3=Matt|last4=Zitoun|first4=David|last5=Yang|first5=Peidong|title=Solution-Grown Zinc Oxide Nanowires|journal=Inorganic Chemistry|date=September 2006|volume=45|issue=19|pages=7535–7543|doi=10.1021/ic0601900|pmid=16961338 }}</ref> |
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It can be used as a ] in ]. An example reaction gives a precipitate of ]: |
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:{{chem2|Zn(NO3)2 + ] → ZnCO3 + 2 ]}} |
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==References== |
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{{Reflist}} |
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{{Zinc compounds}} |
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{{nitrates}} |
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] |
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] |