Lead(II) sulfate

Structure

Anglesite (lead(II) sulfate, ) adopts the same orthorhombic crystal structure as celestite (strontium sulfate, ) and barite (barium sulfate, ). All three minerals' structures are in the space group Pbnm (number 62). Each lead(II) ion is surrounded by 12 oxygen atoms from 7 sulfate ions, forming a PbO12 polyhedron. The lead–oxygen distances range from 2.612 Å to 3.267 Å and the average distance is 2.865 Å.

Manufacturing

Lead(II) sulfate is prepared by treating lead oxide, hydroxide or carbonate with warm sulfuric acid or by treating a soluble lead salt with sulfuric acid.

Alternatively, it can be made by the interaction of solutions of lead nitrate and sodium sulfate.

Toxicology

Lead sulfate is toxic by inhalation, ingestion and skin contact. It is a cumulative poison, and repeated exposure may lead to anemia, kidney damage, eyesight damage or damage to the central nervous system (especially in children). It is also corrosive - contact with the eyes can lead to severe irritation or burns. Typical threshold limit value is 0.15 mg/m3.

Mineral

The naturally occurring mineral anglesite, PbSO4, occurs as an oxidation product of primary lead sulfide ore,

Basic and hydrogen lead sulfates

A number of lead basic sulfates are known: PbSO4·PbO; PbSO4·2PbO; PbSO4·3PbO; PbSO4·4PbO. They are used in manufacturing of active paste for lead–acid batteries. A related mineral is leadhillite, 2PbCO3·PbSO4·Pb(OH)2.

At high concentration of sulfuric acid (80%), lead hydrogensulfate, Pb(HSO4)2, forms.

Chemical properties

Lead(II) sulfate can be dissolved in concentrated HNO3, HCl, H2SO4 producing acidic salts or complex compounds, and in concentrated alkali giving soluble tetrahydroxidoplumbate(II) [Pb(OH)4]2− complexes.

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Lead(II) sulfate decomposes when heated above 1000 °C:

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Applications

• Lead-acid storage batteries
• Paint pigments
• Laboratory reagent

References

References

1. "Molar Mass of Lead Sulphate".
2. "NIST data review 1980". National Institute of Standards and Technology (NIST).
3. (2002). "CRC Handbook of Chemistry and Physics". Taylor & Francis.
4. (December 1934). "The Solubility of Lead Sulfate in Water and Aqueous Solutions of Sulfuric Acid 1". Journal of the American Chemical Society.
5. (2007). "Chemical Principles". Cengage Learning.
6. (2012). "Structural trends for celestite (SrSO₄), anglesite (PbSO₄), and barite (BaSO₄): Confirmation of expected variations within the SO₄ groups". [[American Mineralogist.
7. (1984). "Structural Inorganic Chemistry". Oxford University Press.
8. (2007). "Министерство образования и науки РФ, Реферат "Свинец и его свойства"". Ministry of Education and Science of the Russian Federation.
9. (September 2007). "Hazardous Substance Fact Sheet".