Distinguish between a strong base and a weak base with one example each.

Distinguish between a strong base and a weak base with one example each.

• A. A weak base fully dissociates in water (e.g., NH2OH).
• B. A weak base partially dissociates in water (e.g., NH3).
• C. A strong base partially dissociates in water (e.g., NaOH).
• D. A strong base fully dissociates in water (e.g., NaOH).

Answer: (D)

The main idea is how bases behave in water: strong bases dissociate completely to form hydroxide ions, while weak bases only partially dissociate and rely on an equilibrium to produce OH−. The best statement is that a strong base fully dissociates in water, with NaOH as the example. This captures the defining trait of a strong base—complete ionization in solution—which is why NaOH yields a high concentration of OH− ions directly. For context, ammonia is a classic weak base: it reacts with water in an equilibrium to form NH4+ and OH−, but only a small fraction of ammonia molecules ionize, so the OH− concentration is much lower. The other options misstate the dissociation behavior, reinforcing why the fully dissociating base is the correct description of a strong base.

The main idea is how bases behave in water: strong bases dissociate completely to form hydroxide ions, while weak bases only partially dissociate and rely on an equilibrium to produce OH−.

The best statement is that a strong base fully dissociates in water, with NaOH as the example. This captures the defining trait of a strong base—complete ionization in solution—which is why NaOH yields a high concentration of OH− ions directly.

For context, ammonia is a classic weak base: it reacts with water in an equilibrium to form NH4+ and OH−, but only a small fraction of ammonia molecules ionize, so the OH− concentration is much lower.

The other options misstate the dissociation behavior, reinforcing why the fully dissociating base is the correct description of a strong base.