EASY

JEE Main/Advance

IMPORTANT

Earn 100

$5$ litre of a solution of $H_{2} O_{2}$ with $x N$ strength is diluted to $5.5$ litre. This $5.5$ litre $H_{2} O_{2}$ solution gives $28$ litre $O_{2}$ at NTP. Find the value of $x$ .

Important Questions on Solutions

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 8 - Solutions>EXERCISE-4>Q 8

Two beaker

A and B

present in a closed vessel. Beaker

A

contains

152 .4 g

aqueous solution of urea, containing

12 g

of urea. Beaker

B

contains

196.2 g

aqueous solution of glucose, containing

18 g

of glucose. Both solutions allowed to attain the equilibrium. Determine

w / w %

of glucose in its solution at equilibrium.

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 8 - Solutions>EXERCISE-4>Q 9

The vapour pressure of two pure liquids

A

and

B

, that form an ideal solution, are

100

and

900 torr

respectively at temperature

T

. This liquid solution of

A

and

B

is composed of

1

mole of

A

and

1

mole of

B

. What will be the pressure, when

1

mole of mixture has been vaporized ?

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 8 - Solutions>EXERCISE-4>Q 10

The addition of

3 g

of substance to

100 g {CCl}_{4} (M = 154 g {mol}^{- 1})

raises the boiling point of

{CCl}_{4}

0.60 ° C

K_{b} ({CCl}_{4})

5.03 kg {mol}^{- 1} K

. Calculate:
(a) the freezing point depression
(b) the relative lowering of vapour pressure
(c) the osmotic pressure at

298 K

(d) the molar mass of the substance
Given

K_{f} ({CCl}_{4}) = 31.8 kg {mol}^{- 1} K

and

ρ

(density) of solution

= 1.64 g {cm}^{3}

MEDIUM

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 8 - Solutions>EXERCISE-4>Q 13

30 mL

{CH}_{3} OH (d = 0.7980 g {cm}^{- 3})

and

70 mL

H_{2} O (d = 0.9984 g {cm}^{- 3})

are mixed at

25 ° C

to form a solution of density

0.9575 g {cm}^{- 3}

. Calculate the freezing point of the solution.

K_{f} (H_{2} O)

1.86 kg {mol}^{- 1} K

. Also calculate its molarity.

MEDIUM

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 8 - Solutions>EXERCISE-4>Q 14

The freezing point depression of a

0.109 M

aq. solution of formic acid is

- 0.21 ° C

. Calculate the equilibrium constant for the reaction,

HCOOH (aq) ⇌ H^{+} (aq) + {HCOO}^{⊖} (aq)

K_{f}

for water

= 1.86 kg {mol}^{- 1} K

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 8 - Solutions>EXERCISE-4>Q 15

The freezing point of

0.02 mol

fraction solution of acetic acid

(A)

in benzene

(B)

277.4 K

. Acetic acid exists partly as a dimer

2 A = A_{2}

. Calculate equilibrium constant for the dimerisation. Freezing point of benzene is

278.4 K

and its heat of fusion

{ΔH}_{f}

10.042 kJ {mol}^{- 1}

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 8 - Solutions>EXERCISE-4>Q 16

The vapour pressure of two miscible liquids

(A)

and

(B)

are

300

and

500 mm

Hg

respectively. In a flask

10

mole of

(A)

is mixed with

12

mole of

(B)

. However, as soon as

(B)

is added,

(A)

starts polymerising into a completely insoluble solid. The polymerisation follows first-order kinetics. After

100

minute,

0.525

mole of a solute is dissolved which arrests the polymerisation completely. The final vapour pressure of the solution is

400 mm

Hg

. Estimate the rate constant of the polymerisation reaction. Assume negligible volume change on mixing and polymerisation, and ideal behaviour for the final solution.

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 8 - Solutions>EXERCISE-4>Q 17

1.5 g

of monobasic acid when dissolved in

150 g

of water lowers the freezing point by

0.165 ° C . 0.5 g

