Consider the following reaction scheme: D(tex | vedclass

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(C) The metallic salt $A$ reacts with $K_2CrO_4$ in the presence of acetic acid to give a yellow precipitate $B$,which indicates that $A$ contains $Ba

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barium carbonate

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(C) The metallic salt $A$ reacts with $K_2CrO_4$ in the presence of acetic acid to give a yellow precipitate $B$,which indicates that $A$ contains $Ba^{2+}$ ions. $Sr^{2+}$ and $Ca^{2+}$ do not form a precipitate with $K_2CrO_4$ in acetic acid.The reactions are as follows:$1. Ba^{2+} + K_2CrO_4 \xrightarrow{CH_3COOH} BaCrO_4 \downarrow (	ext{Yellow ppt } B)$$2. Ba^{2+} + dil. H_2SO_4 ightarrow BaSO_4 \downarrow (	ext{White ppt } C)$$3. Ba^{2+} + Na_2CO_3 ightarrow BaCO_3 \downarrow (	ext{White ppt } D)$Thus,the white precipitate $D$ is barium carbonate $(BaCO_3)$.

Consider the following reaction scheme: $D(\text{White ppt}) \xleftarrow{Na_2CO_3} A \xrightarrow[\text{in acetic acid}]{K_2CrO_4} B(\text{Yellow ppt})$ and $A \xrightarrow{dil.\ H_2SO_4} C(\text{White ppt})$. If $A$ is a metallic salt,then the white precipitate $D$ must be:

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