(D) For a weak acid titration,the $pH$ is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.At the $1/4$ stage of

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(D) For a weak acid titration,the $pH$ is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.At the $1/4$ stage of neutralization,$[Salt] = 1/4$ and $[Acid] = 3/4$. So,$pH_1 = pK_a + \log \frac{1/4}{3/4} = pK_a + \log(1/3) = pK_a - \log 3$.At the $3/4$ stage of neutralization,$[Salt] = 3/4$ and $[Acid] = 1/4$. So,$pH_2 = pK_a + \log \frac{3/4}{1/4} = pK_a + \log 3$.The difference in $pH$ is $\Delta pH = pH_2 - pH_1 = (pK_a + \log 3) - (pK_a - \log 3) = 2 \log 3$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Buffer solution

Difficult

$0.1 \ M$ $CH_3COOH$ is titrated against $0.1 \ M$ $NaOH$. What would be the difference in $pH$ between $1/4$ and $3/4$ stages of neutralization of the acid?

A
$2 \log \frac{3}{4}$
B
$2 \log \frac{1}{4}$
C
$2 \log \frac{8}{3}$
D
$2 \log 3$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Buffer solution

What is the $pH$ of a buffer solution prepared by mixing $0.01 \ M$ weak acid and $0.02 \ M$ salt of weak acid with a strong base? $(pK_{a} = 4.680)$

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Calculate the molar ratio of a weak acid $HA$ $(K_a=10^{-6})$ and its salt with a strong base,so that the $pH$ of the buffer solution is $6$.

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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:

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The $pH$ of an aqueous solution containing $1 \ M$ benzoic acid $(pK_{a}=4.20)$ and $1 \ M$ sodium benzoate is $4.5$. The volume of benzoic acid solution in $300 \ mL$ of this buffer solution is . . . . . . $mL$.

DifficultJEE MAIN 2024

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Study the following table:
Buffer Solution Volume (in $mL$) of $0.1 \ M$ Weak acid Volume (in $mL$) of $0.1 \ M$ sodium salt of weak acid
$I$ $4.0$ $4.0$
$II$ $4.0$ $40.0$
$III$ $40.0$ $4.0$
$IV$ $0.1$ $10.0$

Which of the two sets of buffer solutions have the least $pH$?

Buffer Solution	Volume (in $mL$) of $0.1 \ M$ Weak acid	Volume (in $mL$) of $0.1 \ M$ sodium salt of weak acid
$I$	$4.0$	$4.0$
$II$	$4.0$	$40.0$
$III$	$40.0$	$4.0$
$IV$	$0.1$	$10.0$

DifficultTS EAMCET 2004

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$0.1 \ M$ $CH_3COOH$ is titrated against $0.1 \ M$ $NaOH$. What would be the difference in $pH$ between $1/4$ and $3/4$ stages of neutralization of the acid?

Similar Questions

What is the $pH$ of a buffer solution prepared by mixing $0.01 \ M$ weak acid and $0.02 \ M$ salt of weak acid with a strong base? $(pK_{a} = 4.680)$

Calculate the molar ratio of a weak acid $HA$ $(K_a=10^{-6})$ and its salt with a strong base,so that the $pH$ of the buffer solution is $6$.

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:

The $pH$ of an aqueous solution containing $1 \ M$ benzoic acid $(pK_{a}=4.20)$ and $1 \ M$ sodium benzoate is $4.5$. The volume of benzoic acid solution in $300 \ mL$ of this buffer solution is . . . . . . $mL$.

Study the following table:Buffer SolutionVolume (in $mL$) of $0.1 \ M$ Weak acidVolume (in $mL$) of $0.1 \ M$ sodium salt of weak acid$I$$4.0$$4.0$$II$$4.0$$40.0$$III$$40.0$$4.0$$IV$$0.1$$10.0$Which of the two sets of buffer solutions have the least $pH$?

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Study the following table:
Buffer Solution Volume (in $mL$) of $0.1 \ M$ Weak acid Volume (in $mL$) of $0.1 \ M$ sodium salt of weak acid
$I$ $4.0$ $4.0$
$II$ $4.0$ $40.0$
$III$ $40.0$ $4.0$
$IV$ $0.1$ $10.0$

Which of the two sets of buffer solutions have the least $pH$?