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Lead stearate
Names
Other names
Lead(2+) octadecanoate, lead(II) stearate, lead distearate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.012.733 Edit this at Wikidata
EC Number
  • 214-005-2
UNII
  • InChI=1S/2C18H36O2.Pb/c2*1-2-3-4-5-6-7-8-9-10-11-12-13-14-15-16-17-18(19)20;/h2*2-17H2,1H3,(H,19,20);/q;;+2/p-2
    Key: UQLDLKMNUJERMK-UHFFFAOYSA-L
  • CCCCCCCCCCCCCCCCCC(=O)[O-].CCCCCCCCCCCCCCCCCC(=O)[O-].[Pb+2]
Properties
C
36H
70PbO
4
Molar mass 774.14
Appearance White powder
Density 1.4 g/cm3
Melting point 115.7 °C (240.3 °F; 388.8 K)
Boiling point 359.4 °C (678.9 °F; 632.5 K)
Slightly soluble
Hazards
GHS labelling:
GHS07: Exclamation markGHS08: Health hazardGHS09: Environmental hazard
Danger
H302, H332, H360, H373
P260, P281, P304, P340, P405, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Lead stearate is a metal-organic compound, a salt of lead and stearic acid with the chemical formula C
36H
70PbO
4.[1] The compound is classified as a metallic soap, i.e. a metal derivative of a fatty acid.[2] The compound is toxic.

Synthesis

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The compound can be prepared by reacting stearic acid, lead(II) oxide, and a catalyst acetic acid.[3]

Also, an exchange reaction between lead(II) acetate and sodium stearate:

Physical properties

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White powder with a slight fatty odor. Sinks in water.[4] Hygroscopic in air.

Slightly soluble in water.[1] Soluble in hot ethanol.

Uses

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The compound is used as a drier in oil paints and varnishes to speed the polymerization and oxidation processes. Also used as a lubricant and stabilizer in vinyl polymers and as a corrosion inhibitor in petroleum products.[5][6][7]

References

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  1. ^ a b "Lead Stearate". American Elements. Retrieved 7 March 2023.
  2. ^ "T3DB: Lead stearate". t3db.ca. Retrieved 7 March 2023.
  3. ^ "Preparation process of lead stearate based on melting method". 18 December 2013. Retrieved 7 March 2023.
  4. ^ "LEAD STEARATE | CAMEO Chemicals | NOAA". cameochemicals.noaa.gov. Retrieved 7 March 2023.
  5. ^ "Lead Stearate » Waldies Co. Ltd". Waldies Co. Ltd. Retrieved 7 March 2023.
  6. ^ Encyclopedia of Chemical Technology: Fuel resources to heat stabilizers. Wiley. 1991. p. 1074. ISBN 978-0-471-52669-8. Retrieved 7 March 2023.
  7. ^ Titow, M. V. (6 December 2012). PVC Technology. Springer Science & Business Media. p. 269. ISBN 978-94-009-5614-8. Retrieved 7 March 2023.

📚 Artikel Terkait di Wikipedia

Stearic acid

Potassium stearate Calcium stearate Cobaltous stearate Lithium stearate Magnesium stearate Mercuric stearate Sodium stearate Zinc stearate Esters Estradiol

Pyrotechnic composition

potassium dichromate, copper chromite, lead salicylate, lead stearate, lead 2-ethylhexoate, copper salicylate, copper stearate, lithium fluoride, n-butyl ferrocene

Edison Records

lost forever. In late 1888, metallic soaps were tried. At first, a lead stearate was used, but in the summer months, these records started to sweat and

Polymer stabilizer

as lead stearate, organotins and cadmium complexes being highly toxic. Safer modern alternatives include metallic soaps such as calcium stearate, as

Soap

lubricating greases and thickeners. A commercially important example is lithium stearate. Greases are usually emulsions of calcium soap or lithium soap and mineral

Polyvinyl chloride

traditionally, derivatives of heavy metals (lead, cadmium). Metallic soaps (metal "salts" of fatty acids such as calcium stearate) are common in flexible PVC applications

Saponification

In one simplified version, the saponification of stearin gives sodium stearate. C3H5(O2C(CH2)16CH3)3 + 3 NaOH → C3H5(OH)3 + 3 NaO2C(CH2)16CH3 This process

Naphthenic acid

much more so than single isomer carboxylates such as metal acetates and stearates. Their industrial applications exploits this property, where they are