What distinguishes a strong electrolyte from a weak electrolyte?

What distinguishes a strong electrolyte from a weak electrolyte?

• A. A strong electrolyte partially dissociates in solution
• B. A weak electrolyte fully dissociates in solution
• C. A strong electrolyte dissociates completely in solution
• D. A weak electrolyte completely dissolves

Answer: (C)

A strong electrolyte is defined by its ability to fully dissociate into its constituent ions when dissolved in water. This means that a strong electrolyte, such as sodium chloride or potassium nitrate, breaks apart completely into its ions, resulting in a solution that conducts electricity very well due to the presence of a high concentration of charged particles. In contrast, weak electrolytes only partially dissociate, meaning that in solution, not all of the solute molecules break apart into ions. This results in a lower concentration of ions in the solution, which leads to a poorer ability to conduct electricity compared to strong electrolytes. Additionally, the concept of complete dissolution (as mentioned in one of the incorrect options) focuses on the solubility of a substance, rather than its dissociation into ions. Thus, while a weak electrolyte may dissolve in solution, it does not produce a significant amount of ions, which distinguishes it from a strong electrolyte.

A strong electrolyte is defined by its ability to fully dissociate into its constituent ions when dissolved in water. This means that a strong electrolyte, such as sodium chloride or potassium nitrate, breaks apart completely into its ions, resulting in a solution that conducts electricity very well due to the presence of a high concentration of charged particles.

In contrast, weak electrolytes only partially dissociate, meaning that in solution, not all of the solute molecules break apart into ions. This results in a lower concentration of ions in the solution, which leads to a poorer ability to conduct electricity compared to strong electrolytes.

Additionally, the concept of complete dissolution (as mentioned in one of the incorrect options) focuses on the solubility of a substance, rather than its dissociation into ions. Thus, while a weak electrolyte may dissolve in solution, it does not produce a significant amount of ions, which distinguishes it from a strong electrolyte.