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	{{chembox		{{Chembox
			|Verifiedfields = changed
	| verifiedrevid = 442940804
			|Watchedfields = changed
	| ImageFile = Lead(II)Acetate.jpg
			|verifiedrevid = 449566830
	| ImageSize = 200px
			|ImageFile = PbAc2 (jonowo).png
	| IUPACName = Lead(II) ethanoate
			|ImageSize = 150px
	| SystematicName = Lead(II) ethanoate
			|ImageName = Skeletal formula of lead(II) acetate
	| OtherNames = Plumbous acetate, Salt of Saturn, Sugar of Lead, lead diacetate
			|ImageFile1 = Lead(II)Acetate.jpg
	| Section1 = {{Chembox Identifiers
			|ImageSize1 = 200px
	| Abbreviations =
			|ImageName1 = Toxic lead sugar or lead(II) acetate
	| CASNo = 301-04-2
			|IUPACName = Lead(II) acetate
	| CASNo_Ref = {{cascite}}
			|SystematicName = Lead(II) ethanoate
	| CASOther = <br> 6080-56-4 (trihydrate) <br> 51404-69-4 (Basic)
			|OtherNames = Plumbous acetate, Sugar of Lead, lead diacetate, lead sugar, Salt of ], ] powder
	| EINECS =
			|Section1 = {{Chembox Identifiers
	| EINECSCASNO =
			|CASNo = 301-04-2
	| PubChem =
			|CASNo_Ref = {{cascite|correct|CAS}}
	| RTECS =
			|CASNo2_Ref = {{cascite|correct|CAS}}
	| MeSHName =
			|CASNo2 = 6080-56-4
	| ChEBI_Ref = {{ebicite|correct|EBI}}
			|CASNo2_Comment = (trihydrate)
	| ChEBI =
	| KEGG_Ref = {{keggcite|correct|kegg}}		|CASNo3_Ref = {{cascite|correct|CAS}}
			|CASNo3 = 1335-32-6
	| KEGG =
			|CASNo3_Comment = (basic)
	| ATCCode_prefix =
			|UNII_Ref = {{fdacite|correct|FDA}}
	| ATCCode_suffix =
			|UNII = KL498O6790
	| ATC_Supplemental =}}
			|UNII2_Ref = {{fdacite|correct|FDA}}
	| Section2 = {{Chembox Properties
			|UNII2 = RX077P88RY
	| 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)		|UNII2_Comment = (trihydrate)
			|UNII3_Ref = {{fdacite|correct|FDA}}
	| Appearance = White powder or colorless, efflorescent crystals
			|UNII3 = BW7DT27250
	| Density = 3.25 g/cm<sup>3</sup> (anhydrous) <br> 2.55 g/cm<sup>3</sup> (trihydrate) <br> 1.69 g/cm<sup>3</sup> (decahydrate)
			|UNII3_Comment = (basic)
	| MeltingPt = 280 °C (anhydrous) <br> 75 °C (trihydrate) <br> 22 °C (decahydrate)
			|EINECS = 206-104-4
	| BoilingPt =
			|PubChem = 16685321
	| Boiling_notes = decomposes
			|ChemSpiderID = 8956
	| Solubility = 44.39 g/100 mL (20 °C) <br> 211 g/100 mL (50 °C)<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0-07-049439-8</ref>
			|RTECS = OF8050000
	| SolubleOther = anhydrous soluble in ]; hydrates insoluble in alcohol
			|MeSHName = lead+acetate
	| Solvent =
			|ChEBI_Ref = {{ebicite|correct|EBI}}
	| LogP =
			|ChEBI = 31767
	| VaporPressure =
			|ChEMBL_Ref = {{ebicite|changed|EBI}}
	| HenryConstant =
			|ChEMBL = 1909062
	| AtmosphericOHRateConstant =
			|KEGG_Ref = {{keggcite|correct|kegg}}
	| pKa =
	| pKb =		|KEGG =
			|SMILES = CC(=O).CC(=O).
