Lead(II) acetate

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Lead(II) acetate
PbAc2 (jonowo).png
Lead(II)Acetate.jpg
Names
IUPAC name
Lead(II) acetate
Systematic IUPAC name
Lead(II) ethanoate
Other names
Plumbous acetate, Salt of Saturn, Sugar of Lead, Lead diacetate
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.005.551 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 206-104-4
MeSH lead+acetate
PubChem CID
RTECS number
  • OF8050000
UNII
  • InChI=1S/2C2H4O2.Pb/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2 X mark.svgN
    Key: GUWSLQUAAYEZAF-UHFFFAOYSA-L X mark.svgN
  • CC(=O)[O-].CC(=O)[O-].[Pb+2]
Properties
Pb(C2H3O2)2
Molar mass 325.29 g/mol (anhydrous)
379.33g/mol (trihydrate)
AppearanceWhite powder or colourless, efflorescent crystals
Odor Slightly acetic
Density 3.25 g/cm3 (20 °C, anhydrous)
2.55 g/cm3 (trihydrate)
1.69 g/cm3 (decahydrate) [1]
Melting point 280 °C (536 °F; 553 K) (anhydrous)
75 °C (167 °F; 348 K)
(trihydrate) decomposes [2] at ≥ 200 °C
22 °C (72 °F; 295 K)
(decahydrate) [1]
Boiling point Decomposes
Anhydrous:
19.8 g/100 mL (0 °C)
44.31 g/100 mL (20 °C)
69.5 g/100 mL (30 °C) [3]
218.3 g/100 mL (50 °C) [1]
Solubility Anhydrous and trihydrate are soluble in alcohol, glycerol [3]
Solubility in methanol Anhydrous: [3]
102.75 g/100 g (66.1 °C)
Trihydrate: [4]
74.75 g/100 g (15 °C)
214.95 g/100 g (66.1 °C)
Solubility in glycerol Anhydrous: [3]
20 g/100 g (15 °C)
Trihydrate: [4]
143 g/100 g (20 °C)
−89.1·10−6 cm3/mol
1.567 (trihydrate) [1]
Structure
Monoclinic (anhydrous, trihydrate)
Rhombic (decahydrate)
Thermochemistry
−960.9 kJ/mol (anhydrous) [3]
−1848.6 kJ/mol (trihydrate) [4]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Neurotoxic, probable human carcinogen
GHS labelling:
GHS-pictogram-silhouette.svg GHS-pictogram-pollu.svg [2]
Danger
H360, H373, H410 [2]
P201, P273, P308+P313, P501 [2]
NFPA 704 (fire diamond)
NFPA 704.svgHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
2
1
1
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
400 mg/kg (mice, oral) [1]
300 mg/kg (dog, oral) [5]
Related compounds
Other cations
Lead(IV) acetate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Lead(II) acetate, also known as lead acetate, lead diacetate, plumbous acetate, sugar of lead, lead sugar, salt of Saturn , or Goulard's powder, is a white crystalline chemical compound with a slightly sweet taste. Its chemical formula is usually expressed as Pb(CH3COO)2 or Pb(OAc)2, where Ac represents the acetyl group. Like many other lead compounds, it causes lead poisoning. Lead acetate is soluble in water and glycerin. With water it forms the trihydrate, Pb(OAc)2·3H2O, a colourless or white efflorescent monoclinic crystalline substance.

Contents

The substance is used as a reagent to make other lead compounds and as a fixative for some dyes. In low concentrations, it formerly served as the principal active ingredient in progressive types of hair colouring dyes. [6] Lead(II) acetate is also used as a mordant in textile printing and dyeing, and as a drier in paints and varnishes. It was historically used as a sweetener and preservative in wines and in other foods and for cosmetics.

Production

Lead(II) acetate can be made by boiling elemental lead in acetic acid and hydrogen peroxide. This method will also work with lead(II) carbonate or lead(II) oxide.

