Lead(II) carbonate is the chemical compound with the chemical formula PbCO3. It is a white solid with several practical uses, despite its toxicity.[2] It occurs naturally as the mineral cerussite.[3]
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IUPAC name
Lead(II) carbonate
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ChemSpider |
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ECHA InfoCard | 100.009.041 |
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UNII |
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CompTox Dashboard (EPA)
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Properties | |
PbCO3 | |
Molar mass | 267.21 g/mol |
Appearance | White powder |
Density | 6.582 g/cm3 |
Melting point | 315 °C (599 °F; 588 K) (decomposes) |
0.00011 g/(100 mL) (20 °C) | |
Solubility product (Ksp)
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1.46·10−13 |
Solubility | insoluble in alcohol, ammonia; soluble in acid, alkali |
−61.2·10−6 cm3/mol | |
Refractive index (nD)
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1.804[1] |
Hazards | |
GHS labelling: | |
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 | |
Flash point | Non-flammable |
Safety data sheet (SDS) | External MSDS |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references
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Like all metal carbonates, lead(II) carbonate adopts a dense, highly crosslinked structure consisting of intact CO2−3 and metal cation sites. As verified by X-ray crystallography, the Pb(II) centers are seven-coordinate, being surrounded by multiple carbonate ligands. The carbonate centers are bonded bidentate to a single Pb and bridge to five other Pb sites.[4]
Lead carbonate is manufactured by passing carbon dioxide into a cold dilute solution of lead(II) acetate, or by shaking a suspension of a lead salt more soluble than the carbonate with ammonium carbonate at a low temperature to avoid formation of basic lead carbonate.[2]
Lead carbonate is used as a catalyst to polymerize formaldehyde to poly(oxymethylene). It improves the bonding of chloroprene to wire.[2]
The supply and use of this compound is restricted in Europe.[5]
A number of lead carbonates are known:
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