Lead(II) sulfate: Difference between revisions

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| MolarMass = 303.26 g/mol<ref>{{Cite web|title=Molar Mass of Lead Sulphate|url=https://webbook.nist.gov/cgi/cbook.cgi?ID=C7446142&Mask=4&Units=SI|access-date=4 March 2022|website=webbook.nist.gov|language=en|archive-date=13 December 2020|archive-url=https://web.archive.org/web/20201213095047/https://webbook.nist.gov/cgi/cbook.cgi?ID=C7446142&Units=SI&Mask=4|url-status=live}}</ref><ref>{{cite web|title=NIST data review 1980|publisher=National Institute of Standards and Technology (NIST)|url=https://nist.gov/data/PDFfiles/jpcrd166.pdf|url-status=dead|archive-url=https://web.archive.org/web/20161221073943/http://nist.gov/data/PDFfiles/jpcrd166.pdf|archive-date=21 December 2016|access-date=4 March 2022}}</ref>
| MolarMass = 303.26 g/mol<ref>{{Cite web|title=Molar Mass of Lead Sulphate|url=https://webbook.nist.gov/cgi/cbook.cgi?ID=C7446142&Mask=4&Units=SI|access-date=4 March 2022|website=webbook.nist.gov|language=en|archive-date=13 December 2020|archive-url=https://web.archive.org/web/20201213095047/https://webbook.nist.gov/cgi/cbook.cgi?ID=C7446142&Units=SI&Mask=4|url-status=live}}</ref><ref>{{cite web|title=NIST data review 1980|publisher=National Institute of Standards and Technology (NIST)|url=https://nist.gov/data/PDFfiles/jpcrd166.pdf|url-status=dead|archive-url=https://web.archive.org/web/20161221073943/http://nist.gov/data/PDFfiles/jpcrd166.pdf|archive-date=21 December 2016|access-date=4 March 2022}}</ref>
| Appearance = white solid
| Appearance = white solid
| Density = 6.29 g/cm<sup>3</sup><ref name="CRC">{{Cite journal |date=14 September 2002 |title=CRC Handbook of Chemistry and Physics. 83rd Edition |last=Lide |first=David R. |publisher=National Institute of Standards and Technology (NIST); CRC Press: Boca Raton |isbn=9780849304835 |oclc=956588069 |url=https://doi.org/10.1021/ja025295q |url-status=live |archive-url=https://archive.today/20220304180707/https://pubs.acs.org/doi/10.1021/ja025295q |archive-date=4 March 2022 |journal=[[Journal of the American Chemical Society]] |volume=124 |issue=47 |page=14280 |doi=10.1021/ja025295q |issn=0002-7863 |access-date=4 March 2022 |url-access=subscription }}</ref>
| Density = 6.29 g/cm<sup>3</sup><ref name="CRC">{{cite book |last1=Lide |first1=David R. |title=CRC Handbook of Chemistry and Physics |edition=83rd |date=2002 |publisher=Taylor & Francis |isbn=978-0-8493-0483-5 }}{{pn|date=June 2025}}</ref>
| MeltingPtC = 1087
| MeltingPtC = 1087
| MeltingPt_notes = decomposes
| MeltingPt_notes = decomposes
| BoilingPt =  
| BoilingPt =  
| Solubility = 0.0032 g/100 mL (15 °C) <br> 0.0404 g/100 mL (25 °C)<ref>{{Cite web |last=PubChem |title=Lead sulfate |url=https://pubchem.ncbi.nlm.nih.gov/compound/Lead-sulfate#section=Solubility |url-status=live |archive-url=https://web.archive.org/web/20211129111131/https://pubchem.ncbi.nlm.nih.gov/compound/Lead-sulfate |archive-date=29 November 2021 |access-date=2022-03-04 |website=pubchem.ncbi.nlm.nih.gov |language=en}}</ref>
| Solubility = 0.0032 g/100 mL (15 °C) <br> 0.00425 g/100 mL (25 °C)<ref>{{cite journal |last1=Crockford |first1=H. D. |last2=Brawley |first2=D. J. |title=The Solubility of Lead Sulfate in Water and Aqueous Solutions of Sulfuric Acid 1 |journal=Journal of the American Chemical Society |date=December 1934 |volume=56 |issue=12 |pages=2600–2601 |doi=10.1021/ja01327a019 |bibcode=1934JAChS..56.2600C }}</ref>
| SolubilityProduct = 2.13 x 10<sup>−8</sup> (20 °C)
| SolubilityProduct = 2.13 x 10<sup>−8</sup> (20 °C)
| SolubleOther = insoluble in alcohol  
| SolubleOther = insoluble in alcohol  
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  }}
  }}
|Section4={{Chembox Thermochemistry
|Section4={{Chembox Thermochemistry
| DeltaHf = −920&nbsp;kJ·mol<sup>−1</sup><ref name=zumdahl>{{cite book|last=Zumdahl|first=Steven S.|title=Chemical Principles|url=https://books.google.com/books?id=ZpIJzgEACAAJ|publisher=Houghton Mifflin Company|year = 2009|isbn=978-0-618-94690-7|oclc=1029017812|page=A22|edition=6th}}</ref>
