| Revision as of 16:37, 10 January 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,074 edits Saving copy of the {{chembox}} taken from revid 467502155 of page Zinc_hydroxide for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 18:56, 10 December 2024 edit Marbletan (talk | contribs)Extended confirmed users5,615 edits no longer a stub |
| Line 1: |
Line 1: |
|
{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
|
|
{{chembox |
|
{{chembox |
|
|
| Watchedfields = changed |
|
| verifiedrevid = 451313639 |
|
| verifiedrevid = 470636429 |
|
| Name = Zinc hydroxide |
|
| Name = Zinc hydroxide |
|
| ImageFile = Hydroxid zinečnatý.PNG |
|
| ImageFile = Hydroxid zinečnatý.PNG |
|
| ImageSize = |
|
| ImageSize = 250px |
|
| ImageName = Zinc hydroxide |
|
| ImageName = Zinc hydroxide |
|
| IUPACName =Zinc hydroxide |
|
| IUPACName = Zinc hydroxide |
|
| OtherNames = |
|
| OtherNames = |
|
|
| SystematicName = |
|
| Section1 = {{Chembox Identifiers |
|
| Section1 = {{Chembox Identifiers |
|
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
|
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
|
| ChemSpiderID = 7988510 |
|
| ChemSpiderID = 7988510 |
|
| InChI = 1/2H2O.Zn/h2*1H2;/q;;+2/p-2 |
|
| InChI = 1/2H2O.Zn/h2*1H2;/q;;+2/p-2 |
| Line 19: |
Line 20: |
|
| StdInChIKey = UGZADUVQMDAIAO-UHFFFAOYSA-L |
|
| StdInChIKey = UGZADUVQMDAIAO-UHFFFAOYSA-L |
|
| CASNo = 20427-58-1 |
|
| CASNo = 20427-58-1 |
|
| CASNo_Ref = {{cascite|correct|CAS}} |
|
| CASNo_Ref = {{cascite|correct|CAS}} |
|
|
| UNII_Ref = {{fdacite|correct|FDA}} |
| ⚫ |
| PubChem = 9812759 |
|
|
|
| UNII = OXK3V8KJ7L |
|
⚫ |
| PubChem = 9812759 |
|
}} |
|
}} |
|
| Section2 = {{Chembox Properties |
|
| Section2 = {{Chembox Properties |
|
| Formula = Zn(OH)<sub>2</sub> |
|
| Formula = Zn(OH)<sub>2</sub> |
|
| MolarMass = 99.424 g/mol |
|
| MolarMass = 99.424 g/mol |
|
| Appearance = white powder |
|
| Appearance = white powder |
|
| Density = 3.053 g/cm<sup>3</sup>, solid |
|
| Density = 3.053 g/cm<sup>3</sup>, solid |
|
| Solubility = slightly soluble |
|
| Solubility = slightly soluble |
|
| SolubilityProduct = 3.0{{e|−17}} |
|
| SolubilityProduct = 3.0{{e|−17}} |
|
| Solvent = ] |
|
| Solvent = ] |
|
| SolubleOther = insoluble |
|
| SolubleOther = insoluble |
|
| MeltingPt = 125 °C (decomposition) |
|
| MeltingPtC = 125 |
|
|
| MeltingPt_notes = (decomposition) |
|
| BoilingPt = |
|
|
|
| pKa = 3.12, 3.39<ref name=P82db>{{cite book|title=Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution|editor-first=D. D.|editor-last=Perrin|edition=2nd|series=] Chemical Data|issue=29|publisher=Pergamon|location=Oxford|year=1982|publication-date=1984|orig-date=1969|lccn=82-16524|isbn=0-08-029214-3|at=Entry 265}}</ref> |
|
|
| MagSus = −67.0·10<sup>−6</sup> cm<sup>3</sup>/mol |
|
}} |
|
}} |
|
|
| Section3 = |
|
|
| Section4 = {{Chembox Thermochemistry |
|
|
| DeltaHf = −642 kJ·mol<sup>−1</sup><ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7|page=A23}}</ref> |
|
|
| Entropy = |
|
|
}} |
|
|
| Section5 = |
|
|
| Section6 = |
|
| Section7 = {{Chembox Hazards |
|
| Section7 = {{Chembox Hazards |
|
| EUIndex = not listed |
|
| NFPA-H = |
|
| NFPA-H = |
|
| NFPA-R = |
|
| NFPA-R = |
|
| NFPA-F = |
|
⚫ |
| FlashPt = Non-flammable |
|
| NFPA-F = |
|
| ⚫ |
| FlashPt = Non-flammable |
|
|
}} |
|
}} |
|
| Section8 = {{Chembox Related |
|
| Section8 = {{Chembox Related |
|
| OtherAnions = ] |
|
| OtherAnions = ] |
|
| OtherCations = ] |
|
| OtherCations = ] |
|
}} |
|
}} |
|
}} |
|
}} |
|
|
|
|
|
'''Zinc hydroxide''' ](])<sub>2</sub> is an ] ]. It also occurs naturally as 3 rare minerals: ] (orthorhombic), ] and ] (both tetragonal). |
|
|
|
|
|
Like the hydroxides of other metals, such as ], ], ], ] and ], Zinc hydroxide (and ]), is ]. Thus it will dissolve readily in a dilute solution of a ], such as ], and also in a solution of an alkali such as ]. |
|
|
|
|
|
==Preparation== |
|
|
It can be prepared by first dissolving ] in concentrated aqueous solution of sodium hydroxide. The resulting solution is strongly diluted.<ref>{{cite book|author1=F. Wagenknecht|author2=R. Juza|chapter=Zinc Sulfide|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY,NY|volume=2pages=1074}}</ref> |
|
|
:Zn<sup>2+</sup> + 2 OH<sup>−</sup> → Zn(OH)<sub>2</sub>. |
|
|
|
|
|
The initial colorless solution contains the ]: |
|
|
:Zn(OH)<sub>2</sub> + 2 OH<sup>−</sup> → Zn(OH)<sub>4</sub><sup>2−</sup>. |
|
|
Zinc hydroxide will dissolve because the ion is normally surrounded by water ligands; when excess sodium hydroxide is added to the solution the hydroxide ions will reduce the complex to a −2 charge and make it soluble. When excess ammonia is added, it sets up an equilibrium which provides hydroxide ions; the formation of hydroxide ions causes a similar reaction as sodium hydroxide and creates a +2 charged complex with a co-ordination number of 4 with the ammonia ligands - this makes the complex soluble so that it dissolves. |
|
|
|
|
|
Unlike the hydroxides of aluminium and lead, zinc hydroxide also dissolves in excess aqueous ] to form a colorless, water-soluble ]. |
|
|
|
|
|
==Applications== |
|
|
One major use is as an absorbent in ]. |
|
|
It is also used to find zinc salts by mixing ] with the suspect ]. |
|
|
|
|
|
==References== |
|
|
{{reflist}} |
|
|
* Chemistry in Context - By Graham Hill, John Holman (pp. 283,284) |
|
|
|
|
|
{{Zinc compounds}} |
|
|
{{Hydroxides}} |
|
|
|
|
|
] |
|
|
] |