View source for Lead(II) nitrate

{{Chembox
| Name           = 
| ImageFile      = Lead(II) nitrate 1.jpg
| ImageFileL2 = Lead(II)-nitrate-unit-cell-3D-balls.png
| ImageFileR2 = Lead(II)-nitrate-xtal-3D-SF.png
| OtherNames     = 
| IUPACName      = 
| SystematicName = 
| Section1       = {{Chembox Identifiers
| CASNo = 10099-74-8
| CASNo_Ref = {{Cascite|changed|CAS}}
| EC_number = 233-245-9
| ChemSpiderID = 23300
| PubChem = 24924
| RTECS = OG2100000
| UNNumber = 1469
| UNII = 6E5P1699FI
| StdInChI=1S/2NO3.Pb/c2*2-1(3)4;/q2*-1;+2
| StdInChIKey = RLJMLMKIBZAXJO-UHFFFAOYSA-N
| SMILES = [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Pb+2]
 }}
| Section2       = {{Chembox Properties
| Formula = Pb(NO<sub>3</sub>)<sub>2</sub>
| MolarMass = 331.2 g/mol
| Appearance = colorless or white
| Density = 4.53 g/cm<sup>3</sup>
| MeltingPtC = 470
| MeltingPt_notes = decomposes
| MeltingPt_ref = <ref name="patnaik">{{Cite book |last=Patnaik |first=Pradyot |url=https://www.worldcat.org/oclc/50252041 |title=Handbook of inorganic chemicals |date=2003 |publisher=McGraw-Hill |isbn=0-07-049439-8 |location=New York |pages=475 |oclc=50252041}}</ref>
| Solubility = 376.5 g/L (0 °C) <br> 597 g/L (25°C) <br> 1270 g/L (100°C)
| MagSus = −74·10<sup>−6</sup>&nbsp;cm<sup>3</sup>/mol<ref name="CRC97">{{Cite book |url=https://www.worldcat.org/oclc/930681942 |title=CRC handbook of chemistry and physics : a ready-reference book of chemical and physical data. |date=2016 |others=William M. Haynes, David R. Lide, Thomas J. Bruno |isbn=978-1-4987-5428-6 |edition=2016-2017, 97th |location=Boca Raton, Florida |oclc=930681942}}</ref>
| RefractIndex = 1.782<ref name="patnaik"/>
  }}
| Section3       = 
| Section4 = {{Chembox Thermochemistry
| DeltaHform = −451.9&nbsp;kJ·mol<sup>−1</sup><ref name="CRC97"/>
 }}
| Section5       = 
| Section6       = 
| Section7       = {{Chembox Hazards
| ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics1000.htm ICSC 1000]

| GHS_ref=<ref>{{cite web |title=Lead nitrate |url=https://pubchem.ncbi.nlm.nih.gov/compound/Lead-nitrate#section=GHS-Classification |website=pubchem.ncbi.nlm.nih.gov |access-date=19 December 2021 |language=en}}</ref>
| GHSPictograms = {{GHS05}}{{GHS07}}{{GHS08}}{{GHS09}}
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|302|317|318|332|360|373|410}}
| PPhrases = {{P-phrases|201|202|210|220|221|260|261|264|270|271|272|273|280|281|301+312|302+352|304+312|304+340|305+351+338|308+313|310|312|314|321|330|333+313|363|370+378|391|405|501}}
| NFPA-H = 3
| NFPA-F = 0
| NFPA-R = 1
| NFPA-S = OX
| LDLo = 500 mg/kg (guinea pig, oral)<ref name=IDLH>{{IDLH|7439921|Lead compounds (as Pb)}}</ref>
}}
}}

'''Lead(II) nitrate''' is an [[inorganic compound]] with the [[chemical formula]] [[lead|Pb]]([[Nitrate|NO<sub>3</sub>]])<sub>2</sub>. It commonly occurs as a colourless [[crystal]] or white powder and, unlike most other lead(II) [[salt (chemistry)|salts]], is [[solubility|soluble]] in [[water (molecule)|water]].

