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(A) The given solution is a basic buffer solution consisting of a weak base $(NH_4OH)$ and its salt with a strong acid $(NH_4Cl)$.Adding a small amoun

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Adding $1 \, mL$ of water

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(A) The given solution is a basic buffer solution consisting of a weak base $(NH_4OH)$ and its salt with a strong acid $(NH_4Cl)$.Adding a small amount of water to a buffer solution causes dilution,which changes the concentration of the components,but the ratio of $[Salt]/[Base]$ remains constant.According to the Henderson-Hasselbalch equation: $pOH = pK_b + \log(\frac{[Salt]}{[Base]})$.Since the ratio $[Salt]/[Base]$ does not change significantly upon dilution,the $pH$ of the buffer solution remains unchanged.Therefore,adding $1 \, mL$ of water will not change the $pH$.

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

For a $10 \, mL$ solution containing $0.1 \, M \, NH_4Cl$ and $0.01 \, M \, NH_4OH$,which of the following additions will not change the $pH$ of the solution?

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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
$I$ $4.0$ $4.0$
$II$ $4.0$ $40.0$
$III$ $40.0$ $4.0$
$IV$ $0.1$ $10.0$

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