Lead(II) sulfate

Lead(II) sulfate
Names
	IUPAC name lead(II) sulfate
	Other names Anglesite, fast white, milk white, plumbous sulfate
Identifiers
CAS Number	7446-14-2 ;
3D model (JSmol)	Interactive image;
ChemSpider	19956579 ;
ECHA InfoCard	100.028.362
EC Number	231-198-9;
PubChem CID	24008;
UNII	C516H654O8 ;
UN number	1759 1794
CompTox Dashboard (EPA)	DTXSID50883502 ;
	InChI InChI=1S/H2O4S.Pb.4H/c1-5(2,3)4;;;;;/h(H2,1,2,3,4);;;;;/q;+2;;;;/p-2 Key: PIJPYDMVFNTHIP-UHFFFAOYSA-L ; 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-].[PbH4+2];
Properties
Chemical formula	PbSO4
Molar mass	303.26 g/mol
Appearance	white solid
Density	6.29 g/cm3
Melting point	1,087 °C (1,989 °F; 1,360 K) decomposes
Solubility in water	0.0032 g/100 mL (15 °C) ; 0.0404 g/100 mL (25 °C)
Solubility product (Ksp)	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 (nD)	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
Std enthalpy of; formation (ΔfH⦵298)	−920 kJ·mol−1
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). verify (what is ?) Infobox references

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.

Structure

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]

Coordination geometry in lead(II) sulfate^[6]
Lead coordination	Sulfate coordination

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.^[8]

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.

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)

Applications

References

^ "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. (14 September 2002). "CRC Handbook of Chemistry and Physics. 83rd Edition". Journal of the American Chemical Society. 124 (47). National Institute of Standards and Technology (NIST); CRC Press: Boca Raton: 14280. doi:10.1021/ja025295q. ISBN 9780849304835. ISSN 0002-7863. OCLC 956588069. Archived from the original on 4 March 2022. Retrieved 4 March 2022.
^ PubChem. "Lead sulfate". pubchem.ncbi.nlm.nih.gov. Archived from the original on 29 November 2021. Retrieved 2022-03-04.
^ ^a ^b Zumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7. OCLC 1029017812.
^ ^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. doi:10.2138/am.2012.3905. S2CID 55149411.
^ 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

External links

[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.

[CRC-3] Lide, David R. (14 September 2002). "CRC Handbook of Chemistry and Physics. 83rd Edition". Journal of the American Chemical Society. 124 (47). National Institute of Standards and Technology (NIST); CRC Press: Boca Raton: 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.

[zumdahl-5] Zumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7. OCLC 1029017812.

[Antao-6] 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. doi:10.2138/am.2012.3905. S2CID 55149411.

[Wells-7] Wells, A. F. (1984). Structural Inorganic Chemistry (5th ed.). Oxford University Press. p. 1187. ISBN 978-0-19-965763-6.

[8] "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.

[:0-9] Hazardous Substance Fact Sheet (PDF), September 2007

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