Certain positive ions combine with negative ions to form either a liquid, aqueous, solid or gaseous compound. The Solubility Rules help us determine which form is created.
Experiment 5 reacts solutions B: (NH4)2C2O4 and D: CaCl2 to form a white precipitate.
The reaction of (NH4)2C2O4 and CaCl2 is a double displacement reaction:
The product is a white precipitate.
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.
Identify the precipitate formed, if any, in the experiment 5.
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