Pb + H2O2 + 2 H+ → Pb2+ + 2 H2O
Pb2+ + 2 AcO− → Pb(OAc)2

Lead(II) acetate can also be made by dissolving lead(II) oxide in acetic acid: [7]

PbO + 2 AcOH → Pb(OAc)2 + H2O

Lead(II) acetate can also be made via a single displacement reaction between copper acetate and lead metal:

Cu(OAc)2 + Pb → Cu + Pb(OAc)2

Structure

The crystal structure of anhydrous lead(II) acetate has been described as a 2D coordination polymer. In comparison, lead(II) acetate trihydrate's structure is a 1D coordination polymer. [8] In the trihydrate, the Pb2+ ion's coordination sphere consists of nine oxygen atoms belonging to three water molecules, two bidentate acetate groups and two bridging acetate groups. The coordination geometry at Pb is a monocapped square antiprism. [9] [10] The trihydrate thermally decomposes to a hemihydrate, Pb(OAc)2·1⁄2H2O, and to basic acetates such as Pb4O(OAc)6 and Pb2O(OAc)2. [8]

Comparison of anhydrous and trihydrate crystal structures
Anhydrous [8]
Pb(OAc)2		Trihydrate [9] [10]
Pb(OAc)2·3H2O
Lead
coordination
sphere		 Lead(II)-acetate-xtal-Pb-coordination-3D-bs-17.png Lead(II)-acetate-trihydrate-xtal-Pb-coordination-3D-noH-bs-17.png
Strongly bonded
aggregation		 Lead(II)-acetate-xtal-one-layer-3D-bs-17.png
2D sheet		 Lead(II)-acetate-trihydrate-xtal-chain-3D-noH-bs-17.png
1D chain
Weakly bonded
aggregation		 Lead(II)-acetate-xtal-layers-3D-bs-17.png
sheets stacked with
hydrophobic surfaces in contact		 Lead(II)-acetate-trihydrate-xtal-packing-HB-3D-noH-bs-17.png
chains linked by hydrogen bonds

Uses

Sweetener

Like other lead(II) salts, lead(II) acetate has a sweet taste, which led to its historical use as a sugar substitute in both wines and foods. [11] The ancient Romans, who had few sweeteners besides honey, would boil must (unfiltered grape juice) in lead pots to produce a reduced sugar syrup called defrutum , concentrated again into sapa . This syrup was used to sweeten wine and to sweeten and preserve fruit. It is possible that lead(II) acetate or other lead compounds leaching into the syrup might have caused lead poisoning in those who consumed it. [12] Lead acetate is no longer used in the production of sweeteners because of its recognized toxicity. Legislation prohibiting its use as a wine sweetener was ineffective until decades later when chemical methods of detecting its presence had been developed. [13]

Historical incidents

The earliest confirmed poisoning by lead acetate was that of Pope Clement II who died in October 1047. A toxicological examination of his remains conducted in the mid-20th century confirmed centuries-old rumors that he had been poisoned with lead sugar. [14] It is not clear whether he was assassinated.

In 1787 painter and biographer Albert Christoph Dies swallowed, by accident, approximately 3/4 oz (20 g) of lead acetate. His recovery from this poison was slow and incomplete. He lived with illnesses until his death in 1822. [15] [16]

Although the use of lead(II) acetate as a sweetener was already illegal at that time, composer Ludwig van Beethoven may have died of lead poisoning caused by wines adulterated with lead acetate (see also Beethoven's liver). [17] [18]

In the 1850s, Mary Seacole applied lead(II) acetate, among other remedies, against an epidemic of cholera in Panama. [19] [20]

In 1887, 38 hunting horses belonging to Captain William Hollwey Steeds were poisoned in their stables at Clonsilla House, Dublin, Ireland. At least ten of the hunters died. Captain Steeds, an "extensive commission agent", had previously supplied the horses for the Bray and Greystones Coach. It transpired that they had been fed a bran mash that had been sweetened with a toxic lead acetate. [21]

