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Once you have separated the three salts in Study Question 111 into three test tubes, you now need to confirm their presence. (a) For $\mathrm{Pb}^{2+}$ ion, one way...

Question

Once you have separated the three salts in Study Question 111 into three test tubes, you now need to confirm their presence. (a) For $\mathrm{Pb}^{2+}$ ion, one way to do this is to treat a precipitate of $\mathrm{PbCl}_{2}$ with $\mathrm{K}_{2} \mathrm{CrO}_{4}$ to produce the bright yellow insoluble solid, $\mathrm{PbCrO}_{4} .$ Using $K_{\mathrm{sp}}$ values, confirm that the chloride salt should be converted to the chromate salt. (b) Suggest a method for confirming the presence of $\mathrm{A

Once you have separated the three salts in Study Question 111 into three test tubes, you now need to confirm their presence. (a) For $\mathrm{Pb}^{2+}$ ion, one way to do this is to treat a precipitate of $\mathrm{PbCl}_{2}$ with $\mathrm{K}_{2} \mathrm{CrO}_{4}$ to produce the bright yellow insoluble solid, $\mathrm{PbCrO}_{4} .$ Using $K_{\mathrm{sp}}$ values, confirm that the chloride salt should be converted to the chromate salt. (b) Suggest a method for confirming the presence of $\mathrm{Ag}^{+}$ and $\mathrm{Cu}^{2+}$ ions using complex ions.



Answers

A solution contains one or more of the following ions: Ag+, Ca2+, and Cu2+. When you add sodium chloride to the solution, no precipitate forms. When you add sodium sulfate to the solution, a white precipitate forms. You filter off the precipitate and add sodium carbonate to the remaining solution, producing another precipitate. Which ions were present in the original solution? Write net ionic equations for the formation of each of the precipitates observed.


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