Difference between revisions of "Lead(IV) acetate"
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Revision as of 17:09, 20 August 2015
| Properties | |
|---|---|
| PbC8H12O8 | |
| Appearance | Colorless to slight pinkish crystals |
| Density | 2.23 (17°C) |
| Melting point | 175-180°C [1] |
| Boiling point | Decomposes 1 |
| Solubility | hot glacial acetic acid, slightly soluble in benzene, chloroform |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Lead(IV) acetate also known as lead tetraacetate or plumbic acetate is a chemical compound, a lead salt of acetic acid, with the formula Pb(CH3COO)4.
Contents
Properties
Chemical
Lead tetraacetate reacts with water and ethanol to form lead(II) acetate, lead(II) oxide and acetic acid.
Physical
Lead tetraacetate is a white to slight pinkish crystals, soluble in hot acetic acid, chloroform or benzene. It has a vinegar like odor. It melts at 175 °C, and will decompose if heated too high. It has a density of 2.228 g/cm[1].
Availability
Lead tetraacetate is sold by chemical suppliers, though due to its sensitivity to water, it's difficult to purchase. It's best to make it yourself.
Preparation
There are a few ways to prepare lead(IV) acetate.
One method involves the reaction of minium with anhydrous glacial acetic acid. This reaction produces both lead acetates as well as PbO, which can be separated via recrystallization from acetic acid. Acetic anhydride can also be used for a better yield.
Another process involves the oxidation of lead(II)acetate is acetic acid acid with chlorine. Dry chlorine gas is bubbled through the solution, which is heated to 80 °C. This reaction produces lead(II) chloride as residue.
- 2 Pb(CH3COO)2 + Cl2 -> Pb(CH3COO)4 + PbCl2
The resulting precipitate is filtered while hot and washed with hot glacial acetic acid. The filtrate is left to crystallize. Further recrystallization from glacial acetic acid is required to remove any PbCl2 impurities.[2]
A more accessible way involves electrolysis. There are several methods described in literature.
A method described in 1922 involves the electrolysis of lead(II) acetate with acetic acid.[3] One reaction involves the electrolysis of lead(IV) sulfate in acetic acid.[4]
Projects
- THF synthesis
- Aziridine synthesis
- Hoffmann type rearrangements
- Oxidation of n-alkanes to secondary acetates [5]
Handling
Safety
Lead(IV) acetate may be fatal if ingested or inhaled. Skin contact will cause burns and can also cause lead poisoning.
Storage
As it is sensitive to moisture and alcohols, it's best to store it in a hermetic sealed container or a glovebox if you have one.
Disposal
Lead tetraacetate can be reduced with a sulfide to the insoluble lead sulfide and sent to the disposal facilities.
References
- ↑ http://onlinelibrary.wiley.com/doi/10.1002/9780470132326.ch17/summary
- ↑ http://onlinelibrary.wiley.com/doi/10.1002/9780470132326.ch17/summary
- ↑ http://onlinelibrary.wiley.com/doi/10.1002/bbpc.19220282116/abstract
- ↑ http://onlinelibrary.wiley.com/doi/10.1002/bbpc.19000072205/abstract
- ↑ http://www.sciencedirect.com/science/article/pii/S0040403900943041
