Why following two reaction proceed differently?
`Pb_(3)O_(4)+8HClrarr3PbCl_(2)+Cl_(2)+4H_(2)O`
and
`Pb_(3)O_(4)+4HNO_(3)rarr2Pb(NO_(3))_(2)+PbO_(2)+2H_(2)O`

Options

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 two numbers of `Pb^(2+)` ions remain unchanged in their oxidation state
C. one number `Pb^(2+)` ion gets oxidised to `Pb^(4+)` and two numbers of `Pb^(4+)` ions remain unchanged in their oxidation states
D. three numbers of `Pb^(4+)` ions get reduced to `Pb^(2+)` state.

Answer

B

Explanation

`Pb_(3)O_(4)`is a mixture of PbO and `PbO_(2)`.
`Pn_(3)O_(4)-=2PnO*PnO_(2)+8HCl rarr 3PnCl_(2)+Cl_(2)+4H_(2)O`
In the reaction one `Pn^(4+)` ion is reduced to `Pb^(2+)` and two `Pb^(2+)` ions remain unchanged.