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	<!--redirects here: lead (II) chloride, lead dichloride, lead chloride, plumbous chloride, pbcl2-->		<!--redirects here: lead (II) chloride, lead dichloride, lead chloride, plumbous chloride, pbcl2-->
	{{chembox		{{chembox
			| Verifiedfields = changed
⚫	| verifiedrevid = 443915937
			| Watchedfields = changed
⚫	| Name = Lead(II) chloride
		⚫	| verifiedrevid = 444947478
⚫	| ImageFile = Lead(II) chloride.jpg
		⚫	| Name = Lead(II) chloride
	| ImageFile1 = Kristallstruktur Blei(II)-chlorid.png
	| ImageName = Lead(II) chloride		| ImageFile = Lead(II) chloride.jpg
			| ImageFile1 = Cotunnite structure.png
⚫	| IUPACName = Lead(II) chloride<br/>Lead dichloride
			| ImageCaption1 = The crystal structure of PbCl<sub>2</sub>, in the unconventional crystallographic setting Pnam. This corresponds to the standard Pnma setting by switching the labels on the b and c axes.
⚫	| OtherNames = Plumbous chloride<br/>]
		⚫	| ImageName = Lead(II) chloride
⚫	| Section1 = {{Chembox Identifiers
		⚫	| IUPACName = Lead(II) chloride<br/>Lead dichloride
		⚫	| OtherNames = Plumbous chloride<br/>]<br />Dichloroplumbylene
		⚫	| Section1 = {{Chembox Identifiers
			| CASNo_Ref = {{cascite|correct|CAS}}
	| CASNo = 7758-95-4		| CASNo = 7758-95-4
	| CASNo_Ref = {{cascite}}		| UNII_Ref = {{fdacite|changed|FDA}}
			| UNII = 4IL61GN3YI
	| PubChem = 166945		| PubChem = 166945
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 22867		| ChemSpiderID = 22867
			| ChEBI_Ref = {{ebicite|changed|EBI}}
			| ChEBI = 88212
			| EINECS = 231-845-5
	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = HWSZZLVAJGOAAY-UHFFFAOYSA-L		| StdInChIKey = HWSZZLVAJGOAAY-UHFFFAOYSA-L
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	| StdInChI = 1S/2ClH.Pb/h2*1H;/q;;+2/p-2		| StdInChI = 1S/2ClH.Pb/h2*1H;/q;;+2/p-2
	}}		}}
	| Section2 = {{Chembox Properties		| Section2 = {{Chembox Properties
	| Formula = PbCl<sub>2</sub>		| Formula = PbCl<sub>2</sub>
	| MolarMass = 278.10 g/mol		| MolarMass = 278.10&nbsp;g/mol
	| Appearance = white odorless solid		| Appearance = white odorless solid
	| Density = 5.85 g/cm<sup>3</sup>		| Density = 5.85&nbsp;g/cm<sup>3</sup>
			| Solubility = 0.99&nbsp;g/100 mL (20&nbsp;°C)<ref> {{webarchive|url=https://web.archive.org/web/20140211021914/https://www.nist.gov/data/PDFfiles/jpcrd166.pdf |date=2014-02-11 }}</ref>
	| Solubility = 6.73 g/L (0 °C) <br> 9.9 g/L (20 °C) <br> 33.4 g/L (100 °C)
	| SolubilityProduct = 1.7{{e|-5}}		| SolubilityProduct = 1.7×10<sup>−5</sup> (20&nbsp;°C)
	| SolubleOther = slightly soluble in dilute ], ]; <br> insoluble in ]		| SolubleOther = slightly soluble in dilute ], ]; <br> insoluble in ]
	| MeltingPt = 501 °C
			Soluble in hot ] as well as in presence of ]
	| BoilingPt = 950 °C
⚫	| RefractIndex = 2.199<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0-07-049439-8</ref>
			Soluble in concentrated ] (>6M)
			| MeltingPtC = 501
			| BoilingPtC = 950
		⚫	| RefractIndex = 2.199<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}</ref>
			| MagSus = &minus;73.8·10<sup>−6</sup> cm<sup>3</sup>/mol
	}}		}}
