A solution contains one or more of the following ions: Hg2+2, Ba2+, and Fe2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no precipitate. When potassium carbonate is added to the remaining solution, a precipitate forms. What are the net ionic equations for the formation of each of the precipitates observed? Express your answers as chemical equations separated by a comma. Identify all the phases in your answer.

Question

Grant Combs

Chemistry

20 June, 08:26

A solution contains one or more of the following ions: Hg2+2, Ba2+, and Fe2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no precipitate. When potassium carbonate is added to the remaining solution, a precipitate forms. What are the net ionic equations for the formation of each of the precipitates observed? Express your answers as chemical equations separated by a comma. Identify all the phases in your answer.

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Answers (1)

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Jett Wiley · Answer 1

The first one is Hg2Cl2

This leaves you with Ba2 + and Fe2+

What is odd is that the Ba2 + should precipitate with the sulfate. Since it doesn't, there is no net ionic equaiton.

Meaning the last one is the Fe2+

First net ionic equation:

Hg2 2 + (aq) + 2Cl - (aq) - - > Hg2Cl2 (s)

Last net ionic equation:

Fe2 + (aq) + CO3 2 - (aq) - - > FeCO3 (s)

If BaSO4 is formed you would do it the same as the above.