Which of the following is a buffer solution?

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(D) buffer solution is formed when a weak acid reacts with a limited amount of a strong base,or a weak base reacts with a limited amount of a strong a

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All of these

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(D) buffer solution is formed when a weak acid reacts with a limited amount of a strong base,or a weak base reacts with a limited amount of a strong acid,resulting in a mixture of the weak electrolyte and its conjugate salt.$(A)$ $100 \ mL, 0.1 \ M \ CH_3COOH$ $(10 \ mmol)$ + $100 \ mL, 0.05 \ M \ NaOH$ $(5 \ mmol)$: This results in $5 \ mmol$ of $CH_3COOH$ and $5 \ mmol$ of $CH_3COONa$,forming an acidic buffer.$(B)$ $200 \ mL, 0.1 \ M \ NH_4OH$ $(20 \ mmol)$ + $200 \ mL, 0.08 \ M \ HCl$ $(16 \ mmol)$: This results in $4 \ mmol$ of $NH_4OH$ and $16 \ mmol$ of $NH_4Cl$,forming a basic buffer.$(C)$ $300 \ mL, 0.1 \ M \ NaOH$ $(30 \ mmol)$ + $500 \ mL, 0.1 \ M \ C_6H_5COOH$ $(50 \ mmol)$: This results in $20 \ mmol$ of $C_6H_5COOH$ and $30 \ mmol$ of $C_6H_5COONa$,forming an acidic buffer.Since all options result in a mixture of a weak acid/base and its salt,all are buffer solutions.

Similar Questions

In which of the following combinations is buffer action expected?
$1$. $NH_3 + NH_4Cl$
$2$. $HCl + NaCl$
$3$. $NH_3 + HCl$ in $2 : 1$ mole ratio
Select the correct answer using the code given below.

$A$ buffer solution is prepared by mixing $10 \ mL$ of $1.0 \ M$ acetic acid and $20 \ mL$ of $0.5 \ M$ sodium acetate and then diluted to $100 \ mL$ with distilled water. The $pH$ of the buffer solution is ($pK_a$ of acetic acid is $4.76$).

The approximate $pH$ of a solution formed by mixing equal volumes of $0.1 \ M$ sodium propanoate and $0.1 \ M$ propanoic acid (if the dissociation constant of propanoic acid is $1.3 \times 10^{-5}$) will be:

In order to prepare a buffer solution of $pH = 5.74$,sodium acetate is added to acetic acid. If the concentration of acetic acid in the buffer is $1.0 \ M$,the concentration of sodium acetate in the buffer is $......... \ M$. (Round off to the nearest integer).
[Given: $pKa$ (acetic acid) $= 4.74$]

The $pH$ of a simple sodium acetate buffer is given by $pH = pK_a + \log \frac{[Salt]}{[Acid]}$. $K_a$ of acetic acid $= 1.8 \times 10^{-5}$. If $[Salt] = [Acid] = 0.1 \, M$,the $pH$ of the solution would be about

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