	| Section3 = {{Chembox Structure		| Section3 = {{Chembox Structure
			| Structure_ref =<ref>{{cite journal | last=Sass | first=Ronald L. | last2=Brackett | first2=E. B. | last3=Brackett | first3=T. E. | title=THE CRYSTAL STRUCTURE OF LEAD CHLORIDE | journal=The Journal of Physical Chemistry | publisher=American Chemical Society (ACS) | volume=67 | issue=12 | year=1963 | issn=0022-3654 | doi=10.1021/j100806a517 | pages=2863–2864}}</ref>
	| CrystalStruct = ], ]		| CrystalStruct = ], ]
	| SpaceGroup = Pnma, No. 62		| SpaceGroup = Pnma (No. 62)
			| LattConst_a = 762.040 pm
			| LattConst_b = 453.420 pm
			| LattConst_c = 904.520 pm
			| UnitCellFormulas = 4
	}}		}}
	| Section4 = {{Chembox Thermochemistry		| Section4 = {{Chembox Thermochemistry
	| DeltaHf = -359.41 kJ/mol		| DeltaHf = -359.41&nbsp;kJ/mol
	| Entropy = 135.98 J&thinsp;K<sup>−1</sup>&thinsp;mol<sup>−1</sup>		| Entropy = 135.98&nbsp;J{{thin space}}K<sup>−1</sup>{{thin space}}mol<sup>−1</sup>
	}}		}}
	| Section7 = {{Chembox Hazards		| Section7 = {{Chembox Hazards
	| EUClass = Repr. Cat. 1/3<br/>Harmful ('''Xn''')<br/>Dangerous for the environment ('''N''')
	| EUIndex = 082-001-00-6
	| NFPA-H = 3		| NFPA-H = 3
	| NFPA-F = 0		| NFPA-F = 0
	| NFPA-R = 0		| NFPA-R = 0
			| Hazards_ref = <ref>{{cite web |title=Classifications - CL Inventory |url=https://echa.europa.eu/information-on-chemicals/cl-inventory-database/-/discli/details/10492 |website=echa.europa.eu}}</ref>
	| RPhrases = {{R61}}, {{R20/22}}, {{R33}}, {{R62}}, {{R50/53}}
	| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}}		| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}}
			| GHSSignalWord = Danger
			| HPhrases = {{H-phrases|302|332|351|360|372|410}}
			| PPhrases = {{P-phrases|201|261|273|304+340|308+313|312|391}}
			| LDLo = 140 mg/kg (guinea pig, oral)<ref name=IDLH>{{IDLH|7439921|Lead compounds (as Pb)}}</ref>
	}}		}}
	| Section8 = {{Chembox Related		| Section8 = {{Chembox Related
	| OtherAnions = ]<br/>]<br/>]		| OtherAnions = ]<br/>]<br/>]
	| OtherCations = ]<br/>]<br/>]		| OtherCations = ]<br/>]<br/>]
	| OtherCpds = ]<br/>]		| OtherCompounds = ]<br/>]
	}}		}}
	}}		}}
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	==Structure and properties==		==Structure and properties==
	In solid PbCl<sub>2</sub>, each lead ion is coordinated by 9 chloride ions – 6 lie at the apices of a trigonal prism and 3 lie beyond the centers of each prism face. The 9 chloride ions are not equidistant from the central lead atom, 7 lie at 280–309 pm and 2 at 370 pm.<ref>Wells A.F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications ISBN 0-19-855370-6</ref> PbCl<sub>2</sub> forms white orthorhombic needles.		In solid PbCl<sub>2</sub>, each lead ion is coordinated by nine chloride ions in a ] — six lie at the vertices of a triangular prism and three lie beyond the centers of each rectangular prism face. The 9 chloride ions are not equidistant from the central lead atom, 7 lie at 280–309&nbsp;pm and 2 at 370&nbsp;pm.<ref>Wells A. F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications {{ISBN|0-19-855370-6}}</ref> PbCl<sub>2</sub> forms white orthorhombic needles.
