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Acidic Buffer Action

3 grams of ac...

Question

3 grams of acetic acid is added to 250 mL of 0.1 M $H C l$ and the solution is made up to 500 mL. To 20 mL of this solution $\frac{1}{2} mL$ of 5 M $N a O H$ is added. The pH of this solution is .
(Given: $log 3 = 0.4771, p K_{a}$ of acetic acid = 4.74, molar mass of acetic acid = 60 g/mole).

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Solution

mmole of acetic acid in 20 mL = 2
mmole of $H C l$ in 20 mL = 1
mmole of $N a O H$ = 2.5

$\begin{matrix} H C l & + & N a O H & \to & N a C l & + & H_{2} O 1 & 2.5 & - & - - & 1.5 & 1 & 1 \end{matrix}$

$\begin{matrix} C H_{3} C O O H & + & N a O H (remaining) & \to & C H_{3} C O O N a & + & water 2 & 1.5 & - & - 0.5 & 0 & 1.5 & - \end{matrix}$

$p H = p K_{a} + log \frac{1.5}{0.5} = 4.74 + log 3 = 4.74 + 0.48 = 5.22$

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