Editing Lead(II) nitrate (section)

{{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.