			{{gallery
⚫	Vaporized PbCl<sub>2</sub> molecules have a bent structure with the Cl-Pb-Cl angle being 98° and each Pb-Cl bond distance being 2.44 Å.<ref>{{cite journal|last1 = Hargittai|first1 = I|last2 = Tremmel|first2 = J|last3 = Vajda|first3 = E|last4 = Ishchenko|first4 = A|last5 = Ivanov|first5 = A|last6 = Ivashkevich|first6 = L|last7 = Spiridonov|first7 = V|title = Two independent gas electron diffraction investigations of the structure of plumbous chloride|journal = Journal of Molecular Structure|volume = 42|pages = 147|year = 1977|doi = 10.1016/0022-2860(77)87038-5}}</ref> Such PbCl<sub>2</sub> is emitted from internal combustion engines that use ethylene chloride-] additives for antiknock purposes.
			|File:Cotunnite-3D-balls.png|] of part of the ] of cotunnite
			|File:Cotunnite-3D-ionic.png|]
⚫	The ] of PbCl<sub>2</sub> in water is low (9.9 g/L at 20 °C) and for practical purposes it is considered insoluble. Its ] (K<sub>sp</sub>) is 1.7{{e|-5|}}. It is one of only four commonly insoluble chlorides, the other three being ] (AgCl) with K<sub>sp</sub> = 1.8{{e|−10}}, ] (CuCl) with K<sub>sp</sub> = 1.72{{e|−7}} and ] (Hg<sub>2</sub>Cl<sub>2</sub>) with K<sub>sp</sub> = 1.3{{e|−18}}.<ref>CRC Handbook of Chemistry and Physics, 79th Edition, David R. Lide (Ed), p. 8-108</ref><ref>Brown, Lemay, Burnsten. "Chemistry The Central Science". ''Solubility-Product Constants for Compounds at 25 °C.'' (ed 6, 1994). p. 1017</ref>
			|File:Cotunnite-Pb-coordination-geometry-3D-balls.png|] of Pb<sup>2+</sup>
			|File:Cotunnite-Cl-coordination-geometry-3D-balls.png|Coordination geometry of Cl<sup>−</sup>
			|File:Cotunnite-Pb-coordination-CM-3D-balls.png|Coordination polyhedron of Pb<sup>2+</sup>
			}}
		⚫	In the gas phase, PbCl<sub>2</sub> molecules have a bent structure with the Cl–Pb–Cl angle being 98° and each Pb–-Cl bond distance being 2.44&nbsp;Å.<ref>{{cite journal|last1 = Hargittai|first1 = I|last2 = Tremmel|first2 = J|last3 = Vajda|first3 = E|last4 = Ishchenko|first4 = A|last5 = Ivanov|first5 = A|last6 = Ivashkevich|first6 = L|last7 = Spiridonov|first7 = V|title = Two independent gas electron diffraction investigations of the structure of plumbous chloride|journal = Journal of Molecular Structure|volume = 42|pages = 147–151|year = 1977|doi = 10.1016/0022-2860(77)87038-5|bibcode = 1977JMoSt..42..147H}}</ref> Such PbCl<sub>2</sub> is emitted from internal combustion engines that use ethylene chloride-] additives for antiknock purposes.
	==Occurrence==
	] of cotunnite, PbCl<sub>2</sub>]]
	PbCl<sub>2</sub> occurs naturally in the form of the mineral ]. It is colorless, white, yellow, or green with a density of 5.3–5.8 g/cm<sup>3</sup>. The hardness on the ] is 1.5–2. The crystal structure is orthorhombic dipyramidal and the point group is 2/m 2/m 2/m. Each Pb has a coordination number of 9. The composition is 74.50% Pb and 25.50% Cl. Cotunnite occurs near volcanoes: ], Italy; Tarapacá, Chile; and ], Russia.<ref></ref><!--
	It would be helpful if a geologist looked at that page because the terms are foreign to me--><!--
	also, conflicting data w/ the following page (i.e.: hardness): http://rruff.geo.arizona.edu/doclib/hom/cotunnite.pdf-->
		⚫	PbCl<sub>2</sub> is ] in water, ] ''K''<sub>sp</sub> = {{val|1.7e-5}} at 20&nbsp;°C. It is one of only 5 commonly water-insoluble chlorides, the other 4 being ], ] (AgCl) with ''K''<sub>sp</sub> = {{val|1.8e-10}}, ] (CuCl) with ''K''<sub>sp</sub> = {{val|1.72e-7}} and ] (Hg<sub>2</sub>Cl<sub>2</sub>) with ''K''<sub>sp</sub> = {{val|1.3e-18}}.<ref>''CRC Handbook of Chemistry and Physics'', 79th Edition, David R. Lide (Ed), p. 8-108</ref><ref>Brown, Lemay, Burnsten. ''Chemistry The Central Science''. "Solubility-Product Constants for Compounds at 25&nbsp;°C". (ed 6, 1994). p. 1017</ref>
	<br clear = left/>
	==Synthesis==		==Synthesis==
⚫	Lead(II) chloride ]s from solution upon addition of ] sources (HCl, NaCl, KCl) to aqueous solutions of ](II) compounds such as ].
