View source for Chemistry:Lead(II) acetate

{{chembox
|Verifiedfields = changed
|Watchedfields = changed
|verifiedrevid = 449566830
|ImageFile = PbAc2 (jonowo).png
|ImageSize = 150px
|ImageName = Skeletal formula of lead(II) acetate
|ImageFile1 = Lead(II)Acetate.jpg
|ImageSize1 = 200px
|ImageName1 = Toxic lead sugar or lead(II) acetate
|IUPACName = Lead(II) acetate
|SystematicName = Lead(II) ethanoate
|OtherNames = Plumbous acetate, Salt of Saturn, Sugar of Lead, Lead diacetate
|Section1 = {{Chembox Identifiers
|CASNo = 301-04-2
|CASNo_Ref = {{cascite|correct|CAS}}
|CASNo2_Ref = {{cascite|correct|CAS}}
|CASNo2 = 6080-56-4
|CASNo2_Comment = (trihydrate)
|CASNo3_Ref = {{cascite|correct|CAS}}
|CASNo3 = 1335-32-6
|CASNo3_Comment = (basic)
|UNII_Ref = {{fdacite|correct|FDA}}
|UNII = KL498O6790
|UNII2_Ref = {{fdacite|correct|FDA}}
|UNII2 = RX077P88RY
|UNII2_Comment = (trihydrate)
|UNII3_Ref = {{fdacite|correct|FDA}}
|UNII3 = BW7DT27250
|UNII3_Comment = (basic)
|EINECS = 206-104-4
|PubChem = 16685321
|ChemSpiderID = 8956
|RTECS = OF8050000
|MeSHName = lead+acetate
|ChEBI_Ref = {{ebicite|correct|EBI}}
|ChEBI = 31767
|ChEMBL_Ref = {{ebicite|changed|EBI}}
|ChEMBL = 1909062
|KEGG_Ref = {{keggcite|correct|kegg}}
|KEGG =
|SMILES = CC(=O)[O-].CC(=O)[O-].[Pb+2]
|StdInChI = 1S/2C2H4O2.Pb/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2
|StdInChI_Ref = {{stdinchicite|changed|chemspider}}
|StdInChIKey = GUWSLQUAAYEZAF-UHFFFAOYSA-L
|StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
}}
|Section2 = {{Chembox Properties
|Formula = Pb(C<sub>2</sub>H<sub>3</sub>O<sub>2</sub>)<sub>2</sub>
|MolarMass = 325.29 g/mol (anhydrous)<br>379.33g/mol (trihydrate)
|Pb=1|C=4|H=6|O=4
|Appearance = White powder or colourless, efflorescent crystals
|Odour = Slightly acetic
|Density = 3.25 g/cm<sup>3</sup> (20 °C, anhydrous)<br>2.55 g/cm<sup>3</sup> (trihydrate)<br>1.69 g/cm<sup>3</sup> (decahydrate)<ref name=pphoic/>
|MeltingPtC = 280
|MeltingPt_notes = (anhydrous)<br>{{convert|75|C|F K}}<br>(trihydrate) decomposes<ref name="sigma"/> at ≥&nbsp;200&nbsp;°C<br>{{convert|22|C|F K}}<br>(decahydrate)<ref name=pphoic/>
|BoilingPt = Decomposes
|Solubility = Anhydrous:<br>19.8 g/100 mL (0 °C)<br>44.31 g/100 mL (20 °C)<br>69.5 g/100 mL (30 °C)<ref name=chemister>{{Cite web|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=1990|title = Lead(II) acetate}}</ref><br>218.3 g/100 mL (50 °C)<ref name=pphoic>{{cite book|last=Pradyot|first=Patnaik|year=2003|title=Handbook of Inorganic Chemicals|publisher=The McGraw-Hill Companies, Inc.|isbn=0-07-049439-8}}</ref>
|SolubleOther = Anhydrous and trihydrate are soluble in [[Chemistry:Ethanol|alcohol]], [[Chemistry:Glycerol|glycerol]]<ref name=chemister/>
|Solubility1 = Anhydrous:<ref name=chemister/><br>102.75 g/100 g (66.1 °C)<br>Trihydrate:<ref name=chemister2>{{Cite web|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=1762|title = Lead(II) acetate trihydrate}}</ref><br>74.75 g/100 g (15 °C)<br>214.95 g/100 g (66.1 °C)
|Solvent1 = methanol
|Solubility2 = Anhydrous:<ref name=chemister/><br>20 g/100 g (15 °C)<br>Trihydrate:<ref name=chemister2/><br>143 g/100 g (20 °C)
|Solvent2 = glycerol
|RefractIndex = 1.567 (trihydrate)<ref name=pphoic/>
|MagSus = &minus;89.1·10<sup>−6</sup> cm<sup>3</sup>/mol
}}
|Section3 = {{Chembox Structure
|CrystalStruct = Monoclinic (anhydrous, trihydrate)<br>Rhombic (decahydrate)
}}
|Section4 = {{Chembox Thermochemistry
|DeltaHf = −960.9 kJ/mol (anhydrous)<ref name=chemister/><br>−1848.6 kJ/mol (trihydrate)<ref name=chemister2/>
}}
|Section5 = {{Chembox Hazards
|MainHazards = Neurotoxic, probable human [[Biology:Carcinogen|carcinogen]]
|GHSPictograms = {{GHS08}} {{GHS environment}}<ref name="sigma">{{Sigma-Aldrich|id=316512|name=Lead(II) acetate trihydrate|accessdate=2014-06-08}}</ref>
|GHSSignalWord = Danger
|HPhrases = {{H-phrases|360|373|410}}<ref name="sigma"/>
|PPhrases = {{P-phrases|201|273|308+313|501}}<ref name="sigma"/>
|NFPA-H =2
|NFPA-F =1
|NFPA-R =1
|FlashPt = Non-flammable
|LD50 = 400 mg/kg (mice, oral)<ref name=pphoic/>
|LCLo = 300 mg/kg (dog, oral)<ref name=IDLH>{{IDLH|7439921|Lead compounds (as Pb)}}</ref>
}}
|Section6 = {{Chembox Related
|OtherCations = [[Chemistry:Lead(IV) acetate|Lead(IV) acetate]]
}}
}}

