Question

Consider the following reactions.
$\mathrm{PbCl}_{2}+\mathrm{K}_{2}\mathrm{CrO}_{4} \rightarrow \mathrm{A}+2\mathrm{KCl}$ (Hot solution)
$\mathrm{A}+\mathrm{NaOH} \rightleftharpoons \mathrm{B}+\mathrm{Na}_{2}\mathrm{CrO}_{4}$
$\mathrm{PbSO}_{4}+4\mathrm{CH}_{3}\mathrm{COONH}_{4} \rightarrow (\mathrm{NH}_{4})_{2}\mathrm{SO}_{4}+\mathrm{X}$
In the above reactions, A, B and X are respectively.

Accepted Answer

(D) $\mathrm{PbCrO}_{4}, \mathrm{Na}_{2}\left[\mathrm{~Pb}(\mathrm{OH})_{4}\right]$ and $\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{~Pb}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{4}\right]$

Answer

(A) $\mathrm{Na}_{2}\left[\mathrm{~Pb}(\mathrm{OH})_{2}\right], \mathrm{PbCrO}_{4}$ and $\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{~Pb}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{4}\right]$

Answer

(B) $\mathrm{PbCrO}_{4}, \mathrm{Na}_{2}\left[\mathrm{~Pb}(\mathrm{OH})_{4}\right]$ and $\left[\mathrm{Pb}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}$

Answer

(C) $\mathrm{Na}_{2}\left[\mathrm{~Pb}(\mathrm{OH})_{2}\right], \mathrm{PbCrO}_{4}$ and $\left[\mathrm{Pb}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}$

JEE Main · 2026 · 21 Jan 2026 · Shift 1 · Practical and Analytical Chemistry

Solution

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