	:Pb(NO<sub>3</sub>)<sub>2(aq)</sub> + 2 ]<sub>(aq)</sub> → PbCl<sub>2(s)</sub> + 2 ]<sub>(aq)</sub>
	:]<sub>(aq)</sub> + ]<sub>(aq)</sub> → PbCl<sub>2(s)</sub> + 2 ]<sub>(aq)</sub>
	:basic ] + 2 HCl<sub>(aq)</sub> → PbCl<sub>2(s)</sub> + CO<sub>2(g)</sub> + H<sub>2</sub>O<ref name="chemnetbase.com">Dictionary of Inorganic and Organometallic Compounds. ''Lead(II) Chloride.'' </ref>
	:Pb(NO<sub>3</sub>)<sub>2(aq)</sub> + 2 HCl<sub>(aq)</sub> → PbCl<sub>2(s)</sub> + 2 HNO<sub>3(aq)</sub>
		⚫	Solid lead(II) chloride ]s upon addition of aqueous ] sources (HCl, NaCl, KCl) to aqueous solutions of ](II) compounds, such as ] and ]:
	Treatment of lead dioxide with hydrochloric acid gives lead(II) chloride as well as chlorine gas:
	:](s)</sub> + 4 HCl → PbCl<sub>2(s)</sub> + ] + 2 H<sub>2</sub>O		:{{chem2|Pb(NO3)2 + 2 HCl → PbCl2(s) + 2 HNO3}}
			It also forms by treatment of basic lead(II) compounds such as ] and ].
			] is reduced by chloride as follows:
	Treatment of lead oxide with hydrochloric acid gives lead(II) chloride as well as water
	:](s)</sub> + 2 HCl → PbCl<sub>2(s)</sub> + H<sub>2</sub>O		:{{chem2|PbO2 + 4 HCl → PbCl2(s) + Cl2 + 2 H2O}}
	PbCl<sub>2(s)</sub> also forms by the action of ] gas on lead metal:		It also formed by the oxidation of lead metal by ]:
	:] + Cl<sub>2</sub> → PbCl<sub>2</sub>		:{{chem2|Pb + CuCl2 → PbCl2 + Cu}}
			Or most straightforwardly by the action of ] gas on lead metal:
			:{{chem2|Pb + Cl2 → PbCl2}}
	==Reactions==		==Reactions==
	Addition of chloride ions to a suspension of PbCl<sub>2</sub> gives rise to soluble ] ions. In these reactions the additional chloride (or other ]s) break up the chloride bridges that comprise the polymeric framework of solid PbCl<sub>2(s)</sub>.		Addition of chloride ions to a suspension of PbCl<sub>2</sub> gives rise to soluble ] ions. In these reactions the additional chloride (or other ]s) break up the chloride bridges that comprise the polymeric framework of solid PbCl<sub>2(s)</sub>.
