A colorless aqueous solution contains nitrate | vedclass

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(A) $1$. The addition of $NaCl$ to the solution containing nitrates of $X$ and $Y$ produces white precipitates of $AgCl$ and $PbCl_2$.$2$. $PbCl_2$ is

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$Ag$ and $Pb$

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(A) $1$. The addition of $NaCl$ to the solution containing nitrates of $X$ and $Y$ produces white precipitates of $AgCl$ and $PbCl_2$.$2$. $PbCl_2$ is soluble in hot water,while $AgCl$ is not. Thus,the residue $P$ is $AgCl$ and the hot filtrate $Q$ contains $PbCl_2$.$3$. $AgCl$ (residue $P$) is soluble in aqueous $NH_3$ to form $[Ag(NH_3)_2]Cl$ and in excess sodium thiosulfate to form $Na_3[Ag(S_2O_3)_2]$.$4$. The hot solution $Q$ containing $Pb^{2+}$ ions reacts with $KI$ to form a yellow precipitate of $PbI_2$ $(Pb^{2+} + 2I^- \rightarrow PbI_2 \downarrow)$.$5$. Therefore,$X$ is $Ag$ and $Y$ is $Pb$.

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