	| RefractIndex = 1.567 (trihydrate)
			|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 |title=Lead(II) acetate |website=chemister.ru |url=http://chemister.ru/Database/properties-en.php?dbid=1&id=1990}}</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 ], ]<ref name=chemister/>
			|Solubility1 = Anhydrous:<ref name=chemister/><br>102.75 g/100 g (66.1 °C)<br>Trihydrate:<ref name=chemister2>{{cite web |title=Lead(II) acetate trihydrate |website=chemister.ru |url=http://chemister.ru/Database/properties-en.php?dbid=1&id=1762}}</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 = ], probable human ]
			|GHSPictograms = {{GHS08}} {{GHS environment}}<ref name="sigma">{{Sigma-Aldrich|id=316512|name=Lead(II) acetate trihydrate|access-date=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 = ]
	}}		}}
	| Section3 = {{Chembox Structure
	| CrystalStruct = Monoclinic
	| Coordination =
	| MolShape = }}
	| Section4 = {{Chembox Thermochemistry
	| DeltaHf =
	| DeltaHc =
	| Entropy =
	| HeatCapacity = }}
	| Section5 = {{Chembox Pharmacology
	| AdminRoutes =
	| Bioavail =
	| Metabolism =
	| HalfLife =
	| ProteinBound =
	| Excretion =
	| Legal_status =
	| Legal_US =
	| Legal_UK =
	| Legal_AU =
	| Legal_CA =
	| PregCat =
	| PregCat_AU =
	| PregCat_US = }}
	| Section6 = {{Chembox Explosive
	| ShockSens =
	| FrictionSens =
	| ExplosiveV =
	| REFactor = }}
	| Section7 = {{Chembox Hazards
	| EUClass =
	| EUIndex =
	| MainHazards = Neurotoxic, Probable Human Carcinogen
	| NFPA-H = 3
	| NFPA-F = 1
	| NFPA-R = 0
	| NFPA-O =
	| RPhrases =
	| SPhrases =
	| RSPhrases =
	| FlashPt = Nonflammable
	| Autoignition =
	| ExploLimits =
	| PEL = }}
	| Section8 = {{Chembox Related
	| OtherAnions =
	| OtherCations =
	| OtherFunctn =
	| Function =
	| OtherCpds = }}
	}}		}}
	'''Lead(II) acetate''' (Pb(CH<sub>3</sub>COO)<sub>2</sub>), also known as '''lead acetate''', '''lead diacetate''', '''plumbous acetate''', '''sugar of lead''', '''lead sugar''', '''salt of ]''', and '''] powder''', is a white crystalline ] with a ]ish taste. It is made by treating ] with ]. Like other lead compounds, it is ]. Lead acetate is soluble in ] and ]. With water it forms the trihydrate, Pb(CH<sub>3</sub>COO)<sub>2</sub>·3H<sub>2</sub>O, a colorless or white ] ] ] substance.
			'''Lead(II) acetate''' is a white crystalline ] with a slightly ]. Its ] is usually expressed as {{chem2|Pb(CH3COO)2}} or {{chem2|Pb(OAc)2}}, where Ac represents the ]. Like many other ] compounds, it causes ]. Lead acetate is soluble in water and ]. With water it forms the trihydrate, {{chem2|Pb(OAc)2*3H2O}}, a colourless or white ] ] ] 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 ] dyes. Lead(II) acetate is also used as a ] in ] and ], as a ] in ] and ], and in preparing other lead compounds.
			The substance is used as a reagent to make other lead compounds and as a fixative for some dyes. In low concentrations, it formerly served as the principal active ingredient in progressive types of ] dyes.<ref name="fda.gov">{{cite web |title=Lead Acetate in 'Progressive' Hair Dye Products |date=7 October 2021 |website=fda.gov |url=https://www.fda.gov/cosmetics/cosmetic-products/lead-acetate-progressive-hair-dye-products}}</ref> Lead(II) acetate is also used as a ] in ] and ], and as a ] in ]s and ]es. It was historically used as a ] and ] in wines and in other foods and for ].
			==Production==
			Lead(II) acetate can be made by boiling elemental lead in acetic acid and hydrogen peroxide. This method will also work with ] or ].
			:{{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 ] between ] and lead metal:
			:{{chem2|Cu(OAc)2 + Pb → Cu + Pb(OAc)2}}
			==Structure==
			The ] of ] lead(II) acetate has been described as a 2D ]. In comparison, lead(II) acetate ]'s structure is a 1D coordination polymer.<ref name="Martinez">{{cite journal |journal=] |year=2016 |volume=55 |issue=17 |pages=8576–8585 |last1=Martínez-Casado |first1=Francisco J. |last2=Ramos-Riesco |first2=Miguel |last3=Rodríguez-Cheda |first3=José A. |last4=Cucinotta |first4=Fabio |last5=Matesanz |first5=Emilio |last6=Miletto |first6=Ivana |last7=Gianotti |first7=Enrica |last8=Marchese |first8=Leonardo |last9=Matěj |first9=Zdeněk |title=Unraveling the Decomposition Process of Lead(II) Acetate: Anhydrous Polymorphs, Hydrates, and Byproducts and Room Temperature Phosphorescence |pmid=27548299 |doi=10.1021/acs.inorgchem.6b01116}}</ref> In the trihydrate, the Pb<sup>2+</sup> ion's ] consists of nine oxygen atoms belonging to three water molecules, two bidentate acetate groups and two bridging acetate groups. The ] at Pb is a monocapped square antiprism.<ref name="Rajaram&MohanaRao">{{cite journal |title=Crystal structure of lead acetate trihydrate |last1=Rajaram |first1=R. K. |last2=Mohana Rao |first2=J. K. |journal=] |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 |last1=Bryant |first1=Robert G. |last2=Chacko |first2=V. P. |last3=Etter |first3=Margaret C. |authorlink3=Margaret C. Etter |journal=] |year=1984 |volume=23 |issue=22 |pages=3580–3584 |doi=10.1021/ic00190a029}}</ref> The trihydrate ] 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
			| ]
			| ]
			|-
			! Strongly bonded<br>aggregation
			| ]<br>2D sheet
			| ]<br>1D chain
			|-
			! Weakly bonded<br>aggregation
			| ]<br>sheets stacked with<br>] surfaces in contact
			| ]<br>chains linked by ]s
			|}
	==Uses==		==Uses==
			Lead acetate is used as a precursor to other lead compounds such as the various carbonate.
