HARD

JEE Main

IMPORTANT

Earn 100

The concentration of hydrogen ion in a $0.2 M$ solution of formic acid is $6.4 \times 10^{- 3} mol$ per litre. To this solution, sodium formate is added to adjust the concentration of sodium formate to one mole per litre. What will be the $pH$ of this solution? The dissociation constant of formic acid is $2.4 \times 10^{- 4}$ and the degree of dissociation of sodium formate is $0.75$ .

50% studentsanswered this correctly

Important Questions on Ionic Equilibrium in Aqueous Solutions

HARD

JEE Main

IMPORTANT

Modern Approach to Chemical Calculations>Chapter 16 - Ionic Equilibrium in Aqueous Solutions>PROBLEMS>Q 23

When

0.20 M

acetic acid is neutralised with

0.20 M NaOH

0.50 L

of solution, the resulting solution is slightly alkaline. Calculate the

pH

of the resulting solution.

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

HARD

JEE Main

IMPORTANT

Modern Approach to Chemical Calculations>Chapter 16 - Ionic Equilibrium in Aqueous Solutions>PROBLEMS>Q 24

The

pH

of a

0.1 M

solution of

{NH}_{4} Cl

5.13

. Find the dissociation constant of

{NH}_{4} OH

. Give answer as

=

dissociation constant

\times 10^{5}

HARD

JEE Main

IMPORTANT

Modern Approach to Chemical Calculations>Chapter 16 - Ionic Equilibrium in Aqueous Solutions>PROBLEMS>Q 25

A buffer solution is prepared by dissolving

0.2 mole

of sodium formate and

0.25 mole

of formic acid in approximately

200 (\pm 50)

mL

of water. What will be the concentration of

H^{+}

and

{OH}^{-} ? K_{a} (HCOOH) = 1.8 \times 10^{- 4}

HARD

JEE Main

IMPORTANT

Modern Approach to Chemical Calculations>Chapter 16 - Ionic Equilibrium in Aqueous Solutions>PROBLEMS>Q 26

A buffer solution was prepared by dissolving $0.05 mole$ formic acid and $0.06 mole$ sodium formate in enough water to make $1 litre$ of solution. $K_{a} (HCOOH) = 1.8 \times 10^{- 4}$ .

Calculate the $pH$ of the solution.

HARD

JEE Main

IMPORTANT

Modern Approach to Chemical Calculations>Chapter 16 - Ionic Equilibrium in Aqueous Solutions>PROBLEMS>Q 26

A buffer solution was prepared by dissolving $0.05 mole$ formic acid and $0.06 mole$ sodium formate in enough water to make $1 litre$ of solution. $K_{a} (HCOOH) = 1.8 \times 10^{- 4}$ .

If this solution were diluted to $10$ times its volume, what would be the $pH$ ?

HARD

JEE Main

IMPORTANT

Modern Approach to Chemical Calculations>Chapter 16 - Ionic Equilibrium in Aqueous Solutions>PROBLEMS>Q 27

How many

gram moles

HCl

will be required to prepare one

litre

of a buffer solution (containing

NaCN

and

HCN

) of

pH 8.5

using

0.01

gram

-formula weight of

NaCN ? K_{dissociation} (HCN) = 4.1 \times 10^{- 10}

HARD

JEE Main

IMPORTANT

Modern Approach to Chemical Calculations>Chapter 16 - Ionic Equilibrium in Aqueous Solutions>PROBLEMS>Q 28

The

{pK}_{a}

of acetyl salicylic acid (aspirin) is

3 \cdot 5

. The

pH

of gastric juice in the human stomach is about

2 - 3

and the

pH

in the small intestine is about

8

. Aspirin will be

HARD

JEE Main

IMPORTANT

Modern Approach to Chemical Calculations>Chapter 16 - Ionic Equilibrium in Aqueous Solutions>PROBLEMS>Q 29

Calculate the degree of hydrolysis of an

N / 10

KCN

solution at

25 ° C

K_{a} (HCN) = 7.2 \times 10^{- 10}; K_{w} = 1 \times 10^{- 14}

Important Questions on Ionic Equilibrium in Aqueous Solutions

Learn and Prepare for any exam you want !