White precipitate of ${\mathrm{PbSO}}_4$ gets dissolved in :

Reaction is given as,

${\mathrm{PbSO}}_4\downarrow +\underset{(\mathrm{Hot} \mathrm{and} \mathrm{cone}.) }{{\mathrm{H}}_2{\mathrm{SO}}_4}⟶{\mathrm{Pb}}^{2+}+2{\mathrm{HSO}}_4^{-}$

White precipitate of ${\mathrm{PbSO}}_4$ gets dissolved in concentrated ${\mathrm{H}}_2{\mathrm{SO}}_4$ on heating and concentrated $\mathrm{NaOH}$.

Thus, options A and B are correct .