Cosmetics

Lead(II) acetate, as well as white lead, has been used in cosmetics throughout history. [22]

Until recently,[ when? ] it was still used in the USA in men's hair colouring products [23] like Grecian Formula. It was not until 2018 that the manufacturer removed lead acetate from the hair coloring product. Lead acetate has been replaced by bismuth citrate as the progressive colorant. Its use in cosmetics has been banned in Canada by Health Canada since 2005 (effective at the end of 2006) based on tests showing possible carcinogenicity and reproductive toxicity, [24] and it is also banned in the European Union. [24]

Medical uses

Lead(II) acetate solution was a commonly used folk remedy for sore nipples. [25] In modern medicine, for a time, it was used as an astringent, in the form of Goulard's extract, and it has also been used to treat poison ivy. [26]

Industrial uses

Lead(II) acetate paper is used to detect the poisonous gas hydrogen sulfide. The gas reacts with lead(II) acetate on the moistened test paper to form a grey precipitate of lead(II) sulfide.

An aqueous solution of lead(II) acetate is the byproduct of a 1:1 ratio of hydrogen peroxide and white vinegar (acetic acid) used in the cleaning and maintenance of stainless steel firearm suppressors (silencers) and compensators. The solution is agitated by the bubbling action of the hydrogen peroxide, with the main reaction being the oxidation of lead by hydrogen peroxide and subsequent dissolution of lead oxide by the acetic acid, which forms lead acetate. Because of its high toxicity, this chemical solution must be appropriately disposed by a chemical processing facility or hazardous materials centre. Alternatively, the solution may be reacted with sulfuric acid to precipitate nearly insoluble lead(II) sulfate. The solid may then be removed by mechanical filtration and is safer to dispose of than aqueous lead acetate.

Other uses

It was also used in making of slow matches during the Middle Ages. It was made by mixing a natural form of lead(II) oxide called litharge and vinegar.

Sugar of lead was a recommended agent added to linseed oil during heating to produce "boiled" linseed oil, the lead and heat acting to cause the oil to cure faster than raw linseed oil. [27]

Lead(II) acetate ("salt of Saturn") was used to synthesise acetone which was then known as "spirit of Saturn" for being made with the salt of Saturn and thought to be a lead compound in the 17th century. [28]

See also

Related Research Articles

<span class="mw-page-title-main">Acetate</span> Salt compound formed from acetic acid and a base

An acetate is a salt formed by the combination of acetic acid with a base. "Acetate" also describes the conjugate base or ion typically found in aqueous solution and written with the chemical formula C
2H
3O−
2. The neutral molecules formed by the combination of the acetate ion and a positive ion are also commonly called "acetates". The simplest of these is hydrogen acetate with corresponding salts, esters, and the polyatomic anion CH
3CO−
2, or CH
3COO−
.

<span class="mw-page-title-main">Hair coloring</span> Practice of changing the hair color

Hair coloring, or hair dyeing, is the practice of changing the color of the hair on humans' heads. The main reasons for this are cosmetic: to cover gray or white hair, to alter hair to create a specific look, to change a color to suit preference or to restore the original hair color after it has been discolored by hairdressing processes or sun bleaching.

<span class="mw-page-title-main">Sodium acetate</span> Chemical compound

Sodium acetate, CH3COONa, also abbreviated NaOAc, is the sodium salt of acetic acid. This colorless deliquescent salt has a wide range of uses.

<span class="mw-page-title-main">Lead(II,IV) oxide</span> Chemical compound

Lead(II,IV) oxide, also called red lead or minium, is the inorganic compound with the formula Pb3O4. A bright red or orange solid, it is used as pigment, in the manufacture of batteries, and rustproof primer paints. It is an example of a mixed valence compound, being composed of both Pb(II) and Pb(IV) in the ratio of two to one.

