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Lead(II) perchlorate

Trihydrate
Names
Other names Plumbous perchlorate
Identifiers
CAS Number	13637-76-8
3D model (JSmol)	Interactive image
ChemSpider	55560
ECHA InfoCard	100.033.736
EC Number	237-125-7
PubChem CID	61655
UN number	1470
CompTox Dashboard (EPA)	DTXSID10890712
InChI InChI=1S/2ClHO4.Pb/c2*2-1(3,4)5;/h2*(H,2,3,4,5);/q;;+2/p-2
SMILES Cl(=O)(=O)=O.Cl(=O)(=O)=O.
Properties
Chemical formula	Pb(ClO4)2
Molar mass	406.10 g/mol
Appearance	White solid
Density	2.6 g/cm
Boiling point	250 °C (482 °F; 523 K) (decomposes)
Solubility in water	256.2 g/100 ml (25 °C)
Vapor pressure	0.36 Torr (trihydrate)
Hazards
GHS labelling:
Pictograms
Hazard statements	H272, H302, H332, H360Df, H373, H410
Precautionary statements	P210, P260, P273, P301+P312, P304+P340, P308+P313
Related compounds
Other cations	Mercury(II) perchlorate; Tin(II) perchlorate; Cadmium perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Infobox references

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.

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. The monohydrate is produced by only partially dehydrating the trihydrate, and this salt undergoes hydrolysis at 103 °C.

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

1. ^ H. H. Willard; J. L. Kassner (1930). "PREPARATION AND PROPERTIES OF LEAD PERCHLORATE". Journal of the American Chemical Society. 52 (6). ACS Publications: 2391–2396. doi:10.1021/ja01369a027.
2. Zinov'ev, A. A.; and Kritsov, N. V. (1960). Zhur. Neorg. Khim. issue 5: p. 1418, as cited in Giridharan, A. S.; Udupa, M. R.; Aravamudan, G. (February 1975). "Thermal behaviour of thallous perchlorate". Journal of Thermal Analysis. 7 (1): 65–71. doi:10.1007/BF01911626. ISSN 0022-5215.
3. A. V. Dudin (1993). "Water-vapor pressure and thermodynamics of the dehydration of manganese, nickel, cadmium, and lead perchlorate hydrates". Russian Chemical Bulletin. 42: 417–421. doi:10.1007/BF00698419.
4. Boyd, R. N.; Rauscher, T.; Reitzner, S. D.; Vogel, P. (2003-10-31). "Observing nucleon decay in lead perchlorate". Physical Review D. 68 (7). arXiv:hep-ph/0307280. doi:10.1103/PhysRevD.68.074014. ISSN 0556-2821.

• Lead(II) compounds
• Perchlorates