Ionic EquilibriumHard
Question
To 20 ml of 0.1 M – NaOH solution, 3 ml of 1 M acetic acid solution is added. Is the solution now neutral, acidic or alkaline? How much more of the acetic acid solution we add to produce a change of pH = 0.3 unit? (pKa for CH3COOH = 4.74, log 2 = 0.3)
Options
A.acidic, 2 ml
B.alkaline, 1 ml
C.acidic, 1 ml
D.neutral, 2 ml
Solution
$\underset{\begin{aligned} & 2\text{ m mole} \\ & \text{Final 0} \end{aligned}}{OH^{-}} + \underset{\begin{aligned} & 3\text{ m mole} \\ & \text{1 m mole} \end{aligned}}{ACOH} \rightleftharpoons \underset{\begin{aligned} & 0 \\ & 2\text{ m mole} \end{aligned}}{ACO^{-}} + H_{2}O$
$P^{H} = 4.74 + \log\frac{2}{1} = 5.04\left( \text{Acidic} \right)$
Addition of 1 ml ACOH will decrease PH by 0.3 unit.
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