A solution contains some or all of the following ions: Sn 4+ , Ag + , and Pb 2+

Question

A solution contains some or all of the following ions: Sn4+, Ag+, and Pb2+. The solution is treated as described below:

Test 1) Addition of 6M HCl causes a precipitate to form.
Test 2) Addition of H2S and 0.2 M HCl to the liquid remaining from Test 1 produces no reaction.

What conclusions can be drawn from the results of these two tests?

Ag+ is present, and Pb2+ and Sn2+ are not present. Only Ag+ is present. Either Ag+ or Pb2+, or possibly both, are present, but Sn4+ is not present. Both Pb2+ and Sn4+ are present.

Explanation / Answer

Since both Ag+ and Pb2+ ions can readily precipitates as chlorides, the test1 indicates the presence of either Ag+ or Pb2+, or possibly both are present.

Furthur, these two can be distuinguished by adding Ammonia solution to the precipitate

PbCl2 precipitate do not change on adding ammonia while AgCl get dissolves in ammonia

But sn4+ is not present because if it is present in solution it precipitates as sulfide in acidic medium on adding H2S in the presence of dil.HCl

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