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(C) The solution is a buffer solution containing a weak acid (propanoic acid) and its salt with a strong base (sodium propanoate).For a buffer solutio

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$4.89$

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(C) The solution is a buffer solution containing a weak acid (propanoic acid) and its salt with a strong base (sodium propanoate).For a buffer solution,the $pH$ is calculated using the Henderson-Hasselbalch equation:$pH = pKa + \log \frac{[Salt]}{[Acid]}$Given that equal volumes are mixed,the concentrations of both the salt and the acid are halved,but their ratio remains the same:$[Salt] = 0.05 \ M$,$[Acid] = 0.05 \ M$$pKa = -\log(Ka) = -\log(1.3 	imes 10^{-5}) = 5 - \log(1.3) \approx 5 - 0.1139 = 4.8861$$pH = 4.8861 + \log \frac{0.05}{0.05} = 4.8861 + \log(1) = 4.8861 + 0 = 4.8861$Rounding to two decimal places,the $pH$ is approximately $4.89$.

Buffer Solution	Volume of $0.1 \ M$ Weak Acid (mL)	Volume of $0.1 \ M$ Sodium Salt (mL)
$I$	$4.0$	$4.0$
$II$	$4.0$	$40.0$
$III$	$40.0$	$4.0$
$IV$	$0.1$	$10.0$

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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