Lead(II) acetate

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Lead(II) acetate
Skeletal formula of lead(II) acetate
Toxic lead sugar or lead(II) acetate
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 Edit this at Wikidata
EC Number
  • 206-104-4
MeSH lead+acetate
RTECS number
  • OF8050000
UNII
  • InChI=1S/2C2H4O2.Pb/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2 ☒N
    Key: GUWSLQUAAYEZAF-UHFFFAOYSA-L ☒N
  • CC(=O)[O-].CC(=O)[O-].[Pb+2]
Properties
Pb(C2H3O2)2
Molar mass 325.29 g/mol (anhydrous)
379.33g/mol (trihydrate)
Appearance White 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[4] 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)[2]
218.3 g/100 mL (50 °C)[1]
Solubility Anhydrous and trihydrate are soluble in alcohol, glycerol[2]
Solubility in methanol Anhydrous:[2]
102.75 g/100 g (66.1 °C)
Trihydrate:[3]
74.75 g/100 g (15 °C)
214.95 g/100 g (66.1 °C)
Solubility in glycerol Anhydrous:[2]
20 g/100 g (15 °C)
Trihydrate:[3]
143 g/100 g (20 °C)
−89.1·10−6 cm3/mol
1.567 (trihydrate)[1]
Structure
Monoclinic (anhydrous, trihydrate)
Rhombic (decahydrate)
Thermochemistry
Std enthalpy of
formation
(ΔfH⦵298)
 −960.9 kJ/mol (anhydrous)[2]
−1848.6 kJ/mol (trihydrate)[3]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Neurotoxic, probable human carcinogen
GHS labelling:
GHS08: Health hazard GHS09: Environmental hazard[4]
Danger
H360, H373, H410[4]
P201, P273, P308+P313, P501[4]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 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).
☒N verify (what is checkY☒N ?)

Lead(II) acetate, also known as lead acetate, lead diacetate, plumbous acetate, sugar of lead, lead sugar, salt of

crystalline
substance.

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

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
Strongly bonded
aggregation
2D sheet
1D chain
Weakly bonded
aggregation
hydrophobic
surfaces in contact
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

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, 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

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,[

California Proposition 65 warning list as a carcinogen since 1988.[25]

Medical uses

Lead(II) acetate solution was a commonly used folk remedy for sore nipples.

Goulard's extract, and it has also been used to treat poison ivy.[27]

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

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.[28]

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.[29]

See also

  • Saturn's Tree

References

  1. ^
    ISBN 0-07-049439-8
    .
  2. ^ a b c d e "Lead(II) acetate".
  3. ^ a b c "Lead(II) acetate trihydrate".
  4. ^ a b c d Sigma-Aldrich Co., Lead(II) acetate trihydrate. Retrieved on 2014-06-08.
  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. ISBN 978-0-08-037941-8
    .
  8. ^
    PMID 27548299
    .
  9. ^
    S2CID 201671682
    .
  10. ^
    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
  13. 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. ^  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. ISBN 0-299-02791-0
    .
  17. ^ "Beethoven und Blei: Tödliches Zusammenspiel". Archived from the original on 2009-02-21. Retrieved 2009-09-12.
  18. ^ "Beethoven litt unter Bleivergiftung". Archived from the original on 2009-02-21. Retrieved 2020-02-24.
  19. ISBN 0-14-043902-1
  20. 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
  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. ^ a b "Can West News Service: Grecian Formula in a grey zone after ban". Archived from the original on 2007-08-08.
  25. ^ "The Proposition 65 List". Archived (PDF) from the original on 2014-10-31. Retrieved 2014-11-01.
  26. ^ The American Frugal Housewife, by Lydia M. Child
  27. ^ Laboratory manual in biology. Sharpe. 1911, American Book Company. p. 351
  28. ^ 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.
  29. ^ Mel Gorman, History of acetone (1600-1850), 1962

External links

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