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Standard XII

Chemistry

Auto Protolysis of Water

If the ioniza...

Question

If the ionization (dissociation) constant of acetic acid is $k_{a}$ , what will be the pH of a solution containing equal concentrations of acetic acid and sodium acetate?

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Solution

For an acidic buffer solution made from acetic acid and sodium acetate,
$p H = p K a + l o g \frac{[C H_{3} C O O N a]}{[C H_{3} C O O H]}$
For a solution containing equal concentrations of acetic acid and sodium acetate
$\frac{[C H_{3} C O O N a]}{[C H_{3} C O O H]} = 1$
$l o g \frac{[C H_{3} C O O N a]}{[C H_{3} C O O H]} = l o g 1 = 0$
$p H = p K a$

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If the ionization (dissociation) constant of acetic acid is ka, what will be the pH of a solution containing equal concentrations of acetic acid and sodium acetate?

For an acidic buffer solution made from acetic acid and sodium acetate, pH=pKa+log[CH3COONa][CH3COOH]For a solution containing equal concentrations of acetic acid and sodium acetate[CH3COONa][CH3COOH]=1log[CH3COONa][CH3COOH]=log1=0pH=pKa

If the ionization (dissociation) constant of acetic acid is $k_{a}$ , what will be the pH of a solution containing equal concentrations of acetic acid and sodium acetate?