Salts preparable via nitrate formation and chloride precipitation Steps:

• React PbCO3 with dilute HNO3 to form soluble Pb(NO3)2; evaporate filtrate for pure dry Pb(NO3)2.
• React Mg(OH)2 with dilute HNO3 to form soluble Mg(NO3)2; evaporate filtrate for pure dry Mg(NO3)2.
• Add NaCl(aq) (assuming chloride source) to Pb(NO3)2 solution to precipitate sparingly soluble PbCl2; filter, wash, dry for pure solid.
• Cannot form SO4^2- products purely: PbSO4 requires SO4^2- source absent; MgSO4 from mixing yields contaminated solution.

Why B is correct:

• B lists only the achievable salts: nitrates via acid reaction/evaporation, PbCl2 via double displacement/precipitation (Pb(NO3)2 + 2NaCl → PbCl2↓ + 2NaNO3).

Why the others are wrong:

• A: Includes PbSO4 and MgSO4, impossible without SO4^2- ions for pure preparation.
• C: Includes PbSO4, impossible without SO4^2- ions.
• D: Omits PbCl2, which forms as a pure dry precipitate.

Final answer: B