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Which may be added to one litre of water to act as a buffer :

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Important Questions on Ionic Equilibrium

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Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

What will be the

pH

of solution formed by mixing

10 mL 0.1 {MNaH}_{2} {PO}_{4}

15 mL

0.1 {MNa}_{2} {HPO}_{4}

[Given:

{pK}_{1} = 2.12, {pK}_{2} = 7.2]

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Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

Which of the following mixtures will have the lowest pH at $298 K ?$

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

A buffer solution can be prepared by mixing equal volumes of

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Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

Which among the following pairs is not an acidic buffer?

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Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

Which will make basic buffer?

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

The negative logarithm of dissociation constant of

{NH}_{4} OH

4.745

. A buffer solution contains

0.035

mole

{NH}_{4} OH

and

0.35

mole

{NH}_{4} Cl

per litre. The

pH

of the buffer solution is

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

Among the following, the correct statement is

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Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

The

pH

of the blood is maintained by buffer system given by

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Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

An acidic buffer is obtained on mixing:

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

A solution of

0.1

mole of

{CH}_{3} {NH}_{2} (K_{b} = 5 \times 10^{- 4})

and

0.08 mole

HCl

is diluted to one litre, then the

pOH

of the solution is

(\log 1.25 = 0.1)

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

If the molar concentrations of base and its conjugate acid are same, then

pOH

of the buffer solution is

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH 6. If ionization constant of HA is

10^{- 5}

, the ratio of salt to acid concentration in the buffer solution will be:

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

Calculate the

pH

of a solution containing

0.2 M {CH}_{3} COOH

and

0.1 M {CH}_{3} COONa .

The

K_{a}

{CH}_{3} COOH = 1.8 \times 10^{- 5} (- \log (1.8 \times 10^{- 5}) = 4.74)

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

For a buffer of a mixture of

0.12 mol L^{- 1}

{CH}_{3} COOH

and

0.12 mol L^{- 1} {CH}_{3} COONa,

the buffer capacity is

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

In a

100 mL

of buffer solution of acetic acid and sodium acetate, both are

0.1 mol

. In this buffer,

10 mL

0.01 mole

HCl

is added. The

pH

of the buffer

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Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

The

pH

of the solution containing

50 mL

each of

0.10 M

sodium acetate and

0.01 M

acetic acid is
[Given

{pK}_{a}

{CH}_{3} COOH = 4.57

]

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

A student needs to prepare a buffer solution of propanoic acid and its sodium salt with

pH 4

. The ratio of

\frac{[{CH}_{3} {CH}_{2} {COO}^{-}]}{[{CH}_{3} {CH}_{2} COOH]}

required to make buffer is Given :

K_{a} ({CH}_{3} {CH}_{2} COOH) = 1.3 \times 10^{- 5}

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Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

If the

pH

of a solution containing

10 mL

0.5 M {CH}_{3} COOH

and

10 mL

0.25 M NaOH

5

. What is the

{pK}_{a}

of the acid?

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Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

50 mL

0 .2 M

ammonia solution is treated with

25 mL of 0.2 M HCl

. If

{pK}_{b}

of ammonia solution is

4.75

, the

pH

of the mixture will be:

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Buffer Solutions

Which one of the following pairs of solution is not an acidic buffer?

Which may be added to one litre of water to act as a buffer :

Important Questions on Ionic Equilibrium

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