True or False All soluble ionic compounds are strong electrolyte
The correct answer and explanation is:
False.
Not all soluble ionic compounds are considered strong electrolytes. While many soluble ionic compounds do dissociate completely in water to form ions, which is a characteristic of strong electrolytes, some do not fully dissociate and are considered weak electrolytes. The key difference lies in the degree of dissociation of the compound when dissolved in water.
Explanation:
An electrolyte is a substance that, when dissolved in water, produces ions that can conduct electricity. Ionic compounds typically dissociate into their constituent ions in aqueous solutions, but the extent to which this dissociation occurs determines whether they are strong or weak electrolytes.
A strong electrolyte is one that completely dissociates into ions when dissolved in water. Examples include sodium chloride (NaCl) and potassium nitrate (KNO3). These compounds dissolve in water to form ions that are free to move and carry electrical charge.
On the other hand, a weak electrolyte only partially dissociates into ions in solution. For example, acetic acid (CH3COOH) is a weak electrolyte because it only partially dissociates into ions when dissolved in water. Similarly, some ionic compounds, like calcium carbonate (CaCO3), may dissolve slightly in water but do not dissociate fully into ions.
The distinction between strong and weak electrolytes depends on the compound’s solubility and the extent of dissociation. Soluble ionic compounds that do not completely dissociate, such as silver chloride (AgCl), are not considered strong electrolytes, despite being soluble in water.
In summary, while many soluble ionic compounds are strong electrolytes, this is not a rule that applies universally. The behavior depends on the compound’s tendency to dissociate fully in solution.