Question:
Which one of the pairs will form a buffer solution?
Which one of the pairs will form a buffer solution?
Show Hint
To quickly identify a buffer solution:
- Look for a Weak Acid + its conjugate salt (Acidic Buffer).
- Look for a Weak Base + its conjugate salt (Basic Buffer).
Pairs containing strong acids or bases alone (like $\text{NaOH}$) do not form buffers unless they are part of a partial neutralization reaction where the weak component remains in excess.
- Look for a Weak Acid + its conjugate salt (Acidic Buffer).
- Look for a Weak Base + its conjugate salt (Basic Buffer).
Pairs containing strong acids or bases alone (like $\text{NaOH}$) do not form buffers unless they are part of a partial neutralization reaction where the weak component remains in excess.
Updated On: Jun 3, 2026
- $\text{CH}_3\text{COONa}$ & $\text{NaOH}$
- $\text{CH}_3\text{COONH}_4$ & $\text{NH}_4\text{Cl}$
- $\text{NH}_4\text{Cl}$ & $\text{NH}_4\text{OH}$
- $\text{CH}_3\text{COONa}$ & $\text{HCl}$
Show Solution
Verified By Collegedunia
The Correct Option is C
Solution and Explanation
Step 1: Understanding the Question:
The question asks to identify which of the given mixtures of chemical species will act as a buffer solution.
Step 2: Detailed Explanation:
• A buffer solution is an aqueous solution that resists changes in its pH level upon the addition of small amounts of a strong acid or a strong base.
• Buffer solutions are of two primary types:
- Acidic Buffer: Formed by mixing a weak acid and its salt with a strong base (e.g., $\text{CH}_3\text{COOH}$ and $\text{CH}_3\text{COONa}$).
- Basic Buffer: Formed by mixing a weak base and its salt with a strong acid (e.g., $\text{NH}_4\text{OH}$ and $\text{NH}_4\text{Cl}$).
• Let us analyze each of the given options:
• Option (A): $\text{CH}_3\text{COONa}$ is a salt of a weak acid and a strong base, and $\text{NaOH}$ is a strong base. Since there is no weak acid or weak base present, this pair cannot act as a buffer solution.
• Option (B): $\text{CH}_3\text{COONH}_4$ is a salt of a weak acid and weak base, and $\text{NH}_4\text{Cl}$ is a salt of a weak base and strong acid. A mixture of two salts does not form a standard buffer solution.
• Option (C): $\text{NH}_4\text{OH}$ is a weak base, and $\text{NH}_4\text{Cl}$ is its conjugate salt formed with a strong acid ($\text{HCl}$). This matches the exact definition of a basic buffer solution. Therefore, this pair will form a buffer.
• Option (D): $\text{CH}_3\text{COONa}$ is a salt and $\text{HCl}$ is a strong acid. Although they can react to form a weak acid ($\text{CH}_3\text{COOH}$), the given pair itself is not a buffer mixture unless mixed in specific non-stoichiometric ratios where the weak acid is generated in excess alongside its salt. Among the direct choices, Option (C) is the classic basic buffer.
Step 3: Final Answer:
The pair that will form a buffer solution is $\text{NH}_4\text{Cl}$ & $\text{NH}_4\text{OH}$.
The question asks to identify which of the given mixtures of chemical species will act as a buffer solution.
Step 2: Detailed Explanation:
• A buffer solution is an aqueous solution that resists changes in its pH level upon the addition of small amounts of a strong acid or a strong base.
• Buffer solutions are of two primary types:
- Acidic Buffer: Formed by mixing a weak acid and its salt with a strong base (e.g., $\text{CH}_3\text{COOH}$ and $\text{CH}_3\text{COONa}$).
- Basic Buffer: Formed by mixing a weak base and its salt with a strong acid (e.g., $\text{NH}_4\text{OH}$ and $\text{NH}_4\text{Cl}$).
• Let us analyze each of the given options:
• Option (A): $\text{CH}_3\text{COONa}$ is a salt of a weak acid and a strong base, and $\text{NaOH}$ is a strong base. Since there is no weak acid or weak base present, this pair cannot act as a buffer solution.
• Option (B): $\text{CH}_3\text{COONH}_4$ is a salt of a weak acid and weak base, and $\text{NH}_4\text{Cl}$ is a salt of a weak base and strong acid. A mixture of two salts does not form a standard buffer solution.
• Option (C): $\text{NH}_4\text{OH}$ is a weak base, and $\text{NH}_4\text{Cl}$ is its conjugate salt formed with a strong acid ($\text{HCl}$). This matches the exact definition of a basic buffer solution. Therefore, this pair will form a buffer.
• Option (D): $\text{CH}_3\text{COONa}$ is a salt and $\text{HCl}$ is a strong acid. Although they can react to form a weak acid ($\text{CH}_3\text{COOH}$), the given pair itself is not a buffer mixture unless mixed in specific non-stoichiometric ratios where the weak acid is generated in excess alongside its salt. Among the direct choices, Option (C) is the classic basic buffer.
Step 3: Final Answer:
The pair that will form a buffer solution is $\text{NH}_4\text{Cl}$ & $\text{NH}_4\text{OH}$.
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