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Salt of Weak Acid and Strong Base

0.1 M weak ac...

Question

0.1 M weak acid HA (pH = 3) is titrated with 0.05 M NaOH solution. Calculate the pH (approx.) when 25% of acid has been neutralised. (\log 3 = 0.48)

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0.1 M

{C H}_{3} C O O H

0.05 M

N a O H

p H

0.1 M

{C H}_{3} C O O H

3

p H

\frac{1}{4}

[H^{+}]

0.1 M, 25 m L

H A (K_{a (H A)} = 10^{- 5})

0.05 M N a O H

N a O H

36.12 m L

0.1 M N a O H

18.06 m L 0.1 M H C l

p H

4.92

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0.10 M

p H = 3

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C H_{3} C O O H

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p K_{a}

C H_{3} C O O H = 4.74

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