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
Names
Other names
  • Plumbous perchlorate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.736
EC Number
  • 237-125-7
UN number 1470
  • InChI=1S/2ClHO4.Pb/c2*2-1(3,4)5;/h2*(H,2,3,4,5);/q;;+2/p-2
  • [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Pb+2]
Properties
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)
256.2 g/100 ml (25 °C)
Vapor pressure 0.36 Torr (trihydrate)
Hazards
GHS labelling:
GHS03: OxidizingGHS07: Exclamation markGHS06: ToxicGHS09: Environmental hazard
H272, H302, H332, H360Df, H373, H410
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. The anhydrous salt decomposes into lead(II) chloride and lead(II) oxide at 250 °C. The monohydrate is produced by only partially dehydrating the trihydrate, and this salt undergoes hydrolysis at 103 °C.[2]

The solution of anhydrous lead(II) perchlorate in methanol is explosive.

References
  1. H. H. Willard; J. L. Kassner (1930). "PREPARATION AND PROPERTIES OF LEAD PERCHLORATE". Journal of the American Chemical Society. ACS Publications. 52 (6): 2391–2396. doi:10.1021/ja01369a027.
  2. 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.
Compounds containing perchlorate group
HClO4 He
LiClO4 Be(ClO4)2 B(ClO4)−4
B(ClO4)3		 ROClO3 N(ClO4)3
NH4ClO4
NOClO4		 H3OClO4 FClO4 Ne
NaClO4 Mg(ClO4)2 Al(ClO4)3
Al(ClO4)−4
Al(ClO4)2−5
Al(ClO4)3−6		 Si P S ClO−4
ClOClO3
Cl2O7		 Ar
KClO4 Ca(ClO4)2 Sc(ClO4)3 Ti(ClO4)4 VO(ClO4)3
VO2(ClO4)		 Cr(ClO4)3 Mn(ClO4)2 Fe(ClO4)2
Fe(ClO4)3		 Co(ClO4)2,
Co(ClO4)3		 Ni(ClO4)2 Cu(ClO4)2 Zn(ClO4)2 Ga(ClO4)3 Ge As Se Br Kr
RbClO4 Sr(ClO4)2 Y(ClO4)3 Zr(ClO4)4 Nb(ClO4)5 Mo Tc Ru Rh(ClO4)3 Pd(ClO4)2 AgClO4 Cd(ClO4)2 In(ClO4)3 Sn(ClO4)4 Sb TeO(ClO4)2 I Xe
CsClO4 Ba(ClO4)2   Lu(ClO4)3 Hf(ClO4)4 Ta(ClO4)5
TaO(ClO4)3
TaO2ClO4		 W Re Os Ir Pt Au Hg2(ClO4)2,
Hg(ClO4)2		 Tl(ClO4),
Tl(ClO4)3		 Pb(ClO4)2 Bi(ClO4)3 Po At Rn
FrClO4 Ra   Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La Ce(ClO4)x Pr(ClO4)3 Nd(ClO4)3 Pm Sm(ClO4)3 Eu(ClO4)3 Gd(ClO4)3 Tb(ClO4)3 Dy(ClO4)3 Ho(ClO4)3 Er(ClO4)3 Tm(ClO4)3 Yb(ClO4)3
Ac Th(ClO4)4 Pa UO2(ClO4)2 Np Pu Am Cm Bk Cf Es Fm Md No
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