Question

In the redox reaction,
$ Pb_{3}O_{4}+8HCl \to 3PbCl_{2} + Cl_{2} + 4H_{2}O $

• A. three numbers of $ Pb^{2+} $ ions get oxidised to $ Pb^{4+} $ state
• B. one number $ Pb^{4+} $ ion gets reduced to $ Pb^{2+} $ and $ 2 $ numbers of $ Pb^{2+} $ ions remain unchanged in their oxidation state
• C. one number $ Pb^{2+} $ ion gets oxidised to $ Pb^{4+} $ and two number of $ Pb^{4+} $ ions remain unchanged in their oxidation states
• D. three numbers of $ Pb^{4+} $ ions get reduced to $ Pb^{2+} $ state

Answer 1

Answer: (B)

$Pb_{3}O_{4}$ is a mixture of $PbO$ and $PbO_{2}$
$Pb_{3}O_{4} \equiv 2PbO\cdot PbO_{2}+8HCl \to 3PbCl_{2}+Cl_{2}+4H_{2}O$
In the reaction, one $Pb^{4+}$ ion is reduced to $Pb^{2+}$ and two $Pb^{2+}$ ions remain unchanged