'''Lead(II) acetate''', also known as lead acetate, lead diacetate, plumbous acetate, sugar of lead, lead sugar, salt of [[Religion:Saturn (mythology)|Saturn]], or Goulard's powder, is a white crystalline [[Chemistry:Chemical compound|chemical compound]] with a slightly sweet taste. Its [[Chemistry:Chemical formula|chemical formula]] is usually expressed as {{chem2|Pb(CH3COO)2}} or {{chem2|Pb(OAc)2}}, where Ac represents the [[Chemistry:Acetyl group|acetyl group]]. Like many other [[Chemistry:Lead|lead]] compounds, it causes [[Medicine:Lead poisoning|lead poisoning]]. Lead acetate is soluble in water and glycerin. With water it forms the trihydrate, {{chem2|Pb(OAc)2*3H2O}}, a colourless or white efflorescent [[Chemistry:Monoclinic|monoclinic]] [[Chemistry:Crystalline|crystalline]] substance.

The substance is used as a reagent to make other lead compounds and as a fixative for some dyes. In low concentrations, it is the principal active ingredient in progressive types of hair colouring dyes.<ref name="fda.gov">{{cite web |title=Lead Acetate in 'Progressive' Hair Dye Products |url=https://www.fda.gov/cosmetics/cosmetic-products/lead-acetate-progressive-hair-dye-products |website=fda.gov|date=7 October 2021 }}</ref> Lead(II) acetate is also used as a [[Engineering:Mordant|mordant]] in textile printing and [[Chemistry:Dyeing|dyeing]], and as a [[Chemistry:Desiccant|drier]] in [[Engineering:Paint|paint]]s and varnishes. It was historically used as a [[Chemistry:Sweetener|sweetener]] and [[Chemistry:Preservative|preservative]] in wines and in other foods and for cosmetics.

==Production==
Lead(II) acetate can be made by boiling elemental lead in acetic acid and hydrogen peroxide. This method will also work with lead(II) carbonate or [[Chemistry:Lead(II) oxide|lead(II) oxide]].

