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Standard XII

Chemistry

Henderson Hassleback Equation

The pH of a b...

Question

The pH of a buffer solution containing 2.0 mol per litre $C H_{3} C O O N a$ and 1.5 mol per litre $C H_{3} C O O H$ is: ( $K_{a}$ for acetic acid is $1.8 \times 10^{- 5})$

4.87

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5.8

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2.4

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9.2

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Solution

The correct option is A 4.87
The given solution is acidic buffer so Henderson-Hasselbach equation is
$p H = - l o g K_{a} + l o g \frac{[S a l t]}{[A c i d]}$
$p H = - l o g [1.8 \times 10^{- 4}] + l o g \frac{[S a l t]}{[A c i d]}$
$p H = - l o g [1.8 \times 10^{- 4}] + l o g \frac{2.0}{1.5}$
$p H = 4.745 + 0.124 = 4.869$

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Similar questions

Q. The pH of a buffer solution containing 2.0 mol per litre

C H_{3} C O O N a

and 1.5 mol per litre

C H_{3} C O O H

is: (

K_{a}

for acetic acid is

1.8 \times 10^{- 5})

Q. What is the pH of the solution when 0.2 mole of hydrochloric acid is added to one litre of a solution containing 1 M acetic acid and acetate ion? Assume that the total volume is one litre.

K_{a}

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{CH}_{3} COOH = 1.8 \times 10^{- 5}

Q. What will be the new

p H

0.01 m o l

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is added to a

1 L

buffer solution that is

0.1 M

in acetic acid

(C H_{3} C O O H)

and

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in sodium acetate

(C H_{3} C O O N a)

?
Dissociation constant

K_{a}

of acetic acid at

25^{\circ} C

1.8 \times 10^{- 5}

Q. How many moles of acetic acid and sodium acetate each should be dissolved to prepare one litre of

0.063

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?
(

K_{a}

for

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

)

Q. Suppose it is required to make a buffer solution of pH = 4, using acetic acid and sodium acetate.
How many grams of sodium acetate is to be added to one litre of

\frac{N}{10}

acetic acid?

K_{a} = 1.8 \times 10^{- 5}

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Henderson Hassleback Equation

Standard XII Chemistry

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The pH of a buffer solution containing 2.0 mol per litre CH3COONa and 1.5 mol per litre CH3COOH is: (Ka for acetic acid is 1.8×10−5)

The correct option is A 4.87The given solution is acidic buffer so Henderson-Hasselbach equation is pH=−log Ka+log[Salt][Acid] pH=−log[1.8×10−4]+log[Salt][Acid] pH=−log[1.8×10−4]+log2.01.5 pH=4.745+0.124=4.869

The pH of a buffer solution containing 2.0 mol per litre $C H_{3} C O O N a$ and 1.5 mol per litre $C H_{3} C O O H$ is: ( $K_{a}$ for acetic acid is $1.8 \times 10^{- 5})$