Lead(II) nitrate

Lead(II) nitrate is an inorganic compound with the chemical formula Pb(NO3)2. It commonly occurs as a colourless crystal or white powder and, unlike most other lead(II) salts, is soluble in water.

Lead(II) nitrate
IUPAC name
Lead(II) nitrate
Other names
Lead nitrate
Plumbous nitrate
Lead dinitrate
3D model (JSmol)
ECHA InfoCard 100.030.210
RTECS number
  • OG2100000
UN number 1469
Molar mass 331.2 g/mol[1]
Appearance Colourless
Density 4.53 g/cm3 (20 °C)[1]
Melting point 470 °C (878 °F; 743 K)[1] decomposes
See data page
74.0·10−6 cm3/mol[2]
Face-centred cubic, cP36
Pa3, No. 205[4]
a = 0.78586 nm[4]
0.4853 nm3
Safety data sheet See: data page
ICSC 1000
Lethal dose or concentration (LD, LC):
500 mg/kg (guinea pig, oral)[5]
Supplementary data page
Refractive index (n),
Dielectric constantr), etc.
Phase behaviour
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Known since the Middle Ages by the name plumb dulcis (from Latin: 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 19th 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the main use was as a raw material in the production of pigments for lead paints, but such paints have been superseded by less toxic paints based on titanium dioxide.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 include heat stabilisation 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.


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.[6] 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. It was 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.[7] Although originally not understood during the following centuries, the decrepitation property of lead(II) nitrate led to its use in matches and special explosives.[8]

In the 19th century lead(II) nitrate began to be produced commercially. The production process is chemically straightforward: metallic lead is dissolved in nitric acid. The compound is obtained by crystallization from concentrated solution. The main use was as a white pigment in paint, but the use of lead paint has been superseded by the use of less toxic paints that use titanium dioxide as the white pigment.

Preparation and properties

Lead(II) nitrate can be obtained by reaction of lead(II) oxide with nitric acid[9]

PbO + 2 HNO3 → Pb(NO3)2 + H2O

When concentrated nitric acid is used, crystals of lead nitrate are obtained as the common ion effect reduces the solubility of lead nitrate in this medium.[10]

The compound crystallizes in the face-centred cubic system, space group Pa3Z=4 (Bravais lattice notation), with unit cell length 784 pm.[11] There is no evidence for free internal rotation of the nitrate groups within the crystal lattice at elevated temperatures.

In nitric acid treatment of lead-containing wastes, e.g., in the processing of lead–bismuth wastes from lead refineries, impure solutions of lead(II) nitrate are formed as by-product. These solutions are reported to be used in the gold cyanidation process.[12]

When concentrated sodium hydroxide solution is added to a nitrate solution, basic nitrates may be formed. Up through the half equivalence point, Pb(NO3)2·Pb(OH)2 predominates, then after this point Pb(NO3)2·5Pb(OH)2 is formed. Simple Pb(OH)2 is not formed up to at least pH 12.[13][14]

Lead(II) has a standard reduction potential (E0) of −0.125 V and the nitrate ion has an E0 of +0.956 V.[15] These properties show that lead(II) nitrate can behave as an oxidizing agent only towards easily oxidized substrates.

When heated, lead(II) nitrate crystals decompose to lead(II) oxide, oxygen and nitrogen dioxide.

2 Pb(NO3)2 (s) → 2 PbO (s) + 4 NO2 (g) + O2 (g)

Because of this property, lead nitrate is sometimes used in fireworks.[8]


Lead nitrate has been used to make complexes involving lead(II) because of its relatively high solubility, compared to other lead salts, in various solvents. For example, combining lead nitrate and pentaethylene glycol (EO5) in a solution of acetonitrile and methanol followed by slow evaporation produces the complex [Pb(NO3)2(EO5)].[16] In the crystal structure for this compound, the EO5 chain is wrapped around the lead ion in an equatorial plane. The two nitrate ligands are both bidentate; one is situated above the plane and the other below. The total coordination number is 10. Reaction of the tripodal ligand 2,4,6-tris[4-(imidazol-1-ylmethyl)phenyl]-1,3,5-triazine (timpt) with lead(II) nitrate produced a polycatenated structure in which the lead atom has a stereochemically active lone pair of electrons.[17] The nitrate ion acts as a bridging ligand in this complex.


Because of the toxicity of lead(II) salts, the production lead paints has all but ceased. Titanium dioxide is now the preferred substance to use as a white pigment in paint.[18] Other historical applications of lead(II) nitrate, such as in matches and fireworks, have declined or ceased as well.

Current applications of lead(II) nitrate include use as a heat stabilization in nylon and polyesters, in thermographic printing paper, and in rodenticides.[9] To improve the leaching process in the gold cyanidation process, lead(II) nitrate solution is added. Although a bulk process, only limited amounts (10 to 100 milligrams lead(II) nitrate per kilogram gold) are required.[19][20] Both the cyanidation itself, as well as the use of lead compounds in the process, are deemed controversial due to the compounds' toxic nature.

On a laboratory scale, lead(II) nitrate may be used to make nitrogen dioxide. The dry compound is heated in a steel vessel, producing nitrogen dioxide gas, which dimerizes to dinitrogen tetroxide when condensed to a liquid or when it is dissolved in an organic solvent.

Pb(NO3)2 → PbO2 + 2 NO2

In organic chemistry, lead(II) nitrate has been used as an oxidant, for example as an alternative to the Sommelet reaction for oxidation of benzylic halides to aldehydes.[21] It has also found use in the preparation of isothiocyanates from dithiocarbamates.[22] Because of its toxicity it has largely fallen out of favour, but it still finds occasional use, for example as a bromide scavenger during SN1 substitution.[23]


Material Safety Data Sheets

Ingestion lead(II) in any form (including, obviously, lead nitrate) will cause lead poisoning. [24] All inorganic lead compounds are also classified as probably carcinogenic to humans (Category 2A).[25]


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