When pure barium (Ba) is added to a solution of silver acetate (AgC2H3O2), a single displacement reaction occurs, leading to the formation of barium acetate (Ba(C2H3O2)2) and silver metal (Ag).

Here's the balanced chemical equation:

Ba(s) + 2AgC2H3O2(aq) → Ba(C2H3O2)2(aq) + 2Ag(s)

Here's a breakdown of what happens:

* Barium (Ba) is a highly reactive metal, more reactive than silver.

* Silver acetate (AgC2H3O2) is a soluble ionic compound, meaning it dissociates into its ions (Ag+ and C2H3O2-) in solution.

* When barium is added, it displaces the silver ions from the solution, forming barium acetate.

* This is because barium has a higher tendency to lose electrons and form positive ions (Ba2+) compared to silver.

* The reaction results in the formation of solid silver metal, which precipitates out of the solution.

Observations:

* You would observe the formation of a grayish-white precipitate (silver metal) in the solution.

* The solution may turn slightly cloudy due to the presence of barium acetate, which is also soluble but might have a slight milky appearance.

* There might be some bubbling or effervescence as the reaction proceeds, due to the release of small amounts of hydrogen gas.

Important Note: This reaction is highly exothermic and can be vigorous. It is important to carry out this reaction with caution and appropriate safety measures in place.