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Buffer Solutions

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p K_{b}

for

N H_{4} O H

at certain temperature is

4.74

. The

p H

of basic buffer containing equimolar concentration of

N H_{4} O H

and

N H_{4} C l

will be :

$9.26$
$4.74$
$7.74$
$2.37$

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Q. Which of the following can be used as a buffer solution?

A solution containing NaCl and NaOH.
A solution containing NaCl and NH₄OH.
A solution containing sodium acetate.
A solution containing ammonium acetate.

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Q. Aqueous solutions of

H N O_{3}, K O H, C H_{3} C O O H

and

C H_{3} C O O N a

of identical concentrations are provided. The pair(s) of solutions which form a buffer upon mixing is (are)

$H N O_{3} a n d C H_{3} C O O H$
$K O H a n d C H_{3} C O O N a$
$H N O_{3} a n d C H_{3} C O O N a$
$C H_{3} C O O H a n d C H_{3} C O O N a$

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Which of the following is not a buffer solution?

Ammonium chloride + ammonium hydroxide
Sodium acetate + acetic acid
NaOH + HCl
Sodium formate + formic acid

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On the addition of a small amount of an acid or a base, the pH value of a buffer solution:

decreases
remains unaltered
increases
none of these

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Q. If a buffer solution of 2, 4-dinitrophenol has a pH of 5, what is the ratio of dissociated to undissociated molecules of 2, 4-dinitrophenol in the solution? (p

K_{a}

of 2, 4-dinitrophenol = 4)

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0.1

mole arsenic acid

(H_{3} A s O_{4})

is dissolved in a 1L buffer solution of

p H = 8

. Which of the following options is/are correct? For arsenic acid:

K a_{1} = 2.5 \times 10^{- 4}, K a_{2} = 5 \times 10^{- 8}, K a_{3} = 2 \times 10^{- 13}

.
(‘<<’ sign denotes that the higher concentration is 100 times greater than the lower one or more)

$[H_{3} A s O_{4}] << [H_{2} A s O_{4}^{-}]$
$[H_{2} A s O_{4}^{-}] << [H A s O_{4}^{2 -}]$
$[H A s O_{4}^{2 -}] << [H_{2} A s O_{4}^{-}]$
$[A s O_{4}^{3 -}] << [H A s O_{4}^{2 -}]$

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Q. A buffer solution that has a pH of

4.72

is prepared by mixing of

1 M NaOH

and

1 M HCN

. What is the ratio of volumes of the acid to the base?

(p K_{b} {of CN}^{-} = 9.28)

1 : 1
1 : 2
2 : 1
3 : 1

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Q. Ionisation constant of benzoic acid is

6 \times 10^{- 5}

and

K_{s p}

of silver benzoate is

2.5 \times 10^{- 13}

. How many times is the salt more soluble in a buffer of

p H

of 4 as compared to its solubility in pure water?

(Given: \sqrt{\frac{2}{3}} = 0.82)

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Q. Which of the following solutions will alter the pH of the solution on dilution?

$0.1 M C H_{3} C O O N a$
$0.5 M H_{2} C O_{3} + 0.5 M N a H C O_{3}$
$1 M C H_{3} C O O N H_{4}$
$0.1 M N H_{4} O H + 0.1 M N H_{4} C l$

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