Lead(II) hydroxide, Pb(OH)2, is a hydroxide of lead, with lead in oxidation state +2.

Lead oxides are a group of inorganic compounds with formulas including lead (Pb) and oxygen (O).

<span class="mw-page-title-main">Etidronic acid</span> Chemical compound

Etidronic acid, also known as etidronate, is a non-nitrogenous bisphosphonate used as a medication, detergent, water treatment, and cosmetic.

<span class="mw-page-title-main">Mercury(II) acetate</span> Chemical compound

Mercury(II) acetate, also known as mercuric acetate is a chemical compound, the mercury(II) salt of acetic acid, with the formula Hg(O2CCH3)2. Commonly abbreviated Hg(OAc)2, this compound is employed as a reagent to generate organomercury compounds from unsaturated organic precursors. It is a white, water-soluble solid, but some samples can appear yellowish with time owing to decomposition.

<span class="mw-page-title-main">Organolead chemistry</span>

Organolead chemistry is the scientific study of the synthesis and properties of organolead compounds, which are organometallic compounds containing a chemical bond between carbon and lead. The first organolead compound was hexaethyldilead (Pb2(C2H5)6), first synthesized in 1858. Sharing the same group with carbon, lead is tetravalent.

<span class="mw-page-title-main">Lead(IV) acetate</span> Organometallic compound (Pb(C2H3O2)4)

Lead(IV) acetate or lead tetraacetate is an metalorganic compound with chemical formula Pb(C2H3O2)4. It is a colorless solid that is soluble in nonpolar, organic solvents, indicating that it is not a salt. It is degraded by moisture and is typically stored with additional acetic acid. The compound is used in organic synthesis.

<span class="mw-page-title-main">Iron(III) acetate</span> Chemical compound

Ferric acetate is the acetate salt of the coordination complex [Fe3O(OAc)6(H2O)3]+ (OAc− is CH3CO2−). Commonly the salt is known as "basic iron acetate". The formation of the red-brown complex was once used as a test for ferric ions.

<span class="mw-page-title-main">Venetian ceruse</span> Cosmetic product

Venetian ceruse or Venetian white, also known as blanc de céruse de Venise and Spirits of Saturn, was a 16th-century cosmetic used as a skin whitener. It was in great demand and considered the best available at the time, supposedly containing the best quality white lead sourced from Venice, the global merchant capital at the time. It is similar to the regular ceruse, although it was marketed as better, more exclusive and more expensive than the regular ceruse variant. The regular ceruse white pigment is a basic lead carbonate of chemical formula 2 PbCO
3·Pb(OH)
2 while the mineral cerussite is a simple carbonate of lead.

<span class="mw-page-title-main">White lead</span> Chemical compound

White lead is the basic lead carbonate 2PbCO3·Pb(OH)2. It is a complex salt, containing both carbonate and hydroxide ions. White lead occurs naturally as a mineral, in which context it is known as hydrocerussite, a hydrate of cerussite. It was formerly used as an ingredient for lead paint and a cosmetic called Venetian ceruse, because of its opacity and the satiny smooth mixture it made with dryable oils. However, it tended to cause lead poisoning, and its use has been banned in most countries.

<span class="mw-page-title-main">Acetic acid</span> Colorless and faint organic acid found in vinegar

Acetic acid, systematically named ethanoic acid, is an acidic, colourless liquid and organic compound with the chemical formula CH3COOH. Vinegar is at least 4% acetic acid by volume, making acetic acid the main component of vinegar apart from water. It has been used, as a component of vinegar, throughout history from at least the third century BC.

<span class="mw-page-title-main">Lead(II) thiocyanate</span> Chemical compound

Lead(II) thiocyanate is a compound, more precisely a salt, with the formula Pb(SCN)2. It is a white crystalline solid, but will turn yellow upon exposure to light. It is slightly soluble in water and can be converted to a basic salt (Pb(CNS)2·Pb(OH)2 when boiled. Salt crystals may form upon cooling. Lead thiocyanate can cause lead poisoning if ingested and can adversely react with many substances. It has use in small explosives, matches, and dyeing.

