Lead(II) sulfate

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

• Lead-acid storage batteries • Paint pigments • Laboratory reagent == See also ==