Chemistry

Chemistry

Problem

The following complete ionic equation represents mixing aqueous K2CrO4 with aqueous Pb(NO3)2: 2 K+ (aq) + CrO4^2– (aq) + Pb2+ (aq) + 2 NO3– (aq) → PbCrO4(s) + 2 K+ (aq) + 2 NO3– (aq) Which net ionic equation is both mass-balanced and charge-balanced? a) Pb2+(aq)+2 K+(aq)+CrO42−(aq)→PbCrO4(s)+2 K+(aq)\text{Pb}^{2+}(aq) + 2\,\text{K}^{+}(aq) + \text{CrO}_{4}^{2-}(aq) \rightarrow \text{PbCrO}_{4}(s) + 2\,\text{K}^{+}(aq) b) PbCrO4(s)→Pb2+(aq)+CrO42−(aq)\text{PbCrO}_{4}(s) \rightarrow \text{Pb}^{2+}(aq) + \text{CrO}_{4}^{2-}(aq) c) Pb2+(aq)+CrO42−(aq)→PbCrO4(s)\text{Pb}^{2+}(aq) + \text{CrO}_{4}^{2-}(aq) \rightarrow \text{PbCrO}_{4}(s) d) Pb2+(aq)+2 NO3−(aq)→Pb(NO3)2(aq)\text{Pb}^{2+}(aq) + 2\,\text{NO}_{3}^{-}(aq) \rightarrow \text{Pb(NO}_{3})_{2}(aq)

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