Which of the following mixture can act as a buffer solution?...

Which of the following mixture can act as a buffer solution? (1) I litre of $0.2 \mathrm{~N} \mathrm{CH}_{3} \mathrm{COOH}+1$ litre of $0.2 \mathrm{~N} \mathrm{NaOH}$ (2) I litre of $0.1 \mathrm{~N} \mathrm{CH}_{3} \mathrm{COOH}+1$ litre of $0.2 \mathrm{~N} \mathrm{NaOH}$ (3) 1 litre of $0.2 \mathrm{~N} \mathrm{CH}_{3} \mathrm{COOH}+1$ litre of $0.1 \mathrm{~N} \mathrm{NaOH}$ (4) All the above

Which of the following mixture can act as a buffer solution?
(1) I litre of $0.2 \mathrm{~N} \mathrm{CH}_{3} \mathrm{COOH}+1$ litre of $0.2 \mathrm{~N} \mathrm{NaOH}$
(2) I litre of $0.1 \mathrm{~N} \mathrm{CH}_{3} \mathrm{COOH}+1$ litre of $0.2 \mathrm{~N} \mathrm{NaOH}$
(3) 1 litre of $0.2 \mathrm{~N} \mathrm{CH}_{3} \mathrm{COOH}+1$ litre of $0.1 \mathrm{~N} \mathrm{NaOH}$
(4) All the above

Key Concepts

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a useful tool for estimating the pH of a buffer solution. It relates the pH to the pKa (or pKb) of the weak acid (or weak base) and the ratio of the concentrations of the conjugate base to the weak acid, thereby guiding the design and adjustment of buffer systems.

Stoichiometry in Buffer Preparation

Correct stoichiometric ratios are critical when preparing a buffer solution. The amounts of weak acid and strong base (or weak base and strong acid) must be balanced so that after partial neutralization, sufficient quantities of both the weak component and its conjugate form remain to effectively counter subsequent pH changes.

Weak Acid and Conjugate Base

Weak acids only partially dissociate in solution, and in the presence of a strong base (or vice versa), they form a conjugate base. The combination of a weak acid and its conjugate base is essential for a buffer because it allows the solution to counteract pH changes through reversible reactions.

Acid-Base Neutralization Reaction

Acid-base neutralization involves a reaction where an acid reacts with a base to form water and a salt. In the context of buffers, controlled neutralization is used to generate a mixture that contains both unreacted weak acid and the corresponding salt, creating the optimal conditions for buffering.

Buffer Solution

A buffer solution is a system that resists significant changes in pH upon the addition of small amounts of acid or base. It achieves this by containing a weak acid and its conjugate base (or a weak base and its conjugate acid) that neutralize added H+ or OH– ions, ensuring the pH of the solution remains relatively constant.

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