Lead(II) perchlorate

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.^[1]

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 [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Pb+2]
Properties
Chemical formula	Pb(ClO4)2
Molar mass	406.10 g/mol
Appearance	White solid
Density	2.6 g/cm3
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 [77 °F], 100 kPa). Infobox references

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.^[1] The anhydrous salt decomposes into lead(II) chloride and a mixture of lead oxides at 250 °C.^[1][2] The monohydrate is produced by only partially dehydrating the trihydrate, and this salt undergoes hydrolysis at 103 °C.^[3]

The solution of anhydrous lead(II) perchlorate in methanol is explosive.^[1]

Applications

Lead perchlorate has a high nucleon density, making it a viable detector for hypothetical proton decay.^[4]