When ammonium acetate is a strong electrolyte or a weak electrolyte, it is often the object of attention in chemical research. To determine whether it is a strong electrolyte or a weak electrolyte, it should be based on its behavior in aqueous solution.

Strong electrolytes can be completely ionized in aqueous solution to generate corresponding ions, and the conductivity of ions is strong. The weak electrolyte is only partially ionized, and there are still a large number of unionized molecules in the solution.

When ammonium acetate dissolves in water, it quickly dissociates into ammonium ions ($NH_ {4 }^{+}$） and acetate ions ($CH_ {3} COO ^{-}$）。 This dissociation process is quite thorough, and the concentration of ions in the aqueous solution is high, so it has good conductivity.

Furthermore, from the perspective of chemical equilibrium, although ammonium ions and acetate ions will undergo hydrolysis reactions, the degree of hydrolysis is relatively small, which is not enough to change the fact that most of them exist in the form of ions in the aqueous solution.

In summary, ammonium acetate can be almost completely ionized in aqueous solution and should be classified as a strong electrolyte. Its ionization properties are of great significance in many chemical processes and practical applications. For example, in some chemical reaction mediums, due to its strong electrolyte properties, it can effectively promote the reaction and provide a stable ionic environment for chemical research and practice.