On the Weak Electrolyte Properties of Ammonium Acetate
Ammonium acetate is a weak electrolyte among all electrolytes. Looking at what it does in solution, it is very different from a strong electrolyte. Strong electrolytes are almost completely ionized in water, and ions travel freely between solutions, making them highly conductive. However, ammonium acetate is not, but it is only partially ionized in water.

When ammonium acetate ($CH_3COONH_4 $) is placed in water, acetate ions ($CH_3COO ^ - $) and ammonium ions ($NH_4 ^ + $) have a tendency to ionize, but because acetic acid ($CH_3COOH $) and ammonia monohydrate ($NH_3\ cdot H_2O $) are both weak electrolytes, acetate ions and ammonium ions are easy to ionize with water. Hydrolysis reaction occurs when hydrogen ions ($H ^ + $) and hydroxide ions ($OH ^ - $) combine. The hydrolysis formula is as follows:
$CH_3COO ^ - + H_2O\ rightleftharpoons CH_3COOH + OH ^ - $
$NH_4 ^ ++ H_2O\ rightleftharpoons NH_3\ cdot H_2O + H ^ + $

The existence of this hydrolysis reaction makes the ionization balance of ammonium acetate affected by it, and it is difficult to completely ionization like a strong electrolyte. The molecules of ammonium acetate coexist with ions in the solution, and most of the molecules are present.

Because of its partial ionization characteristics, the conductivity of ammonium acetate solution is weaker than that of strong electrolyte solutions. Strong electrolyte solutions are easy to pass through due to high ion concentration and smooth conductive paths. Ammonium acetate solution has relatively low ion concentration, which hinders the passage of current, so its conductivity is inferior.

In summary, ammonium acetate is confirmed to be a weak electrolyte due to its partial ionization, hydrolytic equilibrium and relatively weak conductivity. This is its unique chemical property, which is of great significance for research and application in the field of chemistry.