Question:
Which of the following cannot act as a buffer?
Which of the following cannot act as a buffer?
Show Hint
Buffers require "Weakness." Strong acids or bases like $HCl, HNO_{3},$ or $NaOH$ are never part of a buffer.
Updated On: Jul 4, 2026
- $NH_{4}OH + NH_{4}Cl$
- $CH_{3}COOH + CH_{3}COONa$
- $H_{2}CO_{3} + Na_{2}CO_{3}$
- $HCl + NaCl$
Show Solution
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The Correct Option is D
Solution and Explanation
Step 1: Concept
A buffer solution consists of a weak acid and its salt with a strong base, or a weak base and its salt with a strong acid.
Step 2: Meaning
Strong acids and strong bases do not form buffer solutions because they ionize completely and cannot resist pH changes via equilibrium.
Step 3: Analysis
$NH_{4}OH$ and $CH_{3}COOH$ are weak base/acid. $H_{2}CO_{3}$ is a weak acid. $HCl$ is a strong acid.
Step 4: Conclusion
A mixture of $HCl$ (strong acid) and $NaCl$ (its salt) cannot function as a buffer. Final Answer: (D)
A buffer solution consists of a weak acid and its salt with a strong base, or a weak base and its salt with a strong acid.
Step 2: Meaning
Strong acids and strong bases do not form buffer solutions because they ionize completely and cannot resist pH changes via equilibrium.
Step 3: Analysis
$NH_{4}OH$ and $CH_{3}COOH$ are weak base/acid. $H_{2}CO_{3}$ is a weak acid. $HCl$ is a strong acid.
Step 4: Conclusion
A mixture of $HCl$ (strong acid) and $NaCl$ (its salt) cannot function as a buffer. Final Answer: (D)
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