A solution contains one or more of the following ions: Ag+, Ca2+, and/or Cu2+. When sodium...


A solution contains one or more of the following ions: {eq}Ag^{+} {/eq}, {eq}Ca^{2+} {/eq}, and/or {eq}Cu^{2+} {/eq}. When sodium chloride is added to the solution, no precipitate forms. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered off and sodium carbonate is added to the remaining solution, producing a precipitate.

Which ions were present in the original solution? Write the net ionic equations for the formation of each of the precipitates observed.

Precipitation Reaction:

A precipitate is a solid phase substance that separates out of an aqueous solution. For a salt compound, a precipitate implies that the compound is relatively insoluble in water at the given conditions (ion concentrations, temperature, etc.). Such insoluble products can be created from an aqueous mixture of different cations and anions. Different salt compound solutions are mixed together, each of which contribute their own ions to this mixture.

Answer and Explanation: 1

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Adding NaCl introduces a source of chloride anion, which when paired with the three potential metal cations produces:

{eq}AgCl \\ CaCl_2...

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Precipitation Reactions: Predicting Precipitates and Net Ionic Equations


Chapter 10 / Lesson 9

Study precipitate reactions. Determine precipitate solubility according to solubility rules. Learn to write ionic equations by following a molecular reaction.

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