Molecular Equation: (NH4)2C2O4(aq) + AgNO3(aq) → NH4NO3(aq) + Ag2C2O4(s)
You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts:
|Solution||Solute||Color of Solution|
When these solutions are mixed, the following observations are made:
|Experiment Number||Solutions Mixed||Result|
|1||A+B||No precipitate, yellow solution|
|2||A+C||Red precipitate forms|
|3||A+D||Yellow precipitate forms|
|4||B+C||White precipitate forms|
|5||B+D||White precipitate forms|
|6||C+D||White precipitate forms|
Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.
Write a net ionic equation for the reaction that occurs in the experiment 4.
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