Answer:
\[P{{b}_{3}}{{O}_{4}}\]
is a mixture of \[PbO\] and \[Pb{{O}_{2}}\]in 2 : 1 ratio. \[PbO\]has stable oxidation
state of +2 while in \[Pb{{O}_{2}}\], its oxidation state is +4. Thus, \[Pb{{O}_{2}}\]
acts as an oxidising agent and oxidises \[HCl\]into\[C{{l}_{2}}\]. \[PbO\]on
the other hand is a basic oxide which forms a salt \[(PbC{{l}_{2}})\] with \[HCl\]
The reaction,
\[P{{b}_{3}}{{O}_{4}}+8HCl\to
3PbC{{l}_{2}}+C{{l}_{2}}+4{{H}_{2}}O\] may be
divided into two parts.
\[2PbO+4HCl\to 2PbC{{l}_{2}}+2{{H}_{2}}O\](Acid base
reaction)
\[Pb{{O}_{2}}+4HCl\to PbC{{l}_{2}}+C{{l}_{2}}+2{{H}_{2}}O\](Redox
reaction)
In the second reaction, \[\text{HN}{{\text{O}}_{\text{3}}}\]acts
as oxidising agent only once the reaction may not occur between \[Pb{{O}_{2}}\]
and \[HN{{O}_{3}}\]. \[PbO\]being a basic oxide forms salt with\[HN{{O}_{3}}\].
\[2PbO+4HN{{O}_{3}}\to 2Pb(N{{O}_{3}})+2{{H}_{2}}O\]
(\[Pb{{O}_{2}}\]remain unaffected.)
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