Question detail
Which of the following best describes how a basic buffer resists pH change?
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. By increasing the concentration of hydroxide ions
- B. By partially dissociating to release hydroxide ions
- C. By completely dissociating to form water
- D. By reacting with strong acids only
Answer
By partially dissociating to release hydroxide ions
Explanation
Basic buffers resist pH changes by partially dissociating to release hydroxide ions, which can neutralize any added acids, thus stabilizing the pH of the solution.
Common mistake
Misunderstanding Buffer Action
Students often confuse how basic buffers resist pH change by thinking they only neutralize acids without considering the equilibrium involved.
To explain how basic buffers resist pH change, remember that they consist of a weak base and its conjugate acid. When an acid is added, the weak base reacts with the hydrogen ions, minimizing pH change. For example, in a buffer solution of ammonia (NH3) and ammonium chloride (NH4Cl), the reaction can be represented as: NH3 + H+ ⇌ NH4+. This shows how the weak base (NH3) reacts with added H+ ions, maintaining the pH.
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