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(B) For a buffer solution,the $pH$ is calculated using the Henderson-Hasselbalch equation:$pH = pKa + \log \left( \frac{[salt]}{[acid]} \right)$Since

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$I$ and $III$

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(B) For a buffer solution,the $pH$ is calculated using the Henderson-Hasselbalch equation:$pH = pKa + \log \left( \frac{[salt]}{[acid]} \right)$Since the molarity of the acid and the salt are the same $(0.1 \ M)$,the ratio $\frac{[salt]}{[acid]}$ is equivalent to the ratio of their volumes: $\frac{V_{salt}}{V_{acid}}$.The $pH$ is lowest when the ratio $\frac{[salt]}{[acid]}$ is the smallest,which occurs when the volume of the acid is high and the volume of the salt is low.Calculating the ratios for each:$I: \frac{4.0}{4.0} = 1.0$$II: \frac{40.0}{4.0} = 10.0$$III: \frac{4.0}{40.0} = 0.1$$IV: \frac{10.0}{0.1} = 100.0$Comparing the ratios,$III$ $(0.1)$ and $I$ $(1.0)$ have the lowest values. However,looking at the options provided,$III$ has the lowest ratio,followed by $I$. Re-evaluating the question for the two sets with the lowest $pH$,$III$ and $I$ are the correct candidates.

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

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 $pH$?

Similar Questions

An aqueous buffer is prepared by adding $100 \, mL$ of $0.1 \, mol \, L^{-1}$ acetic acid to $50 \, mL$ of $0.2 \, mol \, L^{-1}$ of sodium acetate. If $pK_a$ of acetic acid is $4.76$,the $pH$ of the buffer is

The $pH$ of a buffer solution made by mixing $25 \ mL$ of $0.02 \ M$ $NH_4OH$ and $25 \ mL$ of $0.2 \ M$ $NH_4Cl$ at $25^{\circ}C$ is ($pK_b$ of $NH_4OH = 4.8$).

Which of the following is a buffer solution?

Which of the following is a buffer solution?

Calculate the $pH$ of a buffer solution containing $0.04 \ M$ $NaF$ and $0.02 \ M$ $HF$ $[pK_a = 3.142]$.

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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 $pH$?

Similar Questions

An aqueous buffer is prepared by adding $100 \, mL$ of $0.1 \, mol \, L^{-1}$ acetic acid to $50 \, mL$ of $0.2 \, mol \, L^{-1}$ of sodium acetate. If $pK_a$ of acetic acid is $4.76$,the $pH$ of the buffer is

The $pH$ of a buffer solution made by mixing $25 \ mL$ of $0.02 \ M$ $NH_4OH$ and $25 \ mL$ of $0.2 \ M$ $NH_4Cl$ at $25^{\circ}C$ is ($pK_b$ of $NH_4OH = 4.8$).

Which of the following is a buffer solution?

Which of the following is a buffer solution?

Calculate the $pH$ of a buffer solution containing $0.04 \ M$ $NaF$ and $0.02 \ M$ $HF$ $[pK_a = 3.142]$.

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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 $pH$?