<span class="mw-page-title-main">Magnesium acetate</span> Chemical compound

Anhydrous magnesium acetate has the chemical formula Mg(C2H3O2)2 and in its hydrated form, magnesium acetate tetrahydrate, it has the chemical formula Mg(CH3COO)2 • 4H2O. In this compound magnesium has an oxidation state of 2+. Magnesium acetate is the magnesium salt of acetic acid. It is deliquescent and upon heating, it decomposes to form magnesium oxide. Magnesium acetate is commonly used as a source of magnesium in biological reactions.

<span class="mw-page-title-main">Lead compounds</span> Type of compound

Compounds of lead exist with lead in two main oxidation states: +2 and +4. The former is more common. Inorganic lead(IV) compounds are typically strong oxidants or exist only in highly acidic solutions.

Aluminium triacetate, formally named aluminium acetate, is a chemical compound with composition Al(CH
3CO
2)
3. Under standard conditions it appears as a white, water-soluble solid that decomposes on heating at around 200 °C. The triacetate hydrolyses to a mixture of basic hydroxide / acetate salts, and multiple species co-exist in chemical equilibrium, particularly in aqueous solutions of the acetate ion; the name aluminium acetate is commonly used for this mixed system.

2-Ethoxyethyl acetate is an organic compound with the formula CH3CH2OCH2CH2O2CCH3. It is the ester of ethoxyethanol and acetic acid. A colorless liquid, it is partially soluble in water.

Lead stearate is a metal-organic compound, a salt of lead and stearic acid with the chemical formula C
36H
70PbO
4. The compound is classified as a metallic soap, i.e. a metal derivative of a fatty acid. The compound is toxic.