Known since the [[Middle Ages]] by the name '''plumbum dulce''', the production of lead(II) nitrate from either metallic [[lead]] or [[lead(II) oxide|lead oxide]] in [[nitric acid]] was small-scale, for direct use in making other [[Inorganic compounds by element#Lead (Plumbum)|lead compounds]]. In the nineteenth century lead(II) nitrate began to be produced commercially in Europe and the United States. Historically, the main use was as a raw material in the production of [[pigment]]s for [[lead paint]]s, but such paints have been superseded by less toxic paints based on [[titanium dioxide]]. Other industrial uses included heat [[stabilizer (chemistry)|stabilization]] in [[nylon]] and [[polyester]]s, and in coatings of [[thermography|photothermographic]] paper. Since around the year 2000, lead(II) nitrate has begun to be used in [[gold cyanidation]].

Lead(II) nitrate is [[lead poisoning|toxic]] and must be handled with care to prevent inhalation, ingestion and skin contact. Due to its [[Hazard|hazardous nature]], the limited applications of lead(II) nitrate are under constant scrutiny.

== History ==

Lead nitrate was first identified in 1597 by the [[alchemy|alchemist]] [[Andreas Libavius]], who called the substance ''plumbum dulce'', meaning "sweet lead", because of its taste.<ref name="libavius">{{cite book|first = Andreas|last = Libavius|author-link = Andreas Libavius|title = Alchemia Andreæ Libavii|location = Francofurti|publisher = Iohannes Saurius|year = 1595}}</ref> It is produced commercially by  reaction of metallic  [[lead]] with concentrated [[nitric acid]] in which it is sparingly soluble.<ref name=britannica1911>{{cite EB1911 |wstitle=Lead |volume=16 |pages=314–320}}</ref><ref name=macgregor>{{cite book|first = John|last = Macgregor|title = Progress of America to year 1846|publisher = Whittaker & Co|location = London|year = 1847|isbn = 0-665-51791-2}}</ref> It has been produced as a raw material for making pigments such as [[chrome yellow]] (lead(II) chromate, PbCrO<sub>4</sub>) and [[chrome orange]] (basic lead(II) chromate, Pb<sub>2</sub>CrO<sub>5</sub>) and [[Naples yellow]]. These pigments were used for [[dyeing]] and printing [[calico (textile)|calico]] and other textiles.<ref name="pigments">{{cite book|title = A Text-book of Inorganic Chemistry|publisher = MacMillan|year = 1950|page = 838|first = James Riddick|last = Partington}}</ref> It has been used as an oxidizer in [[black powder]] and together with [[lead(II) azide|lead azide]] in special [[explosive material|explosives]].<ref name="pyrotechnica">{{cite journal|title = Lead nitrate as an oxidizer in blackpowder|journal = Pyrotechnica |volume = 4 |date = October 1978|pages=16–18|first = J. B.|last = Barkley|publisher = Pyrotechnica Publications|location = [[Post Falls, Idaho]]}}</ref>

== Production ==

Lead nitrate is produced by reaction of [[lead(II) oxide]] with concentrated nitric acid:<ref name="greenwood">{{cite book| first = Norman N.|last = Greenwood|author2=Earnshaw, A. |year = 1997|title = Chemistry of the Elements| url = https://archive.org/details/chemistryelement00earn_612| url-access = limited|edition = 2nd|pages= [https://archive.org/details/chemistryelement00earn_612/page/n409 388], 456|location = Oxford|publisher = Butterworth-Heinemann|isbn = 0-7506-3365-4}}</ref> 
: PbO + 2 HNO<sub>3</sub>(concentrated) → Pb(NO<sub>3</sub>)<sub>2</sub>↓ + H<sub>2</sub>O
  
It may also be obtained evaporation of the solution obtained by reacting [[lead|metallic lead]] with dilute [[nitric acid]].<ref name="kirkothmer">{{cite book|first = D. F.|last = Othmer|author-link = Donald Othmer|title = Kirk-Othmer Encyclopedia of Chemical Technology|edition = second completely revised|volume = 12 (Iron to Manganese)|year = 1967|publisher = [[John Wiley & Sons]]|location = New York|page = 272|isbn = 0-471-02040-0}}</ref> 
: Pb + 4 HNO<sub>3</sub> → Pb(NO<sub>3</sub>)<sub>2</sub> + 2 NO<sub>2</sub> + 2 H<sub>2</sub>O

