To 20 ml of 0.1 M – NaOH solution, 3 ml of 1 M acetic acid solution is added. Is the solution now ne

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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)

Accepted Answer

$\underset{\begin{aligned} & 2	ext{ m mole} \ & 	ext{Final 0} \end{aligned}}{OH^{-}} + \underset{\begin{aligned} & 3	ext{ m mole} \ & 	ext{1 m mole} \end{aligned}}{ACOH} ightleftharpoons \underset{\begin{aligned} & 0 \ & 2	ext{ m mole} \end{aligned}}{ACO^{-}} + H_{2}O$$P^{H} = 4.74 + \log\frac{2}{1} = 5.04\left( 	ext{Acidic} ight)$Addition of 1 ml ACOH will decrease PH by 0.3 unit.

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