Weak electrolytes are compounds that only partially dissociate in water. This means that some of the compound's ions are free to move and conduct electricity, while others remain bound to the molecule. As a result, weak electrolytes have a lower conductivity than strong electrolytes, which completely dissociate in water.

The conductivity of a weak electrolyte solution depends on the concentration of the solution. At low concentrations, the conductivity is low because there are fewer ions present to conduct electricity. As the concentration increases, the conductivity also increases because there are more ions present. However, the conductivity of a weak electrolyte solution will never be as high as the conductivity of a strong electrolyte solution because some of the compound's ions will always remain bound to the molecule.

Some examples of weak electrolytes include acetic acid, ammonia, and carbonic acid.