Solutions and crystals of lead(II) nitrate are formed in the processing of lead–[[bismuth]] wastes from lead refineries.<ref name="sidech">{{cite web|title = Product catalog; other products|url = http://www.sidech.be/products.html|archive-url = https://web.archive.org/web/20070701013928/http://www.sidech.be/products.html|url-status=dead|archive-date = 2007-07-01|publisher = Sidech|location = Tilly, Belgium|access-date = 2008-01-05}}</ref>

== Structure ==
[[File:Lead(II)-nitrate-xtal-Pb-coordination-3D-bs-17.png|thumb|left|200px|[[Coordination sphere]] of the Pb<sup>2+</sup> ion]]
[[Image:LeadNitrateCrystalStructure.png|250px|right|thumb|Crystal structure of Pb(NO<sub>3</sub>)<sub>2</sub> <nowiki>[111]</nowiki> plane]]
The [[crystal structure]] of solid lead(II) nitrate has been determined by [[neutron diffraction]].<ref>{{cite journal|first = W. C.|last = Hamilton|title = A neutron crystallographic study of lead nitrate|journal = [[Acta Crystallographica|Acta Crystallogr.]]|year = 1957|volume = 10|pages = 103–107|doi = 10.1107/S0365110X57000304|issue = 2|doi-access = }}</ref><ref name="nowotny">{{cite journal|title = Structure refinement of lead nitrate|first = H.|last = Nowotny|author2=G. Heger |journal = [[Acta Crystallographica Section C]]|year = 1986 |volume = 42|pages = 133–35|doi = 10.1107/S0108270186097032|issue = 2|doi-access = }}</ref> The compound [[crystallization|crystallizes]] in the cubic system with the lead atoms in a [[cubic crystal system|face-centred cubic]] system. Its [[space group]] is Pa3<sub>Z=4</sub> ([[Bravais lattice]] notation), with each side of the cube with length 784&nbsp;[[picometre]]s.

The black dots represent the lead atoms, the white dots the nitrate groups 27&nbsp;picometres above the plane of the lead atoms, and the blue dots the nitrate groups the same distance below this plane. In this configuration, every lead atom is [[chemical bond|bonded]] to twelve oxygen atoms ([[bond length]]: 281&nbsp;pm). All N–O bond lengths are identical, at 127&nbsp;picometres.<ref>{{cite journal|url=https://scripts.iucr.org/cgi-bin/paper?a25608|title=Cấu trúc của chì nitrat|journal=[[Acta Crystallographica Section C]]|date=15 February 1986|volume=42 |issue=2 |pages=133–135 |doi=10.1107/S0108270186097032 |archive-url=|archive-date=|url-status=|accessdate =15 July 2019 |last1=Nowotny |first1=H. |last2=Heger |first2=G. }}</ref>


Research interest in the crystal structure of lead(II) nitrate was partly based on the possibility of free internal rotation of the nitrate groups within the crystal lattice at elevated temperatures, but this did not materialise.<ref name="nowotny"/>

== Chemical properties and reactions==
{{Image frame 
 | caption=Solubility of lead nitrate in nitric acid at 26 °C.<ref>{{cite journal|first = L. M.|last = Ferris|title = Lead nitrate—Nitric acid—Water system|journal = Journal of Chemical & Engineering Data|year = 1959|doi = 10.1021/je60007a002|volume = 5|pages = 242|issue = 3}}</ref>
 | content = {{Graph:Chart
   | width=250| height=150
   | type=line
   | x=0,4.93,12.96,25.99,50.26,63.84,71.35
   | y=37.41,24.75,12.22,4.26,0.53,0.06,0.008
 | xAxisTitle=Nitric acid concentration /wt% | yAxisTitle=Solubility /wt%  }} 
}}

Lead nitrate decomposes on heating, a property that has been used in [[pyrotechnics]] .<ref name="pyrotechnica"/> It is soluble in water and dilute nitric acid.

