{{Chembox | Name = | ImageFile = Lead(II) nitrate 1.jpg | ImageFileL2 = Lead(II)-nitrate-unit-cell-3D-balls.png | ImageClassL2 = bg-transparent | ImageFileR2 = Lead(II)-nitrate-xtal-3D-SF.png | ImageClassR2 = bg-transparent | 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 = {{chem2|Pb(NO3)2}} | N=2 |O=6 |Pb=1 | Appearance = colorless or white | Density = {{val|4.53|u=g/cm3}} | MeltingPtC = 470 | MeltingPt_notes = decomposes | MeltingPt_ref = <ref name="patnaik">{{Cite book |last=Patnaik |first=Pradyot |title=Handbook of inorganic chemicals |date=2003 |publisher=McGraw-Hill |isbn=0-07-049439-8 |location=New York |pages=475 |oclc=50252041}}</ref> | Solubility = {{ubl |{{val|376.5|u=g/L}} ({{convert|0|C|F K}}) |{{val|597|u=g/L}} ({{convert|25|C|F K}}) |{{val|1270|u=g/L}} ({{convert|100|C|F K}}) }} | MagSus = {{val|−74|e=−6|u=cm3/mol}}<ref name="CRC96">{{CRC96}}</ref>{{page needed|date=November 2025}} | RefractIndex = 1.782<ref name="patnaik"/> }} | Section3 = | Section4 = {{Chembox Thermochemistry | DeltaHform = {{val|−451.9|u=kJ.mol−1}}<ref name="CRC96"/>{{page needed|date=November 2025}} }} | 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 = {{GHS03}}{{GHS05}}{{GHS07}}{{GHS08}}<ref name="FisherSDS"/> | GHSSignalWord = Danger | HPhrases = {{H-phrases|272|302+332|317|318|332|351|360Df|372|373|410}} | PPhrases = {{P-phrases|203|210|220|260|261|264+265|270|271|272|273|280|301+317|302+352|304+340|305+351+338|317|318|319|321|330|333+317|362+364|370+378|391|405|501}} | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 2 | NFPA-S = OX | NFPA_ref=<ref name="FisherSDS">{{cite web |title=SDS - Lead(II) nitrate |url=https://www.fishersci.com/store/msds?partNumber=L62100&productDescription=LEAD+NITRATE+CERTIF+ACS+100G&vendorId=VN00033897&countryCode=US&language=en |website=fishersci.com |publisher=ThermoFisher Scientific |access-date=5 November 2025 |date=9 February 2024}}</ref> | LD50 = {{val|93|u=mg/kg}} (rat, oral)<ref name="FisherSDS"/> | LDLo = {{val|500|u=mg/kg}} (guinea pig, oral)<ref name=IDLH>{{IDLH|7439921|Lead compounds (as Pb)}}</ref> | TLV-TWA={{val|0.05|u=mg/m3}}<ref name="FisherSDS"/> | PEL={{val|0.050|u=mg/m3}} (as lead) | REL={{val|0.050|u=mg/m3}} (TWA, 8h, as lead) | IDLH={{val|100|u=mg/m3}} | NIOSH_id=0368 }} }}
'''Lead(II) nitrate''' is an inorganic compound with the chemical formula {{chem2|Pb(NO3)2}}. It commonly occurs as a colourless crystal or white powder and, unlike most other lead(II) salts, is soluble in water.
Known since the Middle Ages by the name ''plumbum dulce'' (sweet lead), the production of lead(II) nitrate from either metallic lead or lead oxide in nitric acid was small-scale, for direct use in making other 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 pigments for lead paints, but such paints have been superseded by less toxic paints based on titanium dioxide. Other industrial uses included heat stabilization in nylon and polyesters, and in coatings of photothermographic paper. Since around the year 2000, lead(II) nitrate has begun to be used in gold cyanidation.{{cn|date=November 2025}}
Lead(II) nitrate is toxic and must be handled with care to prevent inhalation, ingestion and skin contact. Due to its hazardous nature, the limited applications of lead(II) nitrate are under constant scrutiny.