:{{chem2|Pb + H2O2 + 2 H(+) → Pb(2+) + 2 H2O}}
:{{chem2|Pb(2+) + 2 AcO(-) → Pb(OAc)2}}

Lead(II) acetate can also be made by dissolving lead(II) oxide in acetic acid:<ref>{{Greenwood&Earnshaw2nd|pages=373, 388}}</ref>

:{{chem2|PbO + 2 AcOH -> Pb(OAc)2 + H2O}}

Lead(II) acetate can also be made via a [[Chemistry:Single displacement reaction|single displacement reaction]] between copper acetate and lead metal:

:{{chem2|Cu(OAc)2 + Pb → Cu + Pb(OAc)2}}

==Structure==
The [[Chemistry:Crystal structure|crystal structure]] of [[Chemistry:Anhydrous|anhydrous]] lead(II) acetate has been described as a 2D [[Chemistry:Coordination polymer|coordination polymer]]. In comparison, lead(II) acetate [[Chemistry:Hydrate|trihydrate]]'s structure is a 1D coordination polymer.<ref name="Martinez">{{cite journal |journal=Inorg. Chem. |year=2016 |volume=55 |issue=17 |pages=8576–8585 |first1=Francisco J. |last1=Martínez-Casado |first2=Miguel |last2=Ramos-Riesco |first3=José A. |last3=Rodríguez-Cheda |first4=Fabio |last4=Cucinotta |first5=Emilio |last5=Matesanz |first6=Ivana |last6=Miletto |first7=Enrica |last7=Gianotti |first8=Leonardo |last8=Marchese |first9=Zdeněk |last9=Matěj |title=Unraveling the Decomposition Process of Lead(II) Acetate: Anhydrous Polymorphs, Hydrates, and Byproducts and Room Temperature Phosphorescence |doi=10.1021/acs.inorgchem.6b01116|pmid=27548299 }}</ref> In the trihydrate, the Pb<sup>2+</sup> ion's [[Chemistry:Coordination sphere|coordination sphere]] consists of nine oxygen atoms belonging to three water molecules, two bidentate acetate groups and two bridging acetate groups. The [[Physics:Coordination geometry|coordination geometry]] at Pb is a monocapped square antiprism.<ref name="Rajaram&MohanaRao">{{cite journal |title=Crystal structure of lead acetate trihydrate |first1=R. K. |last1=Rajaram |first2=J. K. |last2=Mohana Rao |journal=Z. Kristallogr. |volume=160 |issue=1–4 |pages=225–233 |year=1982 |doi=10.1524/zkri.1982.160.14.225|s2cid=201671682 }}</ref><ref name="Etter">{{cite journal |title=Carbon-13 CP/MAS NMR and crystallographic investigations of the structure and solid-state transformations of lead(II) acetate trihydrate |first1=Robert G. |last1=Bryant |first2=V. P. |last2=Chacko |first3=Margaret C. |last3=Etter |journal=Inorg. Chem. |year=1984 |volume=23 |issue=22 |pages=3580–3584 |doi=10.1021/ic00190a029}}</ref> The trihydrate [[Physics:Thermal decomposition|thermally decomposes]] to a hemihydrate, Pb(OAc)<sub>2</sub>·{{frac|2}}H<sub>2</sub>O, and to basic acetates such as Pb<sub>4</sub>O(OAc)<sub>6</sub> and Pb<sub>2</sub>O(OAc)<sub>2</sub>.<ref name="Martinez"/>

{| class="wikitable" style="margin:1em auto; text-align:center;"
|+Comparison of anhydrous and trihydrate crystal structures
|-
!
! Anhydrous<ref name="Martinez"/><br>Pb(OAc)<sub>2</sub>
! Trihydrate<ref name="Rajaram&MohanaRao"/><ref name="Etter"/><br>Pb(OAc)<sub>2</sub>·3H<sub>2</sub>O
|-
! Lead<br>coordination<br>sphere
| [[File:Lead(II)-acetate-xtal-Pb-coordination-3D-bs-17.png|150px]]
| [[File:Lead(II)-acetate-trihydrate-xtal-Pb-coordination-3D-noH-bs-17.png|150px]]
|-
! Strongly bonded<br>aggregation
| [[File:Lead(II)-acetate-xtal-one-layer-3D-bs-17.png|200px]]<br>2D sheet
| [[File:Lead(II)-acetate-trihydrate-xtal-chain-3D-noH-bs-17.png|200px]]<br>1D chain
|-
! Weakly bonded<br>aggregation
| [[File:Lead(II)-acetate-xtal-layers-3D-bs-17.png|200px]]<br>sheets stacked with<br>[[Chemistry:Hydrophobic|hydrophobic]] surfaces in contact
| [[File:Lead(II)-acetate-trihydrate-xtal-packing-HB-3D-noH-bs-17.png|200px]]<br>chains linked by [[Chemistry:Hydrogen bond|hydrogen bond]]s
|}