	:PbCl<sub>2(s)</sub> + ] → <sup>-</sup><sub>(aq)</sub>		:PbCl<sub>2(s)</sub> + ] → <sup>−</sup><sub>(aq)</sub>
	:PbCl<sub>2(s)</sub> + 2 Cl<sup>-</sup> → <sup>2-</sup><sub>(aq)</sub>		:PbCl<sub>2(s)</sub> + 2 Cl<sup>−</sup> → <sup>2−</sup><sub>(aq)</sub>
	PbCl<sub>2</sub> reacts with molten ] to give PbO:		PbCl<sub>2</sub> reacts with molten ] to give ]:
	:PbCl<sub>2(l)</sub> + 3 NaNO<sub>2</sub> → PbO + NaNO<sub>3</sub> + 2 NO + 2 NaCl		:PbCl<sub>2(l)</sub> + 3 NaNO<sub>2</sub> → PbO + NaNO<sub>3</sub> + 2 NO + 2 NaCl
	PbCl<sub>2</sub> is used in synthesis of lead(IV) chloride (PbCl<sub>4</sub>): Cl<sub>2</sub> is bubbled through a saturated solution of PbCl<sub>2</sub> in aqueous NH<sub>4</sub>Cl forming <sub>2</sub>. The latter is reacted with cold concentrated ] (H<sub>2</sub>SO<sub>4</sub>) forming PbCl<sub>4</sub> as an oil.<ref>{{Housecroft2nd|page=365}}</ref>		PbCl<sub>2</sub> is used in synthesis of lead(IV) chloride (PbCl<sub>4</sub>): Cl<sub>2</sub> is bubbled through a saturated solution of PbCl<sub>2</sub> in aqueous NH<sub>4</sub>Cl forming <sub>2</sub>. The latter is reacted with cold concentrated ] (H<sub>2</sub>SO<sub>4</sub>) forming PbCl<sub>4</sub> as an oil.<ref>{{Housecroft2nd|page=365}}</ref>
	Lead(II) chloride is the main ] for ] derivatives of lead, such as ]s.<ref>{{cite journal|last1 = Lowack|first1 = R|doi = 10.1016/0022-328X(94)84136-5|title = Decasubstituted decaphenylmetallocenes|year = 1994|pages = 25|volume = 476|journal = ]}}</ref> The usual alkylating agents are employed, including ]s and organolithium compounds:		Lead(II) chloride is the main ] for ] derivatives of lead, such as ]s.<ref>{{cite journal|last1 = Lowack|first1 = R|doi = 10.1016/0022-328X(94)84136-5|title = Decasubstituted decaphenylmetallocenes|year = 1994|pages = 25–32|volume = 476|journal = ]|url = https://zenodo.org/record/1253944}}</ref> The usual alkylating agents are employed, including ]s and organolithium compounds:
	:2 PbCl<sub>2</sub> + 4 RLi → R<sub>4</sub>Pb + 4 LiCl + Pb		:2 PbCl<sub>2</sub> + 4 RLi → R<sub>4</sub>Pb + 4 LiCl + Pb
	:2 PbCl<sub>2</sub> + 4 RMgBr → R<sub>4</sub>Pb + Pb + 4 MgBrCl		:2 PbCl<sub>2</sub> + 4 RMgBr → R<sub>4</sub>Pb + Pb + 4 MgBrCl
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	These reactions produce derivatives that are more similar to organosilicon compounds, ''i.e.'' that Pb(II) tends to disproportionate upon alkylation.		These reactions produce derivatives that are more similar to organosilicon compounds, ''i.e.'' that Pb(II) tends to disproportionate upon alkylation.
			PbCl<sub>2</sub> can be used to produce PbO<sub>2</sub> by treating it with ] (NaClO), forming a reddish-brown precipitate of PbO<sub>2</sub>.
	==Uses==		==Uses==
	*Molten PbCl<sub>2</sub> is used in the synthesis of lead titanate (PbTiO<sub>3</sub>) and ] lead titanate ceramics by cation replacement reactions:<ref name=Ab>{{cite journal|last1 = Aboujalil|first1 = Almaz|last2 = Deloume|first2 = Jean-Pierre|last3 = Chassagneux|first3 = Fernand|last4 = Scharff|first4 = Jean-Pierre|last5 = Durand|first5 = Bernard|title = Molten salt synthesis of the lead titanate PbTiO3, investigation of the reactivity of various titanium and lead salts with molten alkali-metal nitrites|journal = Journal of Materials Chemistry|volume = 8|pages = 1601|year = 1998|doi = 10.1039/a800003d|issue = 7}}</ref>		*Molten PbCl<sub>2</sub> is used in the synthesis of ] and ] lead titanate ceramics by cation replacement reactions:<ref name=Ab>{{cite journal|last1 = Aboujalil|first1 = Almaz|last2 = Deloume|first2 = Jean-Pierre|last3 = Chassagneux|first3 = Fernand|last4 = Scharff|first4 = Jean-Pierre|last5 = Durand|first5 = Bernard|title = Molten salt synthesis of the lead titanate PbTiO<sub>3</sub>, investigation of the reactivity of various titanium and lead salts with molten alkali-metal nitrites|journal = Journal of Materials Chemistry|volume = 8|pages = 1601|year = 1998|doi = 10.1039/a800003d|issue = 7}}</ref>
