Answer:
(a) \[{{H}_{3}}P{{O}_{2}}(aq)+4\overset{+1}{\mathop{AgN{{O}_{3}}}}\,(aq)+2{{H}_{2}}O(l)\to
\]\[{{H}_{3}}P{{O}_{4}}(aq)+4Ag(s)+4HN{{O}_{3}}(aq)\]
\[A{{g}^{+}}\]ion is reduced to , thus \[Ag\] acts as an
oxidising agent, it oxidises \[{{H}_{3}}P{{O}_{2}}\] to \[{{H}_{3}}P{{O}_{4}}\]
(b) \[{{H}_{3}}P{{O}_{2}}(aq)+2\overset{2+}{\mathop{CuS{{O}_{4}}}}\,(aq)+2{{H}_{2}}O(l)\to
\]\[{{H}_{3}}P{{O}_{4}}(aq)+2\overset{0}{\mathop{Cu}}\,(s)+{{H}_{2}}S{{O}_{4}}(aq)\]
\[C{{u}^{2+}}\]ion is reduced to\[Cu(s)\], thus \[C{{u}^{2+}}\]
acts as oxidising agent, it oxidises \[{{H}_{3}}P{{O}_{2}}\] to \[{{H}_{3}}P{{O}_{4}}\].
(c)\[{{C}_{6}}{{H}_{5}}CHO(l)+2{{[\overset{+1}{\mathop{Ag}}\,{{(N{{H}_{3}})}_{2}}]}^{+}}(aq)+3O{{H}^{-}}(aq)\]\[\to
{{C}_{6}}{{H}_{5}}CO{{O}^{-}}+2Ag(s)+4N{{H}_{3}}(aq)+2{{H}_{2}}O(l)\]
In above reaction, \[A{{g}^{+}}\] ion is reduced to \[Ag(s)\]thus
it acts as an oxidising agent; it oxidises \[{{C}_{6}}{{H}_{5}}CHO\]to\[{{C}_{6}}{{H}_{5}}CO{{O}^{-}}(aq).\].
(d) \[{{C}_{6}}{{H}_{5}}CHO(l)+2C{{u}^{2+}}+5O{{H}^{-}}\to
\] No change.
It is not a redox reaction.
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