| DeltaHf = −920&nbsp;kJ·mol<sup>−1</sup><ref name=zumdahl>{{cite book |last1=Zumdahl |first1=Steven |title=Chemical Principles |date=2007 |publisher=Cengage Learning |isbn=978-0-618-94690-7 |page=A22 }}</ref>
| Entropy = 149&nbsp;J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=zumdahl/>
| Entropy = 149&nbsp;J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=zumdahl/>
| HeatCapacity = 103 J/degree mol
| HeatCapacity = 103 J/degree mol
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==Structure==
==Structure==
Anglesite (lead(II) sulfate, {{chem2|PbSO4}}) adopts the same [[Orthorhombic crystal system|orthorhombic]] [[crystal structure]] as [[celestite]] ([[strontium sulfate]], {{chem2|SrSO4}}) and [[barite]] ([[barium sulfate]], {{chem2|BaSO4}}). All three minerals' structures are in the [[space group]] [[List of space groups#List_of_orthorhombic|''Pbnm'' (number 62)]].<ref name="Antao">{{ cite journal | title = Structural trends for celestite (SrSO<sub>4</sub>), anglesite (PbSO<sub>4</sub>), and barite (BaSO<sub>4</sub>): Confirmation of expected variations within the SO<sub>4</sub> groups | first1 = Sytle M. | last1 = Antao | journal = [[American Mineralogist|Am. Mineral.]] | year = 2012 | volume = 97 | issue = 4 | pages = 661–665 | doi = 10.2138/am.2012.3905 | s2cid = 55149411 }}</ref> Each lead(II) ion is surrounded by 12 oxygen atoms from 7 sulfate ions, forming a PbO<sub>12</sub> polyhedron.<ref name="Wells">{{ cite book | first1 = A. F. | last1 = Wells | title = Structural Inorganic Chemistry | edition = 5th | year = 1984 | publisher = Oxford University Press | isbn = 978-0-19-965763-6 | pages = 1187 }}</ref> The lead–oxygen distances range from 2.612 Å to 3.267 Å and the average distance is 2.865 Å.<ref name="Antao" />
Anglesite (lead(II) sulfate, {{chem2|PbSO4}}) adopts the same [[Orthorhombic crystal system|orthorhombic]] [[crystal structure]] as [[celestite]] ([[strontium sulfate]], {{chem2|SrSO4}}) and [[barite]] ([[barium sulfate]], {{chem2|BaSO4}}). All three minerals' structures are in the [[space group]] [[List of space groups#List_of_orthorhombic|''Pbnm'' (number 62)]].<ref name="Antao">{{ cite journal | title = Structural trends for celestite (SrSO<sub>4</sub>), anglesite (PbSO<sub>4</sub>), and barite (BaSO<sub>4</sub>): Confirmation of expected variations within the SO<sub>4</sub> groups | first1 = Sytle M. | last1 = Antao | journal = [[American Mineralogist|Am. Mineral.]] | year = 2012 | volume = 97 | issue = 4 | pages = 661–665 | doi = 10.2138/am.2012.3905 | bibcode = 2012AmMin..97..661A }}</ref> Each lead(II) ion is surrounded by 12 oxygen atoms from 7 sulfate ions, forming a PbO<sub>12</sub> polyhedron.<ref name="Wells">{{ cite book | first1 = A. F. | last1 = Wells | title = Structural Inorganic Chemistry | edition = 5th | year = 1984 | publisher = Oxford University Press | isbn = 978-0-19-965763-6 | page = 1187 }}</ref> The lead–oxygen distances range from 2.612 Å to 3.267 Å and the average distance is 2.865 Å.<ref name="Antao" />


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Revision as of 14:36, 4 June 2025

Template:Chembox

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, Template:Chem2) adopts the same orthorhombic crystal structure as celestite (strontium sulfate, Template:Chem2) and barite (barium sulfate, Template:Chem2). All three minerals' structures are in the space group Pbnm (number 62).[1] Each lead(II) ion is surrounded by 12 oxygen atoms from 7 sulfate ions, forming a PbO12 polyhedron.[2] The lead–oxygen distances range from 2.612 Å to 3.267 Å and the average distance is 2.865 Å.[1]

Coordination geometry in lead(II) sulfate[1]
Lead coordination Sulfate coordination
File:Lead(II)-sulfate-xtal-Pb-coordination-3D-bs-17.png File:Lead(II)-sulfate-xtal-SO4-coordination-3D-bs-17.png

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.[3]

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.

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Template:Chem2

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

Template:Chem2

Applications

See also

References

Template:Reflist

External links

Template:Commons cat

Template:Lead compounds Template:Sulfates

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