The reaction of barium chloride (BaCl₂) with silver nitrate (AgNO₃) is a double displacement reaction that results in the formation of a white precipitate, silver chloride (AgCl), and barium nitrate (Ba(NO₃)₂), which remains dissolved in solution.

Here's the balanced chemical equation:

BaCl₂(aq) + 2AgNO₃(aq) → 2AgCl(s) + Ba(NO₃)₂(aq)

Explanation:

* Reactants:

* Barium chloride (BaCl₂) is a soluble ionic compound.

* Silver nitrate (AgNO₃) is also a soluble ionic compound.

* Products:

* Silver chloride (AgCl) is an insoluble ionic compound, hence it precipitates out of solution as a white solid.

* Barium nitrate (Ba(NO₃)₂) is a soluble ionic compound, so it remains dissolved in solution.

Key Observations:

* The formation of a white precipitate (AgCl) is a clear indication that the reaction has occurred.

* The solution becomes clearer as the silver chloride precipitates out.

Applications:

This reaction can be used for:

* Testing for chloride ions: The formation of the white precipitate is a test for the presence of chloride ions.

* Preparing silver chloride: The precipitate can be collected and used for various applications like photographic processes.

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