== History == Since the Middle Ages, lead(II) nitrate has been produced as a raw material for the production of coloured pigments in lead paints, such as chrome yellow (lead(II) chromate), chrome orange (lead(II) hydroxide chromate) and similar lead compounds. These pigments were used for dyeing and printing 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>
In 1597, the German alchemist Andreas Libavius first described the compound, coining the medieval names of ''plumb dulcis'' and ''calx plumb dulcis'', meaning "sweet lead", because of its taste.<ref name="libavius">{{cite book|first = Andreas|last = Libavius|authorlink = Andreas Libavius|title = Alchemia Andreæ Libavii|location = Francofurti|publisher = Iohannes Saurius|year = 1595}}</ref> Although originally not understood during the following centuries, the decrepitation property of lead(II) nitrate led to its use in matches and special explosives such as lead azide.<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>
The production process was and still is chemically straightforward, effectively dissolving lead in nitric acid and subsequently harvesting the precipitate. However, the production remained small-scale for many centuries, and the commercial production of lead(II) nitrate as raw material for the manufacture of other lead compounds was not reported until 1835.<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> In 1974, the U.S. consumption of lead compounds, excluding pigments and gasoline additives, was 642 tons.<ref name="greenwood">{{cite book| first = Norman N.|last = Greenwood|author2=Earnshaw, A. |year = 1997|title = Chemistry of the Elements|edition = 2nd|pages= 388, 456|location = Oxford|publisher = Butterworth-Heinemann|isbn = 0-7506-3365-4}}</ref>
== Production ==
Lead nitrate is produced by reaction of lead(II) oxide with concentrated nitric acid:<ref name=Greenwood>{{Greenwood&Earnshaw}}</ref>{{rp|388}} :{{chem2|PbO + 2 HNO3 -> Pb(NO3)2↓ + H2O}}
It may also be obtained by evaporation of the solution obtained by reacting 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> :{{chem2|Pb + 4 HNO3 -> Pb(NO3)2 + 2 NO2 + 2 H2O}}
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 == {{Gallery |title=Depictions of the structure of lead(II) nitrate |width=160 | height=170 |noborder=yes |align=center |footer= |File:Lead(II)-nitrate-xtal-Pb-coordination-3D-bs-17.png |Coordination sphere of the {{chem2|Pb(2+)}} ion |File:LeadNitrateCrystalStructure.png |Crystal structure of {{chem2|Pb(NO3)2}} <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 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 crystallizes in the cubic system with the lead atoms in a face-centred cubic system. Its space group is Pa3{{sub|Z{{=}}4}} (Bravais lattice notation), with each side of the cube with length {{convert|784|pm|Å}}.
The black dots represent the lead atoms, the white dots the nitrate groups {{convert|27|pm|Å}} 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 bonded to twelve oxygen atoms (bond length: {{convert|281|pm|Å}}). All {{chem2|N\sO}} bond lengths are identical, at {{convert|127|pm|Å}}.<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. |url-access=subscription }}</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== {{Chart |align=right |definition=Lead Nitrate Solubility in Nitric Acid at 26 Degrees C.chart |data=Lead Nitrate Solubility in Nitric Acid at 26 Degrees C.tab |thumb=1 |width=250 |caption=Solubility of lead nitrate in nitric acid at {{convert|26|C|F}}.<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> }}
Lead nitrate is an oxidizer and has been used as such in pyrotechnics.<ref name="pyrotechnica"/><ref name="Weingart">{{cite book |last1=Weingart |first1=George W. |title=Pyrotechnics |pages=136 |edition=2nd |url=https://archive.org/details/Pyrotechnics_by_G._Weingart_2nd_ed._Corrected/page/n149/mode/2up |access-date=5 November 2025 |date=1947}}</ref>
Basic nitrates are formed when alkali is added to a solution. {{chem2|Pb2(OH)2(NO3)2}} is the predominant species formed at low pH. At higher pH {{chem2|Pb6(OH)5NO3}} 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 {{chem2|[Pb6O(OH)6](4+) }} is unusual in having an oxide ion inside a cluster of 3 face-sharing {{chem2|PbO4}} tetrahedra.<ref name="Greenwood"/>{{rp|395}} There is no evidence for the formation of the hydroxide, {{chem2|Pb(OH)2}}, in aqueous solution below pH 12.
Solutions of lead nitrate can be used to form co-ordination complexes. Lead(II) is a hard acceptor; it forms stronger complexes with nitrogen and oxygen electron-donating ligands. For example, combining lead nitrate and pentaethylene glycol (shortened to EO5 in the referenced paper) in a solution of acetonitrile and methanol followed by slow evaporation produced the compound [{{chem2|Pb(NO3)2}}EO5].<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 = 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 EO5 chain is wrapped around the lead ion in an equatorial plane similar to that of a crown ether. The two bidentate nitrate ligands are in 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 aspect of this type of complex 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 lone pair of lead 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 = 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 photothermographic paper, and in rodenticides.<ref name="Greenwood"/>{{rp|388}}
Heating lead nitrate is convenient means of making nitrogen dioxide:
:{{chem2|2 Pb(NO3)2}}{{nbsp}}{{overset|Δ|{{chem2|→}}}}{{nbsp}}{{chem2|2 PbO + 4 NO2 + O2}}
In the gold cyanidation process, addition of lead(II) nitrate solution improves the leaching process. Only limited amounts ({{val|10|to|100|u=mg}} 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 isothiocyanates from dithiocarbamates.<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 S{{sub|N}}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 lead compounds (but not elemental lead) are classified by the International Agency for Research on Cancer (IARC) as probably carcinogenic to humans (Category 2A). They have been linked to renal cancer and glioma in experimental animals and to renal cancer, 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 enzymes, including δ-aminolevulinic acid dehydratase (porphobilinogen synthase) in the haem biosynthetic pathway and 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>
== See also == * Pigments containing lead, such as white lead, Naples yellow, and red lead
== References == {{reflist|30em}}
== External links == {{Commons category|Lead(II) nitrate}}
{{Lead compounds}} {{nitrates}} {{portal|Chemistry}}
{{DEFAULTSORT:Lead(Ii) Nitrate}} Category:IARC Group 2A carcinogens Category:Lead(II) compounds Category:Nitrates Category:Oxidizing agents