References

  1. 1 2 3 4 5 Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. ISBN   0-07-049439-8.
  2. 1 2 3 4 Sigma-Aldrich Co., Lead(II) acetate trihydrate. Retrieved on 2014-06-08.
  3. 1 2 3 4 5 "Lead(II) acetate". chemister.ru.
  4. 1 2 3 "Lead(II) acetate trihydrate". chemister.ru.
  5. ↑ "Lead compounds (as Pb)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  6. ↑ "Lead Acetate in 'Progressive' Hair Dye Products". fda.gov. 7 October 2021.
  7. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 373, 388. ISBN   978-0-08-037941-8.
  8. 1 2 3 Martínez-Casado, Francisco J.; Ramos-Riesco, Miguel; Rodríguez-Cheda, José A.; Cucinotta, Fabio; Matesanz, Emilio; Miletto, Ivana; Gianotti, Enrica; Marchese, Leonardo; Matěj, Zdeněk (2016). "Unraveling the Decomposition Process of Lead(II) Acetate: Anhydrous Polymorphs, Hydrates, and Byproducts and Room Temperature Phosphorescence". Inorg. Chem. 55 (17): 8576–8585. doi:10.1021/acs.inorgchem.6b01116. PMID   27548299.
  9. 1 2 Rajaram, R. K.; Mohana Rao, J. K. (1982). "Crystal structure of lead acetate trihydrate". Z. Kristallogr. 160 (1–4): 225–233. doi:10.1524/zkri.1982.160.14.225. S2CID   201671682.
  10. 1 2 Bryant, Robert G.; Chacko, V. P.; Etter, Margaret C. (1984). "Carbon-13 CP/MAS NMR and crystallographic investigations of the structure and solid-state transformations of lead(II) acetate trihydrate". Inorg. Chem. 23 (22): 3580–3584. doi:10.1021/ic00190a029.
  11. ↑ "The Disturbingly Long History of Lead Toxicity in Winemaking." Anna Archibald, 30 July 2020. Retrieved: 22 December, 2020.
  12. ↑ "Lead Poisoning and Rome". penelope.uchicago.edu. Retrieved 5 May 2024.
  13. ↑ Stoeppler, M. (1992), Hazardous Metals in the Environment, Techniques and Instrumentation in Analytical Chemistry, vol. 12, Elsevier, p. 60, ISBN   9780080875606, From the results achieved so far it is obvious that the purity law for lead in wines in the last two centuries was frequently ignored.
  14. ↑ Specht, W. and Fischer, K. (1959). "Vergiftungsnachweis an den Resten einer 900 Jahre alten Leiche" [Evidence of poisoning in the remains of a 900-year-old corpse] (in German). Archiv für Kriminologie 124: 61–84.
  15. ↑ Wikisource-logo.svg One or more of the preceding sentences incorporates text from a publication now in the public domain :  Chisholm, Hugh, ed. (1911). "Dies, Christoph Albert". Encyclopædia Britannica . Vol. 8 (11th ed.). Cambridge University Press. p. 211.
  16. ↑ Dies, Albert Christoph (1810). Biographische Nachrichten von Joseph Haydn nach mündlichen Erzählungen desselben entworfen und herausgegeben[Biographical Accounts of Joseph Haydn, written and edited from his own spoken narratives]. Vienna: Camesinaische Buchhandlung. English translation in: Dies, Albert Christoph (1963). "Biographical Accounts of Joseph Haydn". In Gotwals, Vernon (ed.). Haydn: Two Contemporary Portraits. Translated by Gotwals, Vernon. Milwaukee: University of Wisconsin Press. ISBN   0-299-02791-0.
  17. ↑ "Beethoven und Blei: Tödliches Zusammenspiel" [Beethoven and lead: deadly interaction]. www.pharmazeutische-zeitung.de. Archived from the original on 2009-02-21. Retrieved 2009-09-12.
  18. ↑ "Beethoven litt unter Bleivergiftung" [Beethoven suffered from lead poisoning]. www.3sat.de. Archived from the original on 2009-02-21. Retrieved 2020-02-24.
  19. ↑ Mary Seacole (1990), Wonderful Adventures of Mrs. Seacole in Many Lands, Chapter IV, Oxford University Press reprint, ISBN   0-19-506672-3; (2005 Penguin 20th Century Classics reprint, ed. Sarah Salih) ISBN   0-14-043902-1
  20. ↑ Jane Robinson (2004), Mary Seacole: The Charismatic Black Nurse who became a heroine of the Crimea, p.53. Constable ISBN   1-84119-677-0
  21. ↑ Weekly Irish Times, Saturday 15 October 1887; Enniskillen Chronicle and Erne Packet, 24 October 1887, p. 3
  22. ↑ Gunn, Fenja. (1973) The Artificial Face: A History of Cosmetics. — as cited in Leisure Activities of an 18th Century Lady websites.umich.edu
  23. ↑ Lead Based Hair Products: Too Hazardous for Household Use - Results , Howard W. Mielke, PhD, Myiesha D. Taylor, Chris R. Gonzales, M. Kelley Smith, Pamela V. Daniels, and Ayanna V.Buckner. Journal of American Pharmaceutical Association (NS37, Jan/Feb 1997:85-89).
  24. 1 2 "Can West News Service: Grecian Formula in a grey zone after ban". www.canada.com. Archived from the original on 2007-08-08.
  25. ↑ The American Frugal Housewife, by Lydia M. Child www.gutenberg.org
  26. ↑ Laboratory manual in biology. Sharpe. 1911, American Book Company. p. 351
  27. ↑ Andés, Louis Edgar, and Arthur Morris. Oil colours and printers' inks a practical handbook treating of linseed oil, boiled oil, paints, artists' colours, lampblack and printers' inks, black and coloured. London: Scott, Greenwood. 1903. 41. Print.
  28. ↑ Mel Gorman, History of acetone (1600–1850), 1962
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