[[Alkali salt|Basic nitrates]] are formed in when alkali is added to a solution. Pb<sub>2</sub>(OH)<sub>2</sub>(NO<sub>3</sub>)<sub>2</sub> is the predominant species formed at low pH. At higher pH Pb<sub>6</sub>(OH)<sub>5</sub>(NO<sub>3</sub>) is formed.<ref name="pauley">{{cite journal|title = Basic Salts of Lead Nitrate Formed in Aqueous Media|first = J. L.|last = Pauley|author2=M. K. Testerman |journal = [[Journal of the American Chemical Society]]|year = 1954|volume = 76|issue = 16|pages = 4220–4222|doi = 10.1021/ja01645a062}}</ref> The cation [Pb<sub>6</sub>O(OH)<sub>6</sub>]<sup>4+</sup> is unusual in having an oxide ion inside a cluster of 3 face-sharing PbO<sub>4</sub> tetrahedra.<ref>{{Greenwood&Earnshaw}} p. 395</ref>
There is no evidence for the formation of the hydroxide, Pb(OH)<sub>2</sub>, in aqueous solution below [[pH]] 12.

Solutions of lead nitrate can be used to form co-ordination complexes. Lead(II) is a [[HSAB theory|hard acceptor]]; it forms stronger complexes with [[nitrogen]] and [[oxygen]] electron-donating ligands. For example, combining lead nitrate and [[diethylene glycol|pentaethylene glycol]] (EO<sub>5</sub>) in a solution of [[acetonitrile]] and [[methanol]] followed by slow [[evaporation]] produced the compound [Pb(NO<sub>3</sub>)<sub>2</sub>(EO<sub>5</sub>)].<ref>{{cite journal|title = Structural Chemistry of Poly (ethylene glycol). Complexes of Lead(II) Nitrate and Lead(II) Bromide|first = Robin D.|last = Rogers|author2=Andrew H. Bond |author3=Debra M. Roden |journal = [[Inorganic Chemistry (journal)|Inorg. Chem.]]|year = 1996|issue = 24|pages = 6964–6973|doi = 10.1021/ic960587b|volume = 35|pmid=11666874}}</ref> In the crystal structure for this compound, the EO<sub>5</sub> chain is wrapped around the lead ion in an [[Celestial sphere|equatorial plane]] similar to that of a [[crown ether]]. The two bidentate nitrate [[ligand]]s are in [[Cis-trans isomerism|trans configuration]]. The total [[coordination number]] is 10, with the lead ion in a bicapped [[square antiprism]] [[molecular geometry]].

The complex formed by lead nitrate with a [[bithiazole]] bidentate N-donor ligand is binuclear. The crystal structure shows that the nitrate group forms a bridge between two lead atoms.<ref name=mahjoub>{{cite journal|title = A Dimeric Mixed-Anions Lead(II) Complex: Synthesis and Structural Characterization of [Pb<sub>2</sub>(BTZ)<sub>4</sub>(NO<sub>3</sub>)(H<sub>2</sub>O)](ClO<sub>4</sub>)<sub>3</sub> {BTZ = 4,4'-Bithiazole}|first = Ali Reza|last = Mahjoub|author2 = Ali Morsali|journal = [[Chemistry Letters]]|volume = 30|issue = 12|year = 2001|page= 1234|doi=10.1246/cl.2001.1234}}</ref> One interesting aspect of this type of complexes is the presence of a physical gap in the [[coordination sphere]]; i.e., the ligands are not placed symmetrically around the metal ion. This is potentially due to a lead [[lone pair]] of electrons, also found in lead complexes with an [[imidazole]] ligand.<ref name=wan>{{cite journal|title = 2D 4.8<sup>2</sup> Network with threefold parallel interpenetration from nanometre-sized tripodal ligand and lead(II) nitrate|author = Shuang-Yi Wan|author2 =  Jian Fan|author3 = Taka-aki Okamura|author4 = Hui-Fang Zhu|author5 = Xing-Mei Ouyang|author6 = Wei-Yin Sun|author7 = Norikazu Ueyama|name-list-style = amp|journal = [[Chemical Communications|Chem. Commun.]]|year = 2002|pages = 2520–2521|doi = 10.1039/b207568g|issue = 21}}</ref>

