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InChI=1S/H2O4S.Pb.4H/c1-5(2,3)4;;;;;/h(H2,1,2,3,4);;;;;/q;+2;;;;/p-2
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Key: PIJPYDMVFNTHIP-UHFFFAOYSA-L
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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

SMILES

[O-]S(=O)(=O)[O-].[Pb+2]

Properties Chemical formula Pb S O₄ 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 Solubility in water 0.0032 g/100 mL (15 °C)
0.00425 g/100 mL (25 °C)^[4] Solubility product

(

K_sp

)

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

Magnetic susceptibility

(χ)

−69.7·10⁻⁶ cm³/mol Refractive index

(

n_D

)

1.877 Structure Crystal structure orthorhombic, barite Thermochemistry Heat capacity (C) 103 J/degree mol Std molar
entropy (S^⦵₂₉₈) 149 J·mol⁻¹·K⁻¹^[5] Std enthalpy of
formation (Δ_fH^⦵₂₉₈) −920 kJ·mol⁻¹^[5] Hazards GHS labelling: Pictograms Signal word Danger Hazard statements H302, H332, H360Df, H410 Precautionary statements 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 Threshold limit value

(TLV)

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).

N verify

(

what is ^YN

Infobox references

Chemical compound

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.

Anglesite (lead(II) sulfate, PbSO₄) adopts the same orthorhombic crystal structure as celestite (strontium sulfate, SrSO₄) and barite (barium sulfate, BaSO₄). All three minerals' structures are in the space group Pbnm (number 62).^[6] Each lead(II) ion is surrounded by 12 oxygen atoms from 7 sulfate ions, forming a PbO₁₂ polyhedron.^[7] The lead–oxygen distances range from 2.612 Å to 3.267 Å and the average distance is 2.865 Å.^[6]

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.

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.^[8]

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) + 4 NaOH(aq) → Na₂[Pb(OH)₄](aq) + Na₂SO₄(aq)

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

PbSO₄(s) → PbO(s) + SO₃(g)

Lead paint

^ "Molar Mass of Lead Sulphate". webbook.nist.gov. Archived from the original on 13 December 2020. Retrieved 4 March 2022.
^ "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.
^ Lide, David R. (2002). CRC Handbook of Chemistry and Physics (83rd ed.). Taylor & Francis. ISBN 978-0-8493-0483-5.^{[page needed]}
^ Crockford, H. D.; Brawley, D. J. (December 1934). "The Solubility of Lead Sulfate in Water and Aqueous Solutions of Sulfuric Acid 1". Journal of the American Chemical Society. 56 (12): 2600–2601. Bibcode:1934JAChS..56.2600C. doi:10.1021/ja01327a019.
^ ^a ^b Zumdahl, Steven (2007). Chemical Principles. Cengage Learning. p. A22. ISBN 978-0-618-94690-7.
^ ^a ^b ^c Antao, Sytle M. (2012). "Structural trends for celestite (SrSO₄), anglesite (PbSO₄), and barite (BaSO₄): Confirmation of expected variations within the SO₄ groups". Am. Mineral. 97 (4): 661–665. Bibcode:2012AmMin..97..661A. doi:10.2138/am.2012.3905.
^ Wells, A. F. (1984). Structural Inorganic Chemistry (5th ed.). Oxford University Press. p. 1187. ISBN 978-0-19-965763-6.
^ "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.
^ ^a ^b ^c Hazardous Substance Fact Sheet (PDF), September 2007

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