Lead(II) sulfate

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Lead(II) sulfate
sample of lead(II) sulfate
Names
IUPAC name
lead(II) sulfate
Other names
Anglesite, fast white, milk white, plumbous sulfate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.028.362 Edit this at Wikidata
EC Number
  • 231-198-9
UNII
UN number 1759 1794
  • InChI=1S/H2O4S.Pb.4H/c1-5(2,3)4;;;;;/h(H2,1,2,3,4);;;;;/q;+2;;;;/p-2 checkY
    Key: PIJPYDMVFNTHIP-UHFFFAOYSA-L checkY
  • InChI=1S/H2O4S.Pb.4H/c1-5(2,3)4;;;;;/h(H2,1,2,3,4);;;;;/q;+2;;;;/p-2
    Key: PIJPYDMVFNTHIP-QKXYEYSFAV
  • Key: PIJPYDMVFNTHIP-UHFFFAOYSA-L
  • [O-]S(=O)(=O)[O-].[PbH4+2]
Properties
PbSO4
Molar mass 303.26 g/mol[1][2]
Appearance white solid
Density 6.29 g/cm3[3]
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)[4]
2.13 x 10−8 (20 °C)
Solubility insoluble in alcohol

soluble in ammonium acetate (≥ 6 mol/L)

soluble in ammonium tartrate in presence of ammonium chloride and ammonia

−69.7·10−6 cm3/mol
1.877
Structure
orthorhombic, barite
Thermochemistry
103 J/degree mol
149 J·mol−1·K−1[5]
−920 kJ·mol−1[5]
Hazards
GHS labelling:
GHS07: Exclamation markGHS08: Health hazardGHS09: Environmental hazard
Danger
H302, H332, H360Df, H410
P201, P202, P260, P261, P264, P270, P271, P273, P281, P301+P312, P304+P312, P304+P340, P308+P313, P312, P314, P330, P391, P405, P501
NFPA 704 (fire diamond)
3
0
0
Flash point Non-flammable
0.15 mg/m3
Related compounds
Other anions
Lead(II) chloride, Lead(II) bromide, Lead(II) iodide, Lead(II) fluoride
Other cations
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).
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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.

Manufacturing[edit]

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[edit]

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[edit]

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

Basic and hydrogen lead sulfates[edit]

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.[6]

Chemical properties[edit]

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)

External links[edit]

References[edit]

  1. ^ "Molar Mass of Lead Sulphate". webbook.nist.gov. Archived from the original on 13 December 2020. Retrieved 4 March 2022.
  2. ^ "NIST data review 1980" (PDF). National Institute of Standards and Technology (NIST). Archived from the original (PDF) on 21 December 2016. Retrieved 4 March 2022.
  3. ^ Lide, David R. (14 September 2002). "CRC Handbook of Chemistry and Physics. 83rd Edition". Journal of the American Chemical Society. National Institute of Standards and Technology (NIST); CRC Press: Boca Raton. 124 (47): 14280. doi:10.1021/ja025295q. ISBN 9780849304835. ISSN 0002-7863. OCLC 956588069. Archived from the original on 4 March 2022. Retrieved 4 March 2022.
  4. ^ PubChem. "Lead sulfate". pubchem.ncbi.nlm.nih.gov. Archived from the original on 29 November 2021. Retrieved 2022-03-04.
  5. ^ a b Zumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7. OCLC 1029017812.
  6. ^ "Министерство образования и науки РФ, Реферат "Свинец и его свойства"" [Abstract: Lead and its properties]. Ministry of Education and Science of the Russian Federation. 2007. Archived from the original on 21 December 2007.