			===Niche and laboratory uses===
			Lead(II) acetate paper is used to detect the poisonous gas ]. The gas reacts with lead(II) acetate on the moistened test paper to form a grey precipitate of ].
			An aqueous solution of lead(II) acetate is a byproduct of the process used in the cleaning and maintenance of stainless steel ] ]s (silencers) and ] when using a 1:1 ratio of ] and white ] (acetic acid). 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 ] centre. Alternatively, the solution may be reacted with ] to precipitate nearly insoluble ]. The solid may then be removed by mechanical filtration and is safer to dispose of than aqueous lead acetate.
			==Historical uses==
	===Sweetener===		===Sweetener===
			Like other lead(II) salts, lead(II) acetate has a sweet taste, which led to its historical use as a ] in both wines and foods.<ref> ''Anna Archibald'', 30 July 2020. Retrieved: 22 December, 2020.</ref>
	Like other lead(II) salts, lead(II) acetate has a sweet taste, which has led to its use as a ] throughout history. The ], who had few sweeteners besides ], would boil ] (grape juice) in lead pots to produce a reduced sugar syrup called '']'', concentrated again into '']''. This syrup was used to sweeten wine and to sweeten and preserve fruit. It is possible that lead(II) acetate or other lead compounds ] into the syrup might have caused ] in anyone consuming it.<ref></ref> Therefore, lead acetate is no longer used as a sweetener in most of the world because of its recognized toxicity. Modern chemistry can easily detect it, which has all but stopped the illegal use that continued decades after legal use as a sweetener was terminated.
			The ], who had few sweeteners besides ], would boil ] (unfiltered grape juice) in lead pots to produce a reduced sugar syrup called '']'', concentrated again into '']''. This syrup was used to sweeten wine and to sweeten and preserve fruit. It is possible that lead(II) acetate or other lead compounds ] into the syrup might have caused ] in those who consumed it.<ref>{{cite web |title=Lead Poisoning and Rome |website=penelope.uchicago.edu |url=https://penelope.uchicago.edu/~grout/encyclopaedia_romana/wine/leadpoisoning.html |access-date=5 May 2024}}</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, when 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 |last=Stoeppler |first=M. |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>
			The earliest confirmed poisoning by lead acetate was that of ], 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"}} (in German). {{lang|de|Archiv für Kriminologie}} 124: 61–84.</ref> It is not clear whether he was assassinated.
	====Resultant deaths====
	] died in October 1047. A recent toxicologic examination{{Citation needed|date=June 2007}} of his remains confirmed centuries-old rumors that he had been poisoned with lead sugar. It is not clear if he was assassinated.
