We have to write a net ionic equation for the reaction that occurs in experiment 2 and identify the precipitate formed.
A precipitate is an insoluble compound that forms when solutions of two soluble compounds are mixed.
Experiment 2 is the mixing of solutions A and C that results in the formation of a red precipitate.
Solution A: Na2CrO4
Solution C: AgNO3
When these substances react, the cations and anions will exchange. The NO3- ion will change cation from Ag+ to Na+ and CrO42- will change cation from Na+ to Ag+.
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 and identify the precipitate formed, if any, in the experiment 2.
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