== Applications ==

Lead nitrate has been used as a heat stabiliser in nylon and polyesters, as a coating for [[thermography|photothermographic]] paper, and in [[rodenticide]]s.<ref name="greenwood"/>

Heating lead nitrate is convenient means of making [[nitrogen dioxide]]

:<chem>2 Pb(NO_3)_2->[\Delta]2PbO + 4NO_2 +O_2 </chem>

In the [[gold cyanidation]] process, addition of lead(II) nitrate solution improves the [[Tank leaching|leaching]] process. Only limited amounts (10 to 100&nbsp;milligrams lead nitrate per kilogram gold) are required.<ref>{{cite journal|first = Fathi|last = Habashi|title = Recent advances in gold metallurgy|year = 1998 |journal=Revisa de la Facultad de Ingeniera, Universidad Central de Venezuela|volume=13|issue=2|pages=43–54}}</ref><ref>{{cite web|url = http://www.e-goldprospecting.com/html/auxiliary_agents_in_gold_cyani.html|title = Auxiliary agents in gold cyanidation|publisher = Gold Prospecting and Gold Mining|access-date = 2008-01-05}}</ref>

In organic chemistry, it may be used in the preparation of [[isothiocyanate]]s from [[dithiocarbamate]]s.<ref name="OrgSynDains">{{OrgSynth|author =Dains, F. B.|author2 =Brewster, R. Q.|author3 =Olander, C. P. |title = Phenyl isothiocyanate|collvol = 1|collvolpages = 447|prep = cv1p0447}}</ref> Its use as a [[bromide]] scavenger during [[SN1 reaction|S<sub>N</sub>1 substitution]] has been reported.<ref name="OrgSynRapoport">
{{OrgSynth|author = Rapoport, H.|author2 = Jamison, T.|collvol = 9|collvolpages = 344|prep = cv9p0344|year = 1998|title = (S)-N-(9-Phenylfluoren-9-yl)alanine and (S)-Dimethyl-N-(9-phenylfluoren-9-yl)aspartate}}</ref>

== Safety ==
{{pp-move-indef}}
{{main|Lead poisoning}}
Lead(II) nitrate is toxic, and ingestion may lead to acute lead poisoning, as is applicable for all soluble lead compounds.<ref name="icsc">{{cite web|title = Lead nitrate, Chemical Safety Card 1000|url = http://www.inchem.org/documents/icsc/icsc/eics1000.htm |publisher = [[International Labour Organization]], International Occupational Safety and Health Information Centre|date=March 1999|access-date = 2008-01-19}}</ref> All [[Inorganic compounds by element#Lead (Plumbum)|inorganic lead compounds]] are classified by the [[International Agency for Research on Cancer]] (IARC) as [[List of IARC Group 2A carcinogens|probably carcinogenic to humans]] (Category&nbsp;2A).<ref name="IARC1">{{cite journal|publisher=[[International Agency for Research on Cancer]] |year=1987 |url=http://monographs.iarc.fr/ENG/Monographs/suppl7/suppl7.pdf |title=Inorganic and Organic Lead Compounds |journal=IARC Monographs on the Evaluation of Carcinogenic Risks to Humans |volume=Suppl. 7 |access-date=2008-01-19 |page=239 |url-status=dead |archive-url=https://web.archive.org/web/20080306134819/http://monographs.iarc.fr/ENG/Monographs/suppl7/suppl7.pdf |archive-date=2008-03-06 }}</ref> They have been linked to [[renal cell carcinoma|renal cancer]] and [[glioma]] in experimental animals and to renal cancer, [[brain tumor|brain cancer]] and [[lung cancer]] in humans, although studies of workers exposed to lead are often complicated by concurrent exposure to [[arsenic]].<ref name="IARC2">{{cite journal|publisher = [[International Agency for Research on Cancer]]|year = 2006|url = http://monographs.iarc.fr/ENG/Monographs/vol87/volume87.pdf|title = Inorganic and Organic Lead Compounds|journal = IARC Monographs on the Evaluation of Carcinogenic Risks to Humans|volume = 87|isbn = 92-832-1287-8|access-date = 2008-01-01|author = World Health Organization, International Agency for Research on Cancer|url-status=dead|archive-url = https://web.archive.org/web/20071021091930/http://monographs.iarc.fr/ENG/Monographs/vol87/volume87.pdf|archive-date = 2007-10-21}}</ref> Lead is known to substitute for [[zinc]] in a number of [[enzyme]]s, including [[porphobilinogen synthase|δ-aminolevulinic acid dehydratase]] (porphobilinogen synthase) in the [[heme|haem]] biosynthetic pathway and [[Nucleotidase|pyrimidine-5′-nucleotidase]], important for the correct metabolism of [[DNA]] and can therefore cause fetal damage.<ref name=mohammed>{{cite journal|last = Mohammed-Brahim|first = B.|author2 = Buchet, J.P. |author3=Lauwerys, R. |title = Erythrocyte pyrimidine 5'-nucleotidase activity in workers exposed to lead, mercury or cadmium|journal = Int Arch Occup Environ Health|year = 1985|volume = 55|issue = 3|pages = 247–52|pmid = 2987134|doi = 10.1007/BF00383757|s2cid = 40092031}}</ref>

