Question

Choose the correct statement(s) among the following

• A. $SnC{l}_2.2H_{2}O$ is a reducing agent.
• B. $Sn{O}_2$ reacts with $KOH$ to form $K_2\left[Sn(OH{)}_6\right]$.
• C. $A$ solution of $PbC{l}_2$ in $HCl$ contains $P{b}^{2+}$ and $C{l}^{-}$ions.
• D. The reaction of $P{b}_3{O}_4$ with hot dilute nitric acid to give $Pb{O}_2$ is a redox reaction.

Answer 1

Answer: (A), (B)

(A) $S{n}^{2+}$ is less stable than $S{n}^{4+}$,
therefore $SnC{l}_2\cdot 2H_{2}O$ is a Lewis acid.
(B) $Sn{O}_2$ is amphoteric, so it will dissolve in $KOH$ solution forming $K_{2}Sn{O}_3$ or $K_2\left[Sn(OH{)}_6\right]$.
$Sn{O}_2+2KOH+2H_{2}O⟶K_2\left[Sn(OH{)}_6\right]$
(C) $PbC{l}_2$ will form a complex with $HCl$
$PbC{l}_2(s)+2HCl⟶H_2\left[PbC{l}_4\right]$
So, we may assume that now this complex will dissociate as:
$H_2\left[PbC{l}_2\right]⟶2H^{+}+{\left[PbC{l}_4\right]}^{2-}$
So, considering this possibility, option (C) should be incorrect.
(D) $P{b}_3{O}_4$ reacts with conc.$HN{O}_3$ to form $Pb{O}_2$ but the reaction is not a redox reaction.
$\stackrel{(+4)}{Pb{O}_2}.\stackrel{(+2)}{2PbO}+\underset{\text{Conc.}}{4HN{O}_3}\to \stackrel{(+4)}{Pb{O}_2}\downarrow +\stackrel{(+2)}{2Pb}(N{O}_3{)}_2+6H_{2}O$
or
$P{b}_3{O}_4$
So, option (D) is incorrect.