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Salt of Weak Acid and Strong Base

The pH of a...

Question

The $p H$ of a solution that contains $0.10 M$ sodium acetate and $0.03 M$ acetic acid is: $(p K a f o r C H_{3} C O O H = 4.57)$

4.09

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6.09

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5.09

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7.09

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Solution

The correct option is D $5.09$
The expression for the $p H$ of the acidic buffer solution is as given below.

$p H = p K_{a} + l o g \frac{[s a l t]}{[a c i d]}$

$p K_{a} = 4.57$

Substitute values in the above equation.

$p H = 4.57 + l o g \frac{0.1}{0.03} = 5.09$

Option C is correct.

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Similar questions

0.1 N

solution of sodium acetate will have pH________ (

p K_{a} = 4.57

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Calculate the pH of a solution of 0.10 M acetic acid after 50.0 mL of 0.10 M acetic acid solution is treated with 25.0 mL of 0.10 M NaOH. ( $K_{a}$ of acetic acid = $1.8 \times 10^{- 5}$ )

Q. A buffer solution contains 0.1

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The pH of a solution that contains 0.10M sodium acetate and 0.03M acetic acid is: (pKa for CH3COOH=4.57)

The correct option is D 5.09The expression for the pH of the acidic buffer solution is as given below.pH=pKa+log[salt][acid]pKa=4.57Substitute values in the above equation.pH=4.57+log0.10.03=5.09Option C is correct.

The $p H$ of a solution that contains $0.10 M$ sodium acetate and $0.03 M$ acetic acid is: $(p K a f o r C H_{3} C O O H = 4.57)$

The correct option is D $5.09$
The expression for the $p H$ of the acidic buffer solution is as given below.

$p H = p K_{a} + l o g \frac{[s a l t]}{[a c i d]}$

$p K_{a} = 4.57$

Substitute values in the above equation.

$p H = 4.57 + l o g \frac{0.1}{0.03} = 5.09$

Option C is correct.