== References ==
{{reflist|30em}}

== External links ==
{{Commons category|Lead(II) nitrate}}
* {{cite journal|last = Woodbury|first = William D.|title = Lead|url = http://digicoll.library.wisc.edu/cgi-bin/EcoNatRes/EcoNatRes-idx?type=article&did=ECONATRES.MINYB1982V1.WWOODBURY&isize= |journal = Mineral Yearbook Metals and Minerals|year = 1982|publisher = [[United States Bureau of Mines|Bureau of Mines]]|pages = 515–42|access-date = 2008-01-18}}
* {{cite journal|title = Lead|url = https://www.cdc.gov/niosh/npg/npgd0368.html|publisher = National Institute for Occupational Safety and Health|journal = NIOSH Pocket Guide to Chemical Hazards|date=September 2005|id = NIOSH 2005-149| access-date = 2008-01-19}}
* {{cite journal|title = Lead and Lead Compounds Fact Sheet|url = http://www.npi.gov.au/database/substance-info/profiles/50.html|journal = National Pollutant Inventory|publisher = Australian Government, Department of the Environment and Water Resources|date=July 2007| access-date = 2008-01-19| archive-url = https://web.archive.org/web/20080111154608/http://www.npi.gov.au/database/substance-info/profiles/50.html| archive-date = January 11, 2008}}
* {{cite journal|title = Lead|url = http://www.afhh.org/hhe/hhe_lead.htm|journal = A Healthy Home Environment, Health Hazards|publisher = US Alliance for healthy homes|access-date = 2008-01-19|url-status=dead|archive-url = https://web.archive.org/web/20080220005525/http://www.afhh.org/hhe/hhe_lead.htm|archive-date = 2008-02-20}}

;Material Safety Data Sheets
* [http://physchem.ox.ac.uk/MSDS/LE/lead_nitrate.html MSDS for lead nitrate, PTCL, Oxford University]
* [https://web.archive.org/web/20060328120306/http://www.sciencestuff.com/msds/C1980.html MSDS for lead nitrate, Science Stuff Inc]
* [https://web.archive.org/web/20060504233922/http://avogadro.chem.iastate.edu/MSDS/Pb(NO3)2.htm MSDS for lead nitrate, Iowa State University]

{{Lead compounds}}
{{nitrates}}
{{portal|Chemistry}}

{{DEFAULTSORT:Lead(Ii) Nitrate}}
[[Category:IARC Group 2A carcinogens]]
[[Category:Lead(II) compounds]]
[[Category:Nitrates]]
[[Category:Oxidizing agents]]