Red lead Pb3O4 reacts with hot dilute HNO3 as Pb3O4 + 4HNO3 -> 2Pb(NO3)2 + PbO2 + 2H2O. Which of the following is correct?

It is not a redox reaction; Pb3O4 behaves as 2PbO.PbO2 with the basic PbO part dissolving as Pb(II) and PbO2 left as residue

It is a redox reaction in which Pb(II) is oxidised to Pb(IV)

It is not a redox reaction; Pb3O4 behaves as 2PbO.PbO2 with the basic PbO part dissolving as Pb(II) and PbO2 left as residue

It is a disproportionation of Pb(III) to Pb(II) and Pb(IV)

PbO2 is reduced by nitric acid to Pb(II) in the residue

JEE Advanced levelSingle correct optionDifficulty 3 of 3pt187

Red lead $Pb X_{3} O X_{4}$ reacts with hot dilute $HNO X_{3}$ as $Pb X_{3} O X_{4} + 4 HNO X_{3} 2 Pb (NO X_{3}) X_{2} + PbO X_{2} + 2 H X_{2} O$ . Which of the following is correct?

AIt is a redox reaction in which Pb(II) is oxidised to Pb(IV)
BIt is not a redox reaction; $Pb X_{3} O X_{4}$ behaves as $2 PbO \cdot PbO X_{2}$ with the basic PbO part dissolving as Pb(II) and $PbO X_{2}$ left as residue
CIt is a disproportionation of Pb(III) to Pb(II) and Pb(IV)
D $PbO X_{2}$ is reduced by nitric acid to Pb(II) in the residue

Red lead is a mixed oxide containing two Pb(II) and one Pb(IV) centres. The basic PbO portion reacts with the acid to give

Pb (NO X_{3}) X_{2}

, with no change in any oxidation number, while the Pb(IV) in

PbO X_{2}

stays unchanged as the brown residue. Thus no atom changes its oxidation state and the reaction is acid-base in nature.