On the net ionic equation of potassium acetate and silver nitrate
There are two compounds of potassium acetate ($CH_3COOK $) and silver nitrate ($AgNO_3 $). When they meet in solution, they react chemically.

Potassium acetate is ionized in water to obtain acetate ion ($CH_3COO ^ - $) and potassium ion ($K ^ + $). The ionization equation is: $CH_3COOK\ longrightarrow CH_3COO ^ - + K ^ + $.

Silver nitrate is also ionized in water. The ionization equation of raw silver ion ($Ag ^ + $) and nitrate ion ($NO_3 ^ - $) is: $AgNO_3\ longrightarrow Ag ^ ++ NO_3 ^ - $.

When the two solutions are mixed, acetate ions ($CH_3COO ^ - $) interact with silver ions ($Ag ^ + $) to form silver acetate precipitation ($CH_3COOAg $), while potassium ions ($K ^ + $) and nitrate ions ($NO_3 ^ - $) do not participate in the chemical reaction and only exist in solution.

Therefore, the chemical equation of the reaction is: $CH_3COOK + AgNO_3\ longrightarrow CH_3COOAg? + KNO_3 $.

When it is rewritten as an ionic equation, the soluble strong electrolyte is split into ionic form, and the insoluble substance is written as the chemical formula. Then the ion equation is: $CH_3COO ^ - + K ^ ++ Ag ^ ++ NO_3 ^ -\ longrightarrow CH_3COOAg? + K ^ ++ NO_3 ^ - $.

Removing potassium ions ($K ^ + $) and nitrate ions ($NO_3 ^ - $) that did not participate in the reaction, the net ion equation is obtained: $CH_3COO ^ - + Ag ^ +\ longrightarrow CH_3COOAg? $. This net ion equation accurately describes the essence of the reaction between potassium acetate and silver nitrate, that is, the process of acetate ions combining with silver ions to form silver acetate precipitation.