Lead(II) sulfate
{{Chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 427862762
| ImageFile1 = Lead(II) sulfate.jpg
| ImageSize1 = 244
| ImageName1 = sample of lead(II) sulfate
| ImageFile2 = Lead(II)-sulfate-xtal-2x2x2-3D-bs-17.png
| ImageName2 = Crystal structure of lead(II) sulfate
| IUPACName = lead(II) sulfate
| SystematicName =
| OtherNames = Anglesite, fast white, milk white, plumbous sulfate
|Section1={{Chembox Identifiers
| CASNo = 7446-14-2
| CASNo_Ref = {{cascite|correct|CAS}}
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 19956579
| EC_number = 231-198-9
| PubChem = 24008
| RTECS =
| UNNumber = 1759 1794
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = C516H654O8
| InChI = 1S/H2O4S.Pb.4H/c1-5(2,3)4;;;;;/h(H2,1,2,3,4);;;;;/q;+2;;;;/p-2
| InChIKey = PIJPYDMVFNTHIP-QKXYEYSFAV
| SMILES = [O-]S(=O)(=O)[O-].[PbH4+2]
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/H2O4S.Pb.4H/c1-5(2,3)4;;;;;/h(H2,1,2,3,4);;;;;/q;+2;;;;/p-2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = PIJPYDMVFNTHIP-UHFFFAOYSA-L
| InChIKey1 = PIJPYDMVFNTHIP-UHFFFAOYSA-L
}}
|Section2={{Chembox Properties
| MolarMass = 303.26 g/mol{{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}}{{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}}
| Appearance = white solid
| Density = 6.29 g/cm3{{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}}
| MeltingPtC = 1087
| MeltingPt_notes = decomposes
| BoilingPt =
| Solubility = 0.0032 g/100 mL (15 °C)
0.00425 g/100 mL (25 °C){{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 }}
| SolubilityProduct = 2.13 x 10−8 (20 °C)
| SolubleOther = insoluble in alcohol
soluble in ammonium acetate (≥ 6 mol/L)
soluble in ammonium tartrate in presence of ammonium chloride and ammonia
| RefractIndex = 1.877
| MagSus = −69.7·10−6 cm3/mol
}}
|Section3={{Chembox Structure
| CrystalStruct = orthorhombic, barite
| Coordination =
}}
|Section4={{Chembox Thermochemistry
| DeltaHf = −920 kJ·mol−1{{cite book |last1=Zumdahl |first1=Steven |title=Chemical Principles |date=2007 |publisher=Cengage Learning |isbn=978-0-618-94690-7 |page=A22 }}
| HeatCapacity = 103 J/degree mol
}}
|Section7={{Chembox Hazards
| ExternalSDS =
| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}}
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|302|332|360Df|410}}
| PPhrases = {{P-phrases|201|202|260|261|264|270|271|273|281|301+312|304+312|304+340|308+313|312|314|330|391|405|501}}
| NFPA-H = 3
| NFPA-F = 0
| NFPA-R = 0
| NFPA-S =
| FlashPt = Non-flammable
| PEL =
| TLV = 0.15 mg/m3
}}
|Section8={{Chembox Related
| OtherAnions = Lead(II) chloride, Lead(II) bromide, Lead(II) iodide, Lead(II) fluoride
| OtherCations = Tin(II) sulfate, Sodium sulfate, Copper(II) sulfate
| OtherFunction =
| OtherFunction_label =
| OtherCompounds =
}}
}}
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, {{chem2|PbSO4}}) adopts the same orthorhombic crystal structure as celestite (strontium sulfate, {{chem2|SrSO4}}) and barite (barium sulfate, {{chem2|BaSO4}}). All three minerals' structures are in the space group Pbnm (number 62).{{ cite journal | title = Structural trends for celestite (SrSO4), anglesite (PbSO4), and barite (BaSO4): Confirmation of expected variations within the SO4 groups | first1 = Sytle M. | last1 = Antao | journal = Am. Mineral. | year = 2012 | volume = 97 | issue = 4 | pages = 661–665 | doi = 10.2138/am.2012.3905 | bibcode = 2012AmMin..97..661A }} Each lead(II) ion is surrounded by 12 oxygen atoms from 7 sulfate ions, forming a PbO12 polyhedron.{{ 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 }} The lead–oxygen distances range from 2.612 Å to 3.267 Å and the average distance is 2.865 Å.
| class="wikitable" style="margin:1em auto; text-align:center;"
|+Coordination geometry in lead(II) sulfate |
| Lead coordination
! Sulfate coordination |
|---|
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| 150px |
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.{{cite web|title=Министерство образования и науки РФ, Реферат "Свинец и его свойства"|trans-title=Abstract: Lead and its properties|year=2007|publisher=Ministry of Education and Science of the Russian Federation|url=https://revolution.allbest.ru/chemistry/00011389_0.html|url-status=live|archive-url=https://web.archive.org/web/20071221072547/https://revolution.allbest.ru/chemistry/00011389_0.html|archive-date=21 December 2007}}
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.
:{{chem2 | PbSO4(s) + H2SO4(l) <-> Pb(HSO4)2(aq) }}
:{{chem2 | PbSO4(s) + 4 NaOH(aq) -> Na2[Pb(OH)4](aq) + Na2SO4(aq) }}
Lead(II) sulfate decomposes when heated above 1000 °C:
:{{chem2 | PbSO4(s) -> PbO(s) + SO3(g) }}
Applications
See also
References
{{reflist}}
External links
{{Commons cat|Lead(II) sulfate}}
- [https://www.atsdr.cdc.gov/HEC/CSEM/lead/ Case Studies in Environmental Medicine (CSEM): Lead Toxicity]
- [https://www.atsdr.cdc.gov/toxfaqs/tfacts13.pdf ToxFAQs: Lead]
- [https://web.archive.org/web/20080111154608/https://www.npi.gov.au/database/substance-info/profiles/50.html National Pollutant Inventory - Lead and Lead Compounds Fact Sheet]
{{Lead compounds}}
{{Sulfates}}
{{DEFAULTSORT:Lead(Ii) Sulfate}}