	:xPbCl<sub>2(l)</sub> + BaTiO<sub>3(s)</sub> → Ba<sub>1-x</sub>Pb<sub>x</sub>TiO<sub>3</sub> + xBaCl<sub>2</sub>		*:''x''&nbsp;PbCl<sub>2(l)</sub> + BaTiO<sub>3(s)</sub> → Ba<sub>1−''x''</sub>Pb<sub>''x''</sub>TiO<sub>3</sub> + ''x''&nbsp;BaCl<sub>2</sub>
	*PbCl<sub>2</sub> is used in production of infrared transmitting glass,<ref name="chemnetbase.com"/> and ornamental glass called ]. Aurene glass has an iridescent surface formed by spraying with PbCl<sub>2</sub> and reheating under controlled conditions. ] (SnCl<sub>2</sub>) is used for the same purpose.<ref></ref>		*PbCl<sub>2</sub> is used in production of infrared transmitting glass,<ref name="chemnetbase.com">Dictionary of Inorganic and Organometallic Compounds. ''Lead(II) Chloride.''</ref> and ornamental glass called ]. Aurene glass has an iridescent surface formed by spraying with PbCl<sub>2</sub> and reheating under controlled conditions. ] (SnCl<sub>2</sub>) is used for the same purpose.<ref></ref>
	*Pb is used in HCl service even though the PbCl<sub>2</sub> formed is slightly soluble in HCl. Addition of 6–25% of ] (Sb) increases corrosion resistance.<ref>Kirk-Othmer. "Encyclopedia of Chemical Technology". (ed 4). p 913</ref>		*Pb is used in HCl service even though the PbCl<sub>2</sub> formed is slightly soluble in HCl. Addition of 6–25% of ] (Sb) increases corrosion resistance.<ref>Kirk-Othmer. ''Encyclopedia of Chemical Technology''. (ed 4). p 913</ref>
	*A basic chloride of lead, PbCl<sub>2</sub>·Pb(OH)<sub>2</sub>, is known as Pattinson's white lead and is used as pigment in white paint.<ref>Perry & Phillips. "Handbook of Inorganic Compounds". (1995). p 213</ref>		*A basic chloride of lead, PbCl<sub>2</sub>·Pb(OH)<sub>2</sub>, is known as Pattinson's ] and is used as pigment in white paint.<ref>Perry & Phillips. ''Handbook of Inorganic Compounds''. (1995). p 213</ref> ] is now banned as a health hazard in many countries by the ].
	*PbCl<sub>2</sub> is an intermediate in refining ] (Bi) ore. The ore containing Bi, Pb, and Zn is first treated with molten ] to remove traces of acidic elements such as ] and ]. This is followed by the Parkes desilverization process to remove any silver and gold present. The ore now contains Bi, Pb, and Zn. It is treated with Cl<sub>2</sub> gas at 500 °C. ZnCl<sub>2</sub> forms first and is removed. Then PbCl<sub>2</sub> forms and is removed leaving pure Bi. BiCl<sub>2</sub> would form last.<ref>Kirk-Othmer. "Encyclopedia of Chemical Technology". (ed 4). p 241</ref>		*PbCl<sub>2</sub> is an intermediate in refining ] (Bi) ore. The ore containing Bi, Pb, and Zn is first treated with molten ] to remove traces of ] and ]. This is followed by the ] to remove any silver and gold present. There are now Bi, Pb, and Zn in the ore. At 500&nbsp;°C, it receives treatment from Cl2 gas. First, ZnCl2 forms and is excreted. Pure Bi is left behind after PbCl2 forms and is eliminated. Lastly, BiCl3 would form.<ref>Kirk-Othmer. ''Encyclopedia of Chemical Technology''. (ed 4). p. 241</ref>
	==Toxicity==		==Toxicity==
	Like other lead containing compounds, exposure to PbCl<sub>2</sub> may cause ].		Like other soluble lead compounds, exposure to PbCl<sub>2</sub> may cause ].
			{{Clear}}
	==References==		==References==
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	==External links==		==External links==
	{{Commons category|Lead(II) chloride}}		{{Commons category|Lead(II) chloride}}
	*		*
	*		*
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	*		*
	{{Lead compounds}}		{{Lead compounds}}
			{{Chlorides}}
	]		]
	]		]
	]		]
	]		]
	]
	]
	]
	]
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	]