==Uses==
===Sweetener===
Like other lead(II) salts, lead(II) acetate has a sweet taste, which led to its historical use as a [[Chemistry:Sugar substitute|sugar substitute]] in both wines and foods.<ref>[https://www.winemag.com/2020/07/20/lead-toxicity-wine-history/ "The Disturbingly Long History of Lead Toxicity in Winemaking."] ''Anna Archibald'', 30 July 2020. Retrieved: 22 December, 2020.</ref>
The [[History:Ancient Rome|ancient Romans]], who had few sweeteners besides [[Chemistry:Honey|honey]], would boil [[Religion:Must|must]] (unfiltered grape juice) in lead pots to produce a reduced sugar syrup called ''defrutum'', concentrated again into ''sapa''. This syrup was used to sweeten wine and to sweeten and preserve fruit. It is possible that lead(II) acetate or other lead compounds leaching into the syrup might have caused [[Medicine:Lead poisoning|lead poisoning]] in those who consumed it.<ref>[http://penelope.uchicago.edu/~grout/encyclopaedia_romana/wine/leadpoisoning.html Lead Poisoning and Rome]</ref> Lead acetate is no longer used in the production of sweeteners because of its recognized toxicity. Legislation prohibiting its use as a wine sweetener was ineffective until, decades later, chemical methods of detecting its presence had been developed.<ref>{{citation|title=Hazardous Metals in the Environment|volume=12|series=Techniques and Instrumentation in Analytical Chemistry|first=M.|last=Stoeppler|publisher=Elsevier|year=1992|isbn=9780080875606|page=60|url=https://books.google.com/books?id=x1zrlwqHlkoC&pg=PA60|quote=From the results achieved so far it is obvious that the purity law for lead in wines in the last two centuries was frequently ignored.}}</ref>

====Historical incidents====
The earliest confirmed poisoning by lead acetate was that of Pope Clement II who died in October 1047. A toxicological examination of his remains conducted in the mid-20th century confirmed centuries-old rumors that he had been poisoned with lead sugar.<ref>Specht, W. and Fischer, K. (1959). {{lang|de|italic=no|"Vergiftungsnachweis an den Resten einer 900 Jahre alten Leiche"}} [Evidence of poisoning in the remains of a 900-year-old corpse] (in German). {{lang|de|Archiv für Kriminologie}} 124: 61–84.</ref> It is not clear whether he was assassinated.

In 1787 painter and biographer Albert Christoph Dies swallowed, by accident, approximately {{cvt|3//4|oz|g|-1}} of lead acetate. His recovery from this poison was slow and incomplete. He lived with illnesses until his death in 1822.<ref name="EB1911">{{EB1911|inline=y|wstitle=Dies, Christoph Albert|volume=8|page=211}}</ref><ref name=dies>{{cite book |last=Dies |first=Albert Christoph |year=1810 |title=Biographische Nachrichten von Joseph Haydn nach mündlichen Erzählungen desselben entworfen und herausgegeben |trans-title=Biographical Accounts of Joseph Haydn, written and edited from his own spoken narratives |location=Vienna |publisher=Camesinaische Buchhandlung}} English translation in: {{cite book |last=Dies |first=Albert Christoph |chapter=Biographical Accounts of Joseph Haydn |year=1963 |editor-last=Gotwals |editor-first=Vernon |title=Haydn: Two Contemporary Portraits |translator-first=Vernon |translator-last=Gotwals |location=Milwaukee |publisher=University of Wisconsin Press |isbn=0-299-02791-0 |ref=CITEREFGotwals1963}}</ref>

Although the use of lead(II) acetate as a sweetener was already illegal at that time, composer [[History:Ludwig van Beethoven|Ludwig van Beethoven]] may have died of lead poisoning caused by wines adulterated with lead acetate (see also Beethoven's liver).<ref name="beethoven1">{{cite web |url=https://www.pharmazeutische-zeitung.de/index.php?id=magazin_30_2001 |title=Beethoven und Blei: Tödliches Zusammenspiel |access-date=2009-09-12 |url-status=live |archive-url=https://web.archive.org/web/20090221085150/http://www.pharmazeutische-zeitung.de/fileadmin/pza/2001-30/magazin.htm |archive-date=2009-02-21}}</ref><ref name="beethoven2">{{cite web |url=http://www.3sat.de/3sat.php?http%3A%2F%2Fwww.3sat.de%2Fnano%2Fnews%2F11258%2Findex.html |title=Beethoven litt unter Bleivergiftung |access-date=2020-02-24 |url-status=dead |archive-url=https://web.archive.org/web/20090221093939/http://www.3sat.de/3sat.php?http%3A%2F%2Fwww.3sat.de%2Fnano%2Fnews%2F11258%2Findex.html |archive-date=2009-02-21}}</ref>

