When a strong electrolyte such as NaCl dissolves in water, does the number of ions in solution increase compared to dissolving a weak electrolyte like acetic acid (CH3COOH)?

• A. Yes, but only if the solution is saturated.
• B. Yes, because strong electrolytes dissociate completely into ions.
• C. No, because both strong and weak electrolytes produce the same number of ions.
• D. No, because weak electrolytes dissociate more than strong electrolytes.

Answer: (B)

Verified step by step guidance

1. Understand the difference between strong and weak electrolytes: Strong electrolytes dissociate completely into ions in solution, while weak electrolytes only partially dissociate.
2. Recognize that when a strong electrolyte like NaCl dissolves, it separates fully into its constituent ions, Na\textsuperscript{+} and Cl\textsuperscript{-}, increasing the total number of ions in solution.
3. For a weak electrolyte such as acetic acid (CH\textsubscript{3}COOH), only a small fraction of molecules ionize into CH\textsubscript{3}COO\textsuperscript{-} and H\textsuperscript{+}, so fewer ions are present compared to a strong electrolyte at the same concentration.
4. Note that saturation refers to the maximum amount of solute dissolved, but the degree of ionization depends on the nature of the electrolyte, not saturation level.
5. Conclude that the number of ions in solution is greater for strong electrolytes than for weak electrolytes at the same concentration because strong electrolytes dissociate completely.