	In 1787 painter ] swallowed, by accident, approximately {{convert|0.75|oz|0}} of lead acetate. His recovery from this poison was slow and incomplete. He lived with illnesses until his death in 1822.{{Citation needed|date=November 2009}}		In 1787 painter and biographer ] swallowed, by accident, approximately {{convert|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 |author-link=Albert Christoph Dies |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 ] may have died of lead poisoning caused by wines adulterated with lead acetate.<ref name="beethoven1"></ref><ref name="beethoven2"></ref>		Although the use of lead(II) acetate as a sweetener was already illegal at that time, composer ] may have died of lead poisoning caused by wines adulterated with lead acetate (see also ]).<ref name="beethoven1">{{cite web |title=Beethoven und Blei: Tödliches Zusammenspiel |trans-title=Beethoven and lead: deadly interaction |website=pharmazeutische-zeitung.de |url=https://www.pharmazeutische-zeitung.de/magazin-30-2001 |access-date=2024-12-17 |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 |title=Beethoven litt unter Bleivergiftung |trans-title=Beethoven suffered from lead poisoning |website=3sat.de |url=http://www.3sat.de/3sat.php?http%3A%2F%2Fwww.3sat.de%2Fnano%2Fnews%2F11258%2Findex.html |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 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>
	] applied lead(II) acetate, among other remedies, against an epidemic of ] in Panama.<ref name="SeacoleIV">]: ''Wonderful Adventures of Mrs. Seacole in Many Lands'', Chapter IV, (1990 ] reprint) ISBN 0-19-506672-3; (2005 Penguin 20th Century Classics reprint, ed. ]) ISBN 0-14-043902-1</ref><ref name="Robinson">]: ''Mary Seacole: The Charismatic Black Nurse who became a heroine of the Crimea'', p.53. Constable 2004 (p/b. ISBN 1-84119-677-0)</ref>
	===Other uses===		===Cosmetics===
	Lead(II) acetate, as well as ], have been used in cosmetics throughout history, though this practice has ceased in Western countries.<ref>Gunn, Fenja. (1973). The Artificial Face: A History of Cosmetics. &mdash; as cited in <!-- also, F.D.A --></ref>		Lead(II) acetate and ] have been used in cosmetics throughout history.<ref>Gunn, Fenja. (1973) The Artificial Face: A History of Cosmetics. &mdash; as cited in websites.umich.edu</ref>
	It is still used in men's ] products<ref name="Hair">'''', ], PhD, ], ], ], ], and ]. ] (NS37, Jan/Feb 1997:85-89).</ref> like ].
			It was once used for men's ] products<ref name="Hair">'''', 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 ]. The manufacturer did not remove lead acetate from its product until 2018. Lead acetate has been replaced by bismuth citrate as the progressive colorant. Its use in cosmetics has been banned in Canada by ] since 2005 (effective at the end of 2006) based on tests showing possible carcinogenicity and reproductive toxicity,<ref name="canada.com">{{cite web |title=Can West News Service: Grecian Formula in a grey zone after ban |website=canada.com |url=http://www.canada.com/montreal/montrealgazette/news/story.html?id=6caa01c2-3fb0-4431-a559-43aeece93860 |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"/>
	Lead(II) acetate paper is used to detect the poisonous gas ]. The gas reacts with lead(II) acetate on the moistened test paper to form a grey precipitate of ].
			===Medical uses===
	Lead(II) acetate solution was a commonly used folk remedy for sore nipples.<ref></ref>
	In modern medicine, for a time, it was used as an ], in the form of ].		Lead(II) acetate solution was a commonly used folk remedy for sore nipples.<ref> gutenberg.org</ref> In modern medicine, for a time, it was used as an ], in the form of ], and it has also been used to treat ].<ref>Laboratory manual in biology. Sharpe. 1911, American Book Company. p. 351</ref>
			In the 1850s, ] applied lead(II) acetate, among other remedies, against an epidemic of ] in Panama.<ref name="SeacoleIV">] (1990), ''Wonderful Adventures of Mrs. Seacole in Many Lands'', Chapter IV, ] reprint, {{ISBN|0-19-506672-3}}; (2005 Penguin 20th Century Classics reprint, ed. Sarah Salih) {{ISBN|0-14-043902-1}}</ref><ref name="Robinson">] (2004), ''Mary Seacole: The Charismatic Black Nurse who became a heroine of the Crimea'', p.53. Constable {{ISBN|1-84119-677-0}}</ref>
	An aqueous solution of lead(II) acetate is the byproduct of the 50/50 mixture of ] and white ] used in the cleaning and maintenance of stainless steel ] ]s (silencers) and ]. The solution is agitated by the bubbling action of the hydrogen peroxide, and the main reaction is the dissolution of lead deposits within the suppressor 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 ] center. Alternatively, the solution may be reacted with ] to precipitate insoluble lead(II) sulfate. The solid may then be removed by mechanical filtration and is safer to dispose of than aqueous lead acetate.
			===Other historic uses===
	It was also used in making of ] during the ]. It was made by mixing natural form of lead(II) oxide called ] and ].
			It was also used in making of ]es during the ]. It was made by mixing a natural form of lead(II) oxide called ] and ].
			Sugar of lead was a recommended agent added to linseed oil during heating to produce "boiled" ], 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 has also been used to treat ]. {{Citation needed|date=September 2011}}
			Lead(II) acetate ("salt of Saturn") was used to synthesise ] 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>
	==Precautions==
	Lead(II) acetate, as with any other lead ], causes ].
			==See also==
			* ]
	==References==		==References==
	{{reflist}}		{{Reflist}}
	==External links==		==External links==
	{{Commons cat|Lead(II) acetate}}		{{Commons category|Lead(II) acetate}}
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	{{Lead compounds}}		{{Lead compounds}}
			{{Acetates}}
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