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Acidity of Alcohols and Phenols

Acetic acid a...

Question

Acetic acid and $a q . N H_{3}$ are weak monobasic acid and weak monoacidic base respectively and $K_{a}$ of acetic acid is equal to $K_{b}$ of $a q . N H_{3}$ . Which of the following statements are incorrect?

The mixing of

C H_{3} C O O H

and

N H_{3}

in any proportion would result in neutral solution having

p H = 7

25^{\circ} C

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a q . N H_{3}

is exactly half neutralised by

H C l

, then

p O H

of resulting solution is equal to

p K_{b}

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If acetic acid is exactly half neutralised by

N a O H

then

p H

of resulting solution is equal to

p K_{b}

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If acetic acid is exactly neutralised by

a q . N H_{3}

then

p H

of resulting solution is equal to

1 / 2 p K_{w}

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Solution

The correct options are
C If acetic acid is exactly half neutralised by $N a O H$ then $p H$ of resulting solution is equal to $p K_{b}$
D If acetic acid is exactly neutralised by $a q . N H_{3}$ then $p H$ of resulting solution is equal to $1 / 2 p K_{w}$

Suggest Corrections

Similar questions

0.2 M

0.1 M

N a O H

0.5

K_{a}

{C H}_{3} C O O H = 1.8 \times 10^{- 5} .

Solutions of sodium hydroxide and acetic acid are mixed by the reaction: $N a O H + C H_{3} C O O H ⟶ C H_{3} C O O N a + H_{2} O$

Acetic acid is a weak acid. If equal volumes of equal molar solutions are mixed, the pH of the solution will be:

500 m L

0.2 M

500 m L

0.2 M

H C l

25^{o} C

6 g

N a O H

K_{a}

1.75 \times 10^{- 5} M L^{- 1}

5.0 m L

0.1 M N a O H

50 m L

0.1 M

p H

(K a = 1.8 \times 10^{- 5})

500 m L

0.2 M

500 m L

0.30 M

1.5 \times 10^{- 5}

p H

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