Chemistry

Chemistry

Problem

A solution initially contains Ba2+\mathrm{Ba}^{2+}, Pb2+\mathrm{Pb}^{2+}, SO42−\mathrm{SO}_4^{2-}, and Cl−\mathrm{Cl}^- ions in equal amounts. After the solution is allowed to stand, a diagram shows two distinct white precipitates: one consists of Ba2+\mathrm{Ba}^{2+} paired with SO42−\mathrm{SO}_4^{2-}, and the other consists of Pb2+\mathrm{Pb}^{2+} paired with Cl−\mathrm{Cl}^-. Both Pb2+\mathrm{Pb}^{2+} and SO42−\mathrm{SO}_4^{2-} ions are still detected in the remaining solution. Which set of net ionic equations best accounts for all precipitates formed while leaving some ions in solution? a) Ba2+(aq)+2Cl−(aq)→BaCl2(s);Pb2+(aq)+2Cl−(aq)→PbCl2(s)\mathrm{Ba}^{2+}(aq) + 2\mathrm{Cl}^-(aq) \rightarrow \mathrm{BaCl}_2(s);\quad \mathrm{Pb}^{2+}(aq) + 2\mathrm{Cl}^-(aq) \rightarrow \mathrm{PbCl}_2(s) b) Ba2+(aq)+SO42−(aq)→BaSO4(s);Pb2+(aq)+SO42−(aq)→PbSO4(s)\mathrm{Ba}^{2+}(aq) + \mathrm{SO}_4^{2-}(aq) \rightarrow \mathrm{BaSO}_4(s);\quad \mathrm{Pb}^{2+}(aq) + \mathrm{SO}_4^{2-}(aq) \rightarrow \mathrm{PbSO}_4(s) c) Ba2+(aq)+SO42−(aq)→BaSO4(s);Pb2+(aq)+2Cl−(aq)→PbCl2(s)\mathrm{Ba}^{2+}(aq) + \mathrm{SO}_4^{2-}(aq) \rightarrow \mathrm{BaSO}_4(s);\quad \mathrm{Pb}^{2+}(aq) + 2\mathrm{Cl}^-(aq) \rightarrow \mathrm{PbCl}_2(s) d) Pb2+(aq)+2Cl−(aq)→PbCl2(s);Pb2+(aq)+SO42−(aq)→PbSO4(s)\mathrm{Pb}^{2+}(aq) + 2\mathrm{Cl}^-(aq) \rightarrow \mathrm{PbCl}_2(s);\quad \mathrm{Pb}^{2+}(aq) + \mathrm{SO}_4^{2-}(aq) \rightarrow \mathrm{PbSO}_4(s)

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