Question detail
How can you distinguish between a strong acid and a weak acid in terms of their behavior in solution?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Acids and bases (A-level only)
Question
- A. Strong acids completely dissociate in solution, while weak acids partially dissociate.
- B. Weak acids completely dissociate in solution, while strong acids partially dissociate. (A-level cue eb7f6a0d distractor 1)
- C. Both strong and weak acids completely dissociate in solution. (A-level cue eb7f6a0d distractor 2)
- D. Both strong and weak acids partially dissociate in solution. (A-level cue eb7f6a0d distractor 3)
Answer
Strong acids completely dissociate in solution, while weak acids partially dissociate.
Explanation
The correct option is Strong acids completely dissociate in solution, while weak acids partially dissociate.. Strong acids completely dissociate in solution, while weak acids partially dissociate. is correct because it supports the objective: Distinguish acid strength from concentration.. The reasoning stays within Brønsted-Lowry acids and bases (A-level only) and avoids drifting into a similar A-Level Chemistry idea. This item is treated as conceptual revision rather than a formal calculation item because the validated answer is an explanation or option choice, not a worked numerical response.
Common mistake
Confusing Acid Strength with Concentration
Students often confuse the strength of an acid with its concentration, thinking that a more concentrated solution is always a stronger acid.
Acid strength refers to the ability of an acid to donate protons (H+ ions), while concentration refers to the amount of acid present in a given volume of solution. A strong acid completely dissociates in solution, regardless of its concentration, whereas a weak acid only partially dissociates. For example, hydrochloric acid (HCl) is a strong acid, while acetic acid (CH3COOH) is a weak acid. A concentrated solution of acetic acid may still be weaker than a dilute solution of HCl. Always assess the acid's dissociation in water to determine strength.
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