Chemistry Standard 12 Vol II>Chapter 1 - Ionic Equilibrium>Evaluate yourself - 3>Q 1

HARD

12th Tamil Nadu Board

IMPORTANT

Earn 100

Identify the Lewis acid and the Lewis base in the following reactions.

Important Questions on Ionic Equilibrium

HARD

12th Tamil Nadu Board

IMPORTANT

Chemistry Standard 12 Vol II>Chapter 1 - Ionic Equilibrium>Evaluate yourself - 4>Q 1

$H_{3} {BO}_{3}$ accepts hydroxide ion from water as shown below

$H_{3} {BO}_{3} (aq) + H_{2} O (l) ⇌ B (OH)_{4} + H^{+}$

Predict the nature of $H_{3} {BO}_{3}$ using Lewis concept

MEDIUM

12th Tamil Nadu Board

IMPORTANT

Chemistry Standard 12 Vol II>Chapter 1 - Ionic Equilibrium>Evaluate yourself - 5>Q 1

At a particular temperature, the

K_{w}

of a neutral solution was equal to

4 \times 10^{- 14}

. Calculate the concentration of

[H_{3} O^{+}]

and

[{OH}^{-}]

.

MEDIUM

12th Tamil Nadu Board

IMPORTANT

Chemistry Standard 12 Vol II>Chapter 1 - Ionic Equilibrium>Evaluate yourself - 6>Q 1

Calculate

pH

of

10^{- 5} M H_{2} {SO}_{4}

.

HARD

12th Tamil Nadu Board

IMPORTANT

Chemistry Standard 12 Vol II>Chapter 1 - Ionic Equilibrium>Evaluate yourself - 6>Q 1

Calculate the concentration of hydrogen ion in moles per litre of a solution whose

pH

is

5.4

HARD

12th Tamil Nadu Board

IMPORTANT

Chemistry Standard 12 Vol II>Chapter 1 - Ionic Equilibrium>Evaluate yourself - 6>Q 1

Calculate the

pH

of an aqueous solution obtained by mixing

50 ml

of

0.2 M HCl

with

50 ml 0.1 M NaOH

.

HARD

12th Tamil Nadu Board

IMPORTANT

Chemistry Standard 12 Vol II>Chapter 1 - Ionic Equilibrium>Evaluate yourself - 7>Q 1

K_{b}

for

{NH}_{4} OH

is

1.8 \times 10^{- 5}

. Calculate the percentage of ionisation of

0.06 M

ammonium hydroxide solution.

MEDIUM

12th Tamil Nadu Board

IMPORTANT

Chemistry Standard 12 Vol II>Chapter 1 - Ionic Equilibrium>Evaluate yourself - 8>Q 1

Explain the buffer action in a basic buffer containing equimolar ammonium hydroxide and ammonium chloride.

HARD

12th Tamil Nadu Board

IMPORTANT

Chemistry Standard 12 Vol II>Chapter 1 - Ionic Equilibrium>Evaluate yourself - 8>Q 1

Calculate the

pH

of a buffer solution consisting of

0.4 M {CH}_{3} COOH

and

0.4 M {CH}_{3} COONa

. What is the change in the

pH

after adding

0.01 mol

of

HCl

to

500 ml

of the above buffer solution. Assume that the addition of

HCl

causes negligible change in the volume. Given:

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

.