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{{chembox |
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{{Chembox |
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| Watchedfields = changed |
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| verifiedrevid = 402197513 |
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| verifiedrevid = 427862762 |
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| ImageFile = Lead(II) sulfate.jpg |
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| ImageFile1 = Lead(II) sulfate.jpg |
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| ImageSize = 244 |
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| ImageSize1 = 244 |
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| ImageName = sample of lead(II) sulfate |
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| ImageName1 = sample of lead(II) sulfate |
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| ImageFile2 = Lead(II)-sulfate-xtal-2x2x2-3D-bs-17.png |
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| ImageName2 = Crystal structure of lead(II) sulfate |
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| IUPACName = lead(II) sulfate |
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| IUPACName = lead(II) sulfate |
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| SystematicName = |
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| SystematicName = |
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| OtherNames = ] |
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| OtherNames = ], fast white, milk white, plumbous sulfate |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| CASNo = 7446-14-2 |
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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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| CASNo_Ref = {{cascite|correct|CAS}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 19956579 |
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| EC_number = 231-198-9 |
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| PubChem = 24008 |
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| RTECS = |
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| UNNumber = 1759 1794 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = C516H654O8 |
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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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| InChIKey = PIJPYDMVFNTHIP-QKXYEYSFAV |
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| InChIKey = PIJPYDMVFNTHIP-QKXYEYSFAV |
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| SMILES = S(=O)(=O). |
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| SMILES = S(=O)(=O). |
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| StdInChIKey = PIJPYDMVFNTHIP-UHFFFAOYSA-L |
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| StdInChIKey = PIJPYDMVFNTHIP-UHFFFAOYSA-L |
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| InChIKey1 = PIJPYDMVFNTHIP-UHFFFAOYSA-L |
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| InChIKey1 = PIJPYDMVFNTHIP-UHFFFAOYSA-L |
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}} |
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| CASNo = 7446-14-2 |
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|Section2={{Chembox Properties |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| Formula = ]]]<sub>4</sub> |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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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> |
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| ChemSpiderID=19956579 |
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| Appearance = white solid |
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| EINECS = |
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| 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=] |volume=124 |issue=47 |page=14280 |doi=10.1021/ja025295q |issn=0002-7863 |access-date=4 March 2022 }}</ref> |
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| PubChem = |
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| InChI = |
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| MeltingPtC = 1087 |
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| MeltingPt_notes = decomposes |
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| BoilingPt = |
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}} |
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| 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> |
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| Section2 = {{Chembox Properties |
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| SolubilityProduct = 2.13 x 10<sup>−8</sup> (20 °C) |
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| Formula = ]]]<sub>4</sub> |
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| SolubleOther = insoluble in alcohol |
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| MolarMass = 303.26 g/] |
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| Appearance = white solid |
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soluble in ] (≥ 6 mol/L) |
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| Density = 6.29 g/cm<sup>3</sup><ref name="CRC">"CRC Handbook of Chemistry and Physics", 83rd Edition, CRC Press, 2002.</ref> |
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| MeltingPt = 1087 °C, 1360 K<ref name="CRC" /> |
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soluble in ] in presence of ] and ] |
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| BoilingPt = |
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| RefractIndex = 1.877 |
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| Solubility = 4.25 mg/100 mL (25 °C) |
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| MagSus = −69.7·10<sup>−6</sup> cm<sup>3</sup>/mol |
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}} |
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| Solvent = |
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|Section3={{Chembox Structure |
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| CrystalStruct = ], ] |
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| Section3 = {{Chembox Structure |
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| Coordination = |
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| CrystalStruct = ], ] |
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| Coordination = |
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|Section4={{Chembox Thermochemistry |
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}} |
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| DeltaHf = −920 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> |
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| Section4 = {{Chembox Thermochemistry |
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| Entropy = 149 J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=zumdahl/> |
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| DeltaHf = –920.1 kJ/mol |
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| Entropy = –813.4 kJ/mol |
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| HeatCapacity = 103 J/degree mol |
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| HeatCapacity = 103 J/degree mol |
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|Section7={{Chembox Hazards |
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| ExternalSDS = |
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| Section7 = {{Chembox Hazards |
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| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}} |
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| ExternalMSDS = |
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| GHSSignalWord = Danger |
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| EUIndex = 082-001-00-6 |
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| HPhrases = {{H-phrases|302|332|360Df|410}} |
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| EUClass = Repr. Cat. 1/3<br />Toxic ('''T''')<br />Harmful ('''Xn''')<br />Dangerous for the environment ('''N''') |
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| 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}} |
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| RPhrases = {{R61}}, {{R20/22}}, {{R33}}, {{R62}}, {{R50/53}} |
