Question

In the redox reaction,
$P{b}_3{O}_4+8HCl\to 3PbC{l}_2+C{l}_2+4H_{2}O$

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

Answer 1

Answer: (B)

$P{b}_3{O}_4$ is a mixture of $PbO$ and $Pb{O}_2$
$P{b}_3{O}_4\equiv 2PbO\cdot Pb{O}_2+8HCl\to 3PbC{l}_2+C{l}_2+4H_{2}O$
In the reaction, one $P{b}^{4+}$ ion is reduced to $P{b}^{2+}$ and two $P{b}^{2+}$ ions remain unchanged