Textbook for Class XI Chemistry Part I>Chapter 7 - Equilibrium>EXERCISES>Q 7.39

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IMPORTANT

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The species: $H_{2} O, H C O_{3}^{-}, H S O_{4}^{-}$ and ${N H}_{3}$ can act both as Brönsted acids and bases. For each case give the corresponding conjugate acid and base.

Important Questions on Equilibrium

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11th CBSE

IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 7 - Equilibrium>EXERCISES>Q 7.4

Classify the following species into Lewis acids and Lewis bases and show how these act as Lewis acid/base:
(a)

{O H}^{-}

(b)

F^{-}

(c)

H^{+}

(d)

{B C l}_{3}

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IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 7 - Equilibrium>EXERCISES>Q 7.41

The concentration of hydrogen ion in a sample of soft drink is

3.8 \times 10^{- 3} M

. what is its

p H

?

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IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 7 - Equilibrium>EXERCISES>Q 7.42

The

p H

of a sample of vinegar is

3.76

. Calculate the concentration of hydrogen ion in it.

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11th CBSE

IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 7 - Equilibrium>EXERCISES>Q 7.43

The ionization constant of

H F, H C O O H

and

H C N

at

298 K

are

6.8 \times 10^{- 4}, 1.8 \times 10^{- 4}

and

4.8 \times 10^{- 9}

respectively. Calculate the ionization constants of the corresponding conjugate base.

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IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 7 - Equilibrium>EXERCISES>Q 7.44

The ionization constant of phenol is

1.0 \times 10^{10} .

What is the concentration of phenolate ion in

0.05 M

solution of phenol? What will be its degree of ionization if the solution is also

0.01 M

in sodium phenolate?

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11th CBSE

IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 7 - Equilibrium>EXERCISES>Q 7.45

The first ionization constant of

H_{2} S

is

9.1 \times 10^{- 8} .

Calculate the concentration of

{H S}^{-}

ion in its

0.1 M

solution. How will this concentration be affected if the solution is

0.1 M

in

H C l

also? If the second dissociation constant of

H_{2} S

is

1.2 \times 10^{- 13}

, calculate the concentration of

S^{2 -}

under both conditions.

HARD

11th CBSE

IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 7 - Equilibrium>EXERCISES>Q 7.46

The ionization constant of acetic acid is

1.74 \times 10^{- 5}

. Calculate the degree of dissociation of acetic acid in its

0.05 M

Solution.Calculate the concentration of acetate ion in the solution and its

p H .

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11th CBSE

IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 7 - Equilibrium>EXERCISES>Q 7.47

It has been found that the

p H

of a

0.01 M

solution of an organic acid is

4.15

. Calculate the concentration of the anion, the ionization constant of the acid and its

p K a

.