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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
$p H = - l o g K_{a} + l o g \frac{[S a l t]}{[A c i d]}$
$p H = - l o g [1.8 \times 10^{- 5}] + l o g \frac{[S a l t]}{[A c i d]}$
$p H = - l o g [1.8 \times 10^{- 5}] + l o g \frac{2.0}{1.5}$
$p H = 4.745 + 0.124 = 4.869$

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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. Calculate the ratio of pH of a solution containing 1 mol of

C H_{3} C O O N a

+ 1 mol of

H C l

per litre to another solution containing 1 mol of

C H_{3} C O O N a

+ 1 mol of acetic acid per litre.

Q. What is the pH of the solution when

0.2 m o l e

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}

for

{C H}_{3} C O O H = 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

molar buffer solution of pH

4.5

?
(

K_{a}

for

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

)

Q. What is

[H +]

in mol per litre of the solution that is

0.02 M

{C H}_{3} C O O N a

and

0.01 M

{C H}_{3} C O O H

(K_{a} f o r {C H}_{3} C O O H = 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[1.8×10−5]+log[Salt][Acid] pH=−log[1.8×10−5]+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 $1.8 \times 10^{- 5})$