Question:
Which from the following is NOT a buffer solution?
Which from the following is NOT a buffer solution?
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A buffer needs a weak acid with its conjugate base or a weak base with its conjugate acid; NaCl supplies neither.
Updated On: Nov 12, 2026
- \(\text{CH}_{3}\text{COOH}+\text{CH}_{3}\text{COONa}\) in water.
- \(\text{NH}_{4}\text{OH}+\text{NH}_{4}\text{Cl}\) in water.
- \(\text{HCOOH}+\text{HCOONa}\) in water.
- \(\text{CH}_{3}\text{COOH}+\text{NaCl}\) in water.
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The Correct Option is D
Solution and Explanation
Step 1: Understanding the Concept
A buffer contains a weak acid with a salt of its conjugate base, or a weak base with a salt of its conjugate acid.
Step 2: Check the options
\(\text{CH}_3\text{COOH} + \text{CH}_3\text{COONa}\) and \(\text{HCOOH} + \text{HCOONa}\) are acidic buffers. \(\text{NH}_4\text{OH} + \text{NH}_4\text{Cl}\) is a basic buffer.
Step 3: The odd one out
In \(\text{CH}_3\text{COOH} + \text{NaCl}\), NaCl comes from a strong acid and a strong base. It supplies no acetate ions, so there is no reserve to take up added acid.
Final Answer:
Acetic acid with NaCl is not a buffer solution. \[ \boxed{\text{(D) }\text{CH}_{3}\text{COOH}+\text{NaCl}\text{ in water}} \]
A buffer contains a weak acid with a salt of its conjugate base, or a weak base with a salt of its conjugate acid.
Step 2: Check the options
\(\text{CH}_3\text{COOH} + \text{CH}_3\text{COONa}\) and \(\text{HCOOH} + \text{HCOONa}\) are acidic buffers. \(\text{NH}_4\text{OH} + \text{NH}_4\text{Cl}\) is a basic buffer.
Step 3: The odd one out
In \(\text{CH}_3\text{COOH} + \text{NaCl}\), NaCl comes from a strong acid and a strong base. It supplies no acetate ions, so there is no reserve to take up added acid.
Final Answer:
Acetic acid with NaCl is not a buffer solution. \[ \boxed{\text{(D) }\text{CH}_{3}\text{COOH}+\text{NaCl}\text{ in water}} \]
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