Lead(II) perchlorate
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| Plumbous perchlorate
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| ImageFile = Lead(II) perchlorate.svg
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| ImageFile1 = Lead(II) perchlorate trihydrate.jpg
| ImageCaption1 = Trihydrate
| Section1 = {{Chembox Identifiers
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| CASNo = 13637-76-8
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| ChemSpiderID = 55560
| EC_number = 237-125-7
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| InChI = 1S/2ClHO4.Pb/c2*2-1(3,4)5;/h2*(H,2,3,4,5);/q;;+2/p-2
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| PubChem = 61655
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| SMILES = [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Pb+2]
| UNNumber = 1470
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| Section2 = {{Chembox Properties
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| Appearance = White solid
| BoilingPt =
| BoilingPtC = 250
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| BoilingPt_notes= (decomposes)
| Density = 2.6 g/cm3
| Formula = Pb(ClO4)2
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| MolarMass = 406.10 g/mol
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| Solubility = 256.2 g/100 ml (25 °C)
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| VaporPressure = 0.36 Torr (trihydrate)
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| GHSPictograms = {{GHS03}}{{GHS07}}{{GHS06}}{{GHS09}}
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| HPhrases = {{H-phrases|272|360Df|332|302|373|410}}
| PPhrases = {{P-phrases|308+313|210|301+312|304+340|260|273}}
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| Section9 = {{Chembox Related
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| OtherCations = Mercury(II) perchlorate; Tin(II) perchlorate; Cadmium perchlorate
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Lead(II) perchlorate is a chemical compound with the formula Pb(ClO4)2·xH2O, where is x is 0,1, or 3. It is an extremely hygroscopic white solid that is very soluble in water.{{cite journal |author1=H. H. Willard |author2=J. L. Kassner |title=PREPARATION AND PROPERTIES OF LEAD PERCHLORATE |journal=Journal of the American Chemical Society |date=1930 |volume=52 |issue=6 |pages=2391–2396 |doi=10.1021/ja01369a027 |publisher=ACS Publications |language=en}}
Preparation
Lead perchlorate trihydrate is produced by the reaction of lead(II) oxide, lead carbonate, or lead nitrate by perchloric acid:
:Pb(NO3)2 + HClO4 → Pb(ClO4)2 + HNO3
The excess perchloric acid was removed by first heating the solution to 125 °C, then heating it under moist air at 160 °C to remove the perchloric acid by converting the acid to the dihydrate. The anhydrous salt, Pb(ClO4)2, is produced by heating the trihydrate to 120 °C under water-free conditions over phosphorus pentoxide. The trihydrate melts at 83 °C. The anhydrous salt decomposes into lead(II) chloride and a mixture of lead oxides at 250 °C.Zinov'ev, A. A.; and Kritsov, N. V. (1960). Zhur. Neorg. Khim. issue 5: p. 1418, as cited in {{Cite journal |last=Giridharan |first=A. S. |last2=Udupa |first2=M. R. |last3=Aravamudan |first3=G. |date=February 1975 |title=Thermal behaviour of thallous perchlorate |url=http://link.springer.com/10.1007/BF01911626 |journal=Journal of Thermal Analysis |language=en |volume=7 |issue=1 |pages=65–71 |doi=10.1007/BF01911626 |issn=0022-5215|url-access=subscription }} The monohydrate is produced by only partially dehydrating the trihydrate, and this salt undergoes hydrolysis at 103 °C.{{cite journal |author1=A. V. Dudin |title=Water-vapor pressure and thermodynamics of the dehydration of manganese, nickel, cadmium, and lead perchlorate hydrates |journal=Russian Chemical Bulletin |date=1993 |volume=42 |pages=417–421 |doi=10.1007/BF00698419 |language=en}}
The solution of anhydrous lead(II) perchlorate in methanol is explosive.
Applications
Lead perchlorate has a high nucleon density, making it a viable detector for hypothetical proton decay.
References
{{Lead compounds}}
{{Perchlorates}}