A buffer solution of pH- 4 is to be prepared- using CH3COOH and CH3COONa- The concentration of acetic acid and sodium acetate are 110 M and x M- How much will the pH be if 1-5 L of H2O is added to above buffer - KaCH3COOH -4-7447

Using the Henderson Hasselbalch equation for weak acid: pH = pK_a + log [CH_3COONa][CH_3COOH] pH = log K_a + log [CH_3COONa][CH_3COOH] 4 = log 1.8 × 10^ 5 + l ...

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Standard XII

Chemistry

pH the Power of H

A buffer solu...

Question

A buffer solution of $p H = 4$ is to be prepared, using $C H_{3} C O O H$ and $C H_{3} C O O N a .$ The concentration of acetic acid and sodium acetate are $\frac{1}{10} M$ and $x M$ . How much will the $p H$ be if $1.5 L$ of $H_{2} O$ is added to above buffer ? $K_{a} (C H_{3} C O O H) = 4.7447$

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Solution

The correct option is A $4$
Using the Henderson-Hasselbalch equation for weak acid:
$p H = p K_{a} + l o g \frac{[C H_{3} C O O N a]}{[C H_{3} C O O H]}$
$p H = - l o g K_{a} + l o g \frac{[C H_{3} C O O N a]}{[C H_{3} C O O H]}$
$4 = - l o g 1.8 \times 10^{- 5} + l o g \frac{x}{\frac{1}{10}}$
$4 = 4.7447 + l o g 10 x$
$x = 0.018$ M
If $1.5 L$ of $H_{2} O$ is added it increases the volume, thereby decreasing concentration of both acid and salt. The ratio $l o g \frac{[S a l t]}{[A c i d]}$ remains constant.
So $p H$ remains same that is $p H = 4$

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Q. A buffer solution of

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pH the Power of H

Standard XII Chemistry

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A buffer solution of pH=4 is to be prepared, using CH3COOH and CH3COONa. The concentration of acetic acid and sodium acetate are 110 M and x M. How much will the pH be if 1.5 L of H2O is added to above buffer ? Ka(CH3COOH)=4.7447

A buffer solution of $p H = 4$ is to be prepared, using $C H_{3} C O O H$ and $C H_{3} C O O N a .$ The concentration of acetic acid and sodium acetate are $\frac{1}{10} M$ and $x M$ . How much will the $p H$ be if $1.5 L$ of $H_{2} O$ is added to above buffer ? $K_{a} (C H_{3} C O O H) = 4.7447$