20 ml of 0.2 M NaOH is added to 50 ml of 0.20 M acetic acid to give 70 ml of the solution. What is the pH of the solution?

The ionisation constant of acetic acid is $1.8 \times 10^{- 5}$ .

45.686

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4.5686

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45686

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0.456

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Solution

The correct option is B 4.5686
$N a O H + C H_{3} C O O H \to C H_{3} C O O N a + H_{2} O$

6 mmol of acetic acid and 4 mmol of sodium acetate will be left in the solution after the reaction.
$p H = p K_{a} - l o g \frac{[s o d i u m a c e t a t e]}{[a c e t i c a c i d]}$
$p H = 4.74 - l o g \frac{4}{6}$
$p H = 4.5686$

Option B is correct.

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Similar questions

Q. 20 mL of 0.2 M

N a O H

is added to 50 mL of 0.2 M acetic acid to give 70 mL of the solution. What is the

p H

of this solution? Calculate the additional volume of 0.2 M

N a O H

required to make the

p H

of the solution 4.74. The ionisation constant of acetic acid is

1.8 \times 10^{- 5}

20 mL of 0.2 M NaOH is added to 50 mL of 0.2 M acetic acid to give 70 mL of the solution. What is the $p H$ of the solution? Calculate the additional volume $x$ (in mL) of 0.2 M NaOH required to make pH of the solution 4.74. The ionisation constant of acetic acid is $1.8 \times 10^{- 5}$ .