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pH the Power of H

500mL of 0....

Question

$500 m L$ of $0.2 M$ acetic acid are added to $500 m L$ of $0.30 M$ sodium acetate solution. If the dissociation constant of acetic acid is $1.5 \times 10^{- 5}$ then $p H$ of the resulting solution is:

5.0

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9.0

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3.0

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4.0

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Solution

The correct option is A $5.0$
$C H_{3} C O O N a$ - 500 ml x 0.2 M
$C H_{3} C O O H$ - 500 ml x 0.3 M $K_{a} = 1.5 \times 10^{- 5}$
$p H = p K_{a} + l o g [\frac{C H_{3} C O O N a}{C H_{3} C O O H}]$
$p H = - l o g (1.5 \times 10^{- 5}) + l o g [\frac{0.3}{0.2}] = - l o g 1.5 + 5 + l o g 1.5 = 5$

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