In the 1850s, Mary Seacole applied lead(II) acetate, among other remedies, against an epidemic of [[Medicine:Cholera|cholera]] in Panama.<ref name="SeacoleIV">Mary Seacole (1990), ''Wonderful Adventures of Mrs. Seacole in Many Lands'', Chapter IV, [[Organization:Oxford University Press|Oxford University Press]] reprint, {{ISBN|0-19-506672-3}}; (2005 Penguin 20th Century Classics reprint, ed. Sarah Salih) {{ISBN|0-14-043902-1}}</ref><ref name="Robinson">Jane Robinson (2004), ''Mary Seacole: The Charismatic Black Nurse who became a heroine of the Crimea'', p.53. Constable {{ISBN|1-84119-677-0}}</ref>

In 1887, 38 hunting horses belonging to Captain William Hollwey Steeds were poisoned in their stables at Clonsilla House, Dublin, Ireland. At least ten of the hunters died. Captain Steeds, an "extensive commission agent", had previously supplied the horses for the Bray and Greystones Coach. It transpired that they had been fed a bran mash that had been sweetened with a toxic lead acetate.<ref>''Weekly Irish Times'', Saturday 15 October 1887; ''Enniskillen Chronicle'' and ''Erne Packet'', 24 October 1887, p. 3</ref>

===Cosmetics===
Lead(II) acetate, as well as [[Chemistry:White lead|white lead]], has been used in cosmetics throughout history.<ref>Gunn, Fenja. (1973) The Artificial Face: A History of Cosmetics. &mdash; as cited in [http://websites.umich.edu/~ece/student_projects/leisure/leadfacepowder.html Leisure Activities of an 18th Century Lady]</ref>

Until recently,{{when|date=June 2022}} it was still used in the USA in men's hair colouring products<ref name="Hair">''[https://web.archive.org/web/20081204121726/http://www.uwsp.edu/geo/courses/geog100/MielkeHairLead4.htm Lead Based Hair Products: Too Hazardous for Household Use - Results]'', Howard W. Mielke, PhD, Myiesha D. Taylor, Chris R. Gonzales, M. Kelley Smith, Pamela V. Daniels, and Ayanna V.Buckner. Journal of American Pharmaceutical Association (NS37, Jan/Feb 1997:85-89).</ref> like Grecian Formula. It was not until 2018 that the manufacturer removed lead acetate from the hair coloring product. Lead acetate has been replaced by bismuth citrate as the progressive colorant. Its use in cosmetics has been banned in Canada by [[Organization:Health Canada|Health Canada]] since 2005 (effective at the end of 2006) based on tests showing possible carcinogenicity and reproductive toxicity,<ref name="canada.com">{{cite web |url=http://www.canada.com/montreal/montrealgazette/news/story.html?id=6caa01c2-3fb0-4431-a559-43aeece93860 |title=Can West News Service: Grecian Formula in a grey zone after ban |url-status=dead |archive-url=https://web.archive.org/web/20070808083503/http://www.canada.com/montreal/montrealgazette/news/story.html?id=6caa01c2-3fb0-4431-a559-43aeece93860 |archive-date=2007-08-08}}</ref> and it is also banned in the European Union<ref name="canada.com"/> and has been on the California Proposition 65 warning list as a carcinogen since 1988.<ref>{{cite web |url=https://oehha.ca.gov/proposition-65/proposition-65-list |title=The Proposition 65 List |access-date=2014-11-01 |url-status=live |archive-url=https://web.archive.org/web/20141031102829/http://www.oehha.ca.gov/prop65/prop65_list/files/P65single060614.pdf |archive-date=2014-10-31}}</ref>

===Medical uses===
Lead(II) acetate solution was a commonly used folk remedy for sore nipples.<ref>[https://www.gutenberg.org/files/13493/13493-h/13493-h.htm The American Frugal Housewife, by Lydia M. Child]</ref> In modern medicine, for a time, it was used as an astringent, in the form of Goulard's extract, and it has also been used to treat [[Biology:Poison ivy|poison ivy]].<ref>Laboratory manual in biology. Sharpe. 1911, American Book Company. p. 351</ref>

===Industrial uses===
Lead(II) acetate paper is used to detect the poisonous gas [[Chemistry:Hydrogen sulfide|hydrogen sulfide]]. The gas reacts with lead(II) acetate on the moistened test paper to form a grey precipitate of [[Chemistry:Lead(II) sulfide|lead(II) sulfide]].

