| IUPAC name
| Other names
|Molar mass||443.376 g/mol|
|Appearance||Colorless to slight pinkish crystals|
|Density||2.228 g/cm3 (at 17 °C)|
|Melting point||175-180 °C |
|Boiling point||Decomposes |
|Reacts with water|
|Solubility|| Reacts with alcohols|
Soluble in hot glacial acetic acid, slightly soluble in benzene, chloroform
|Safety data sheet||Sparchem|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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.
Lead tetraacetate is sold by chemical suppliers, though due to its toxicity and sensitivity to water, it's difficult to purchase. It's best to make it yourself.
There are a few ways to prepare lead(IV) acetate.
One method involves the reaction of minium with 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, and if small amounts are added in the former reaction it will remove any traces of water from the reaction.
- Pb3O4 + 6 CH3COOH → Pb(CH3COO)4 + Pb(CH3COO)2 + PbO + 3 H2O
- Pb3O4 + 3 (CH3CO)2O → Pb(CH3COO)4 + Pb(CH3COO)2 + PbO
Another process involves the oxidation of lead(II)acetate is acetic 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.
A more accessible way involves electrolysis. There are several methods described in literature.
- THF synthesis
- Aziridine synthesis
- Hoffmann type rearrangements
- Oxidation of n-alkanes to secondary acetates 
Lead(IV) acetate may be fatal if ingested or inhaled. Skin contact will cause burns and can also cause lead poisoning.
As it is sensitive to moisture and alcohols, it's best to store it in a hermetically sealed container, a desiccator or a glovebox if you have one. It is sometimes stabilized with acetic acid or acetic anhydride.
Lead tetraacetate can be reduced with a sulfide to the insoluble lead sulfide and sent to the disposal facilities.