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 6 M 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?

Question

Chemistry

Hayden

10 December, 01:13

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 6 M 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?

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Answers (1)

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Jerome Roach · Answer 1

In the first test precipitates AgCl and PbCl2. In the second one there is SnCl4 and SnS2 that are very soluble, and there ir more SnCl4 that SnS2.

Explanation:

This problem is about the cualitity studies about ions. The acidity is a factor for this studies. The chlorides and sulfides groups are mostly solubles except Pb2+, Ag + and Hg2 + for chlorides and Sr+2, Ba+2, Pb+2 y Hg+2 for sulfides.

In the first case we have a high concentration of HCl. It means that all ions reaction with HCl. In the second one there is no reaction because in the solution we have SnCl4 that is very soluble and SnS2 is very soluble too. There is more SnCl4 because for Le Chatelier if we add more reactive the balance tends to reactive.