LEAD(IV) OXIDE[PbO2]

·         CAS Number 1309-60-0

·         Linear Formula PbO₂

·         Molecular Weight 239.20

·          EC Number 215-174-5

·          MDL number MFCD00011165

·          PubChem Substance ID 24874002

Lead(IV) oxide, commonly called lead dioxide or plumbic oxide or anhydrous plumbic acid is a chemical compound with the formula PbO₂.

Detailed description

 It is an oxide where lead is in an oxidation state +4. It is of an intermediate bond type, displaying both ionic (e.g. the lattice structure) and covalent (e.g. its low melting point and insolubility in water) properties. It is an odorless dark-brown crystalline powder which is nearly insoluble in water. It exists in two crystalline forms. The alpha phase has orthorhombic symmetry; it has been first synthesized in 1941 and identified in nature as a rare mineral scrutinyite in 1988. The more common, tetragonal beta phase was first identified as the mineral plattnerite around 1845 and later produced synthetically. Lead dioxide is a strong oxidizing agent which is used in the manufacture of matches, pyrotechnics, dyes and other chemicals. It also has several important applications in electrochemistry, in particular in the positive plates of lead acid batteries.

Applications

Lead dioxide is used in the production of matches, pyrotechnics, dyes and the curing of sulfide polymers. It is also used in the construction of high-voltage lightning arresters.^[6]

Lead dioxide is used as anode material in electrochemistry. Beta-PbO₂ is more attractive for this purpose than the alpha form because it has relatively low resistivity, good corrosion resistance even in low-pH medium, and a high overvoltage for the evolution of oxygen in sulfuric acid and nitric acid based electrolytes. Lead dioxide can also withstand chlorine evolution in hydrochloric acid. Lead dioxide anodes are inexpensive and were once used instead of conventional platinum and graphite electrodes for regenerating potassium dichromate. They were also applied as oxygen anodes for electroplating copper and zinc in sulfate baths. In organic synthesis, lead dioxide anodes were applied for the production of glyoxylic acid from oxalic acid in a sulfuric acid electrolyte.

The most important use of lead dioxide is as the cathode of lead acid batteries. Its utility arises from the anomalous metallic conductivity of PbO₂. The lead acid battery stores and releases energy by shifting the equilibrium (a comproportionation) between metallic lead, lead dioxide, and lead(II) salts in sulfuric acid.

Pb + PbO₂ + 2 HSO₄⁻ + 2 H⁺ → 2 PbSO₄ + 2 H₂O, E = +2.05 V

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