White lead

White lead
Names
Other names
Basic lead carbonate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.901 Edit this at Wikidata
EC Number
  • 215-290-6
UNII
  • InChI=1S/2CH2O3.2H2O.3Pb/c2*2-1(3)4;;;;;/h2*(H2,2,3,4);2*1H2;;;/q;;;;3*+2/p-6
    Key: RYZCLUQMCYZBJQ-UHFFFAOYSA-H
  • C(=O)([O-])[O-].C(=O)([O-])[O-].[OH-].[OH-].[Pb+2].[Pb+2].[Pb+2]
Properties
2PbCO3·Pb(OH)2
Molar mass 775.633 g/mol
Appearance White powder
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Lead poisoning
GHS labelling:
GHS07: Exclamation markGHS08: Health hazardGHS09: Environmental hazard
H302, H332, H360, H373, H410
P201, P202, P260, P261, P264, P270, P271, P273, P281, P301+P312, P304+P312, P304+P340, P308+P313, P312, P314, P330, P391, P405, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Color pigments used on the warship Vasa, with white lead second from left, bottom shelf

White lead is the basic lead carbonate 2PbCO3·Pb(OH)2.[1] It is a complex salt, containing both carbonate and hydroxide ions. White lead occurs naturally as a mineral, in which context it is known as hydrocerussite,[1] a hydrate of cerussite.[2] It was formerly used as an ingredient for lead paint and a cosmetic called Venetian ceruse, because of its opacity and the satiny smooth mixture it made with dryable oils. However, it tended to cause lead poisoning, and its use has been banned in most countries.[3]

Basic lead carbonate is produced by treating lead acetate with carbon dioxide and air.[4] In the laboratory procedure treats lead acetate with urea.[5] It occurs naturally as the mineral cerussite.[6] The compound has been characterized by X-ray crystallography, which confirms the formula. The structure is complicated, features two kinds of Pb(II) sites, those bonded to hydroxide and those bonded to carbonate and hydroxide.[7]

  1. ^ a b Wiberg, Egon; Holleman, Arnold Frederick (2001). Inorganic Chemistry. Elsevier. ISBN 0-12-352651-5.
  2. ^ see mineral hydration
  3. ^ Hernberg, Sven (September 2000). "Lead Poisoning in a Historical Perspective" (PDF). American Journal of Industrial Medicine. 38 (3): 244–254. CiteSeerX 10.1.1.477.2081. doi:10.1002/1097-0274(200009)38:3<244::AID-AJIM3>3.0.CO;2-F. PMID 10940962. Archived from the original (PDF) on 2013-04-13. Retrieved 2015-04-12.
  4. ^ Carr, Dodd S. (2005). "Lead Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_249. ISBN 978-3527306732.
  5. ^ M. Baudler (1963). "Neutral and Basic Lead Carbonate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=766. NY,NY: Academic Press.
  6. ^ Inorganic Chemistry, Egon Wiberg, Arnold Frederick Holleman Elsevier 2001 ISBN 0-12-352651-5
  7. ^ Cite error: The named reference XRD was invoked but never defined (see the help page).