An aqueous solution of lead(II) acetate is the byproduct of a 1:1 ratio of [[Chemistry:Hydrogen peroxide|hydrogen peroxide]] and white [[Chemistry:Vinegar|vinegar]] (acetic acid) used in the cleaning and maintenance of stainless steel [[Engineering:Firearm|firearm]] suppressors (silencers) and [[Engineering:Muzzle brake|compensators]]. The solution is agitated by the bubbling action of the hydrogen peroxide, with the main reaction being the oxidation of lead by hydrogen peroxide and subsequent dissolution of lead oxide by the acetic acid, which forms lead acetate. Because of its high toxicity, this chemical solution must be appropriately disposed by a chemical processing facility or hazardous materials centre. Alternatively, the solution may be reacted with [[Chemistry:Sulfuric acid|sulfuric acid]] to precipitate nearly insoluble [[Chemistry:Lead(II) sulfate|lead(II) sulfate]]. The solid may then be removed by mechanical filtration and is safer to dispose of than aqueous lead acetate.
===Other uses===
It was also used in making of [[Engineering:Slow match|slow match]]es during the [[History:Middle Ages|Middle Ages]]. It was made by mixing a natural form of lead(II) oxide called [[Chemistry:Litharge|litharge]] and [[Chemistry:Vinegar|vinegar]].

Sugar of lead was a recommended agent added to linseed oil during heating to produce "boiled" [[Biology:Linseed oil|linseed oil]], the lead and heat acting to cause the oil to cure faster than raw linseed oil.<ref>Andés, Louis Edgar, and Arthur Morris. ''Oil colours and printers' inks a practical handbook treating of linseed oil, boiled oil, paints, artists' colours, lampblack and printers' inks, black and coloured''. London: Scott, Greenwood. 1903. 41. Print.</ref>

Lead(II) acetate ("salt of Saturn") was used to synthesise [[Chemistry:Acetone|acetone]] which was then known as "spirit of Saturn" for being made with the salt of Saturn and thought to be a lead compound in the 17th century.<ref>Mel Gorman, History of acetone (1600-1850), 1962</ref>

==See also==
* Saturn's Tree

==References==
{{Reflist}}

==External links==
* [https://www.atsdr.cdc.gov/csem/csem.html Case Studies in Environmental Medicine - Lead Toxicity]
* [http://penelope.uchicago.edu/~grout/encyclopaedia_romana/wine/leadpoisoning.html Essay on "Lead Poisoning and Rome"]
* [https://science.howstuffworks.com/innovation/everyday-innovations/hair-coloring6.htm HowStuffWorks "What Kind of Hair Color Do Men Use?" discussion of progressive dyes containing lead acetate]
* [https://web.archive.org/web/20080111154608/http://www.npi.gov.au/database/substance-info/profiles/50.html National Pollutant Inventory - Lead and Lead Compounds Fact sheet (Does Not Bring Up Lead)]
* [https://wwwn.cdc.gov/TSP/ToxFAQs/ToxFAQsLanding.aspx?id=93&tid=22 ToxFAQs: Lead]
* [https://web.archive.org/web/20070705040143/http://vm.cfsan.fda.gov/~dms/cos-lead.html US Food and Drug Administration (FDA) fact sheet "Lead Acetate in Hair Dye Products"]
* [https://www.accessdata.fda.gov/scripts/cdrh/cfdocs/cfcfr/CFRSearch.cfm?fr=73.2396 US Food and Drug Administration (FDA)21CFR73.2396 "PART 73 -- LISTING OF COLOR ADDITIVES EXEMPT FROM CERTIFICATION, Subpart C--Cosmetics, Sec. 73.2396 Lead acetate"]

{{Lead compounds}}
{{Acetates}}

[[Category:Acetates]]
[[Category:Lead(II) compounds]]
[[Category:Sugar substitutes]]

{{Sourceattribution|Lead(II) acetate}}