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| NFPA-H = 3 |
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| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}} |
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| NFPA-H = 3 |
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| NFPA-F = 0 |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| NFPA-R = 0 |
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| NFPA-S = |
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| FlashPt = Non-flammable |
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| NFPA-O = |
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| PEL = |
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| FlashPt = Non-flammable |
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| TLV = 0.15 mg/m<sup>3</sup> |
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| PEL = |
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| TLV = 0.15 mg/m<sup>3</sup> |
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| OtherAnions = ], ], ], ] |
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| Section8 = {{Chembox Related |
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| OtherAnions = ], ], ], ] |
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| OtherCations = ], ], ] |
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'''Lead(II) sulfate''' (British English '''sulphate''') (PbSO<sub>4</sub>) is a white crystal or powder. It is also known as ''fast white'', ''milk white'', ''sulfuric acid lead salt'' or ''anglesite''. |
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'''Lead(II) sulfate''' (PbSO<sub>4</sub>) 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''. |
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It is often seen in the plates/electrodes of ], 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 ] on the negative terminal or lead dioxide and sulfuric acid on the positive terminal). Lead sulfate is poorly ] in water. |
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It is often seen in the plates/electrodes of ], 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 ] on the negative terminal or ] and sulfuric acid on the positive terminal). Lead sulfate is poorly ] in water. |
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==Structure== |
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Anglesite (lead(II) sulfate, {{chem2|PbSO4}}) adopts the same ] ] as ] (], {{chem2|SrSO4}}) and ] (], {{chem2|BaSO4}}). All three minerals' structures are in the ] ].<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 = ] | 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" /> |
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{| class="wikitable" style="margin:1em auto; text-align:center;" |
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|+] in lead(II) sulfate<ref name="Antao" /> |
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! Lead coordination |
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! Sulfate coordination |
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==Manufacturing== |
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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. |
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Alternatively, it can be made by the interaction of solutions of lead nitrate and sodium sulfate. |
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==Toxicology== |
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==Toxicology== |
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Lead sulfate is toxic by inhalation, ingestion and skin contact. It is a ], and repeated exposure may lead to anemia, kidney damage, eyesight damage or damage to the central nervous system (especially in children). Some lead salts may cause reproductive defects and cardiovascular disturbances. It is also corrosive - contact with the eyes can lead to severe irritation or burns. Typical ] (above which the substance is harmful) is 0.15 mg/m³. |
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Lead sulfate is toxic by inhalation, ingestion and skin contact. It is a ], 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 ] is 0.15 mg/m<sup>3</sup>. |
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==Mineral== |
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==Mineral== |
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The naturally occurring mineral ], PbSO<sub>4</Sub>, occurs as an oxidation product of primary lead sulfide ore, |
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The naturally occurring mineral ], PbSO<sub>4</Sub>, occurs as an oxidation product of primary lead sulfide ore, ]. |
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==Basic and hydrogen lead sulfates== |
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==Basic and hydrogen lead sulfates== |
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A number of lead basic sulfates are known: PbSO<sub>4</Sub>·PbO; PbSO<sub>4</Sub>·2PbO; PbSO<sub>4</Sub>·3PbO; PbSO<sub>4</Sub>·4PbO. They are used in manufacturing of active paste for lead acid batteries. A related mineral is ], 2PbCO<sub>3</sub>·PbSO<sub>4</sub>·Pb(OH)<sub>2</sub>. |
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A number of lead basic sulfates are known: PbSO<sub>4</Sub>·PbO; PbSO<sub>4</Sub>·2PbO; PbSO<sub>4</Sub>·3PbO; PbSO<sub>4</Sub>·4PbO. They are used in manufacturing of active paste for lead–acid batteries. A related mineral is ], 2PbCO<sub>3</sub>·PbSO<sub>4</sub>·Pb(OH)<sub>2</sub>. |
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At high concentration of sulfuric acid (>80%), hydrogen lead sulfate, Pb(HSO<sub>4</sub>)<sub>2</sub>, forms.<ref>Министерство образования и науки РФ, Реферат "Свинец и его свойства", 2007, http://revolution.allbest.ru/chemistry/00011389_0.html</ref> |
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At high concentration of sulfuric acid (>80%), lead hydrogensulfate, Pb(HSO<sub>4</sub>)<sub>2</sub>, forms.<ref>{{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}}</ref> |
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==External links== |
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==Chemical properties== |
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Lead(II) sulfate can be dissolved in concentrated HNO<sub>3</sub>, HCl, H<sub>2</sub>SO<sub>4</sub> producing acidic salts or complex compounds, and in concentrated alkali giving soluble tetrahydroxidoplumbate(II) <sup>2−</sup> complexes. |
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{{Commons cat|Lead(II) sulfate}} |
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:{{chem2 | PbSO4(s) + H2SO4(l) <-> Pb(HSO4)2(aq) }} |
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:{{chem2 | PbSO4(s) + 4 NaOH(aq) -> Na2(aq) + Na2SO4(aq) }} |
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Lead(II) sulfate decomposes when heated above 1000 °C: |
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:{{chem2 | PbSO4(s) -> PbO(s) + SO3(g) }} |
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== Applications == |
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* ]<ref name=":0">{{Citation |title=Hazardous Substance Fact Sheet |date=September 2007 |url=https://nj.gov/health/eoh/rtkweb/documents/fs/1114.pdf}}</ref> |
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* ]s<ref name=":0" /> |
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* Laboratory reagent<ref name=":0" /> |
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== See also == |
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* ] |
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==References== |
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==References== |
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{{reflist}} |
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{{reflist}} |
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==External links== |
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{{Commons cat|Lead(II) sulfate}} |
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{{Lead compounds}} |
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{{Lead compounds}} |
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{{Sulfates}} |
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{{DEFAULTSORT:Lead(Ii) Sulfate}} |
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{{DEFAULTSORT:Lead(Ii) Sulfate}} |
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