Lead(II) oxalate

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Lead(II) oxalate.svg
Identifiers
  • 814-93-7 checkY
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.011.284 Edit this at Wikidata
EC Number
  • 212-413-5
UNII
UN number 2291
  • InChI=1S/C2H2O4.Pb/c3-1(4)2(5)6;/h(H,3,4)(H,5,6);/q;+2/p-2
  • C(=O)(C(=O)[O-])[O-].[Pb+2]
Properties
PbC2O4
Molar mass 295.219
Appearance White Powder
Density 5.28 g/cm3
Melting point 327.4 °C (621.3 °F; 600.5 K)
Boiling point 1,740 °C (3,160 °F; 2,010 K)
Thermochemistry
146.0216 J [1]
Std enthalpy of
formation (ΔfH⦵298)
 -851.444 kJ/mol
Hazards
Main hazards Nephrotoxin, Reproductive Toxin, Neurotoxin, IARC Carcinogen, Birth Defects, Highly Toxic
GHS labelling:
GHS07: Exclamation markGHS08: Health hazardGHS09: Environmental hazard
Signal word
 Danger
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
NIOSH (US health exposure limits):
PEL (Permissible)
 0.05 mg/m3, as Pb
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Lead(II) oxalate is an organic compound with the formula PbC2O4. It is naturally found as a heavy white solid.[2]

Preparation[]

This compound is commercially available. It may be prepared by the metathesis reaction between lead(II) nitrate and sodium oxalate:[3]

Pb2+(aq) + C2O42− → PbC2O4 (s)

Solubility[]

Lead(II) oxalate is sparingly soluble in water. Its solubility is increased in presence of excess oxalate anions, due to the formation of the Pb(C2O4)22− complex ion.[4]

References[]

  1. ^ "Lead(II) Oxalate". Chemistry Reference. http://www.chemistry-reference.com/q_compounds.asp?CAS=814-93-7.
  2. ^ "Lead Oxalate". American Elements: The World's Manufacturer of Engineered & Advanced Materials. http://www.americanelements.com/pboxl.html.
  3. ^ Grases, F.; Ruiz, J.; Costa-Bauzá, A. (1993). "Studies on Lead Oxalate Crystalline Growth". Journal of Colloid and Interface Science. 155 (2): 265–270. doi:10.1006/jcis.1993.1035.
  4. ^ Kolthoff, I.M.; Perlich, R. W.; Weiblen, D. (1942). "The Solubility of lead Sulfate and of Lead Oxalate in Various Media". Journal of Physical Chemistry. 46 (5): 561. doi:10.1021/j150419a004.
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