Anglesite, fast white, milk white, plumbous sulfate
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||303.26 g/mol|
|Melting point||1,087 °C (1,989 °F; 1,360 K) decomposes|
|0.0032 g/100 mL (15 °C) |
0.00443 g/100 mL (20 °C)
Solubility product (Ksp)
|2.13 x 10−8 (20 °C)|
|Solubility||insoluble in alcohol
soluble in ammonium acetate (>6M)
soluble in ammonium tartrate in presence of ammonium chloride and ammonia
Refractive index (nD)
Heat capacity (C)
|103 J/degree mol|
Std enthalpy of
|Repr. Cat. 1/3|
Dangerous for the environment (N)
|R-phrases (outdated)||R61, R20/22, R33, R62, R50/53|
|S-phrases (outdated)||S53, S45, S60, S61|
|NFPA 704 (fire diamond)|
Threshold limit value (TLV)
|Lead(II) chloride, Lead(II) bromide, Lead(II) iodide, Lead(II) fluoride|
|Tin(II) sulfate, Sodium sulfate, Copper(II) sulfate|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Lead(II) sulfate (PbSO4) is a white solid, which appears white in microcrystalline form. It is also known as fast white, milk white, sulfuric acid lead salt or anglesite.
It is often seen in the plates/electrodes of car batteries, as it is formed when the battery is discharged (when the battery is recharged, then the lead sulfate is transformed back to metallic lead and sulfuric acid on the negative terminal or lead dioxide and sulfuric acid on the positive terminal). Lead sulfate is poorly soluble in water.
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.
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.
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.
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.
- PbSO4(s) + H2SO4(l) ⇌ Pb(HSO4)2(aq)
- PbSO4(s) + 4NaOH(aq) → Na2[Pb(OH)4](aq) + Na2SO4(aq)
Lead(II) sulfate decomposes when heated above 1000 °C:
- PbSO4(s) → PbO(s) + SO3(g)
|Wikimedia Commons has media related to Lead(II) sulfate.|
- Case Studies in Environmental Medicine (CSEM): Lead Toxicity
- ToxFAQs: Lead
- National Pollutant Inventory - Lead and Lead Compounds Fact Sheet
- "CRC Handbook of Chemistry and Physics", 83rd Edition, CRC Press, 2002.
- NIST-data review 1980
- Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.
- Министерство образования и науки РФ, Реферат "Свинец и его свойства", 2007, http://revolution.allbest.ru/chemistry/00011389_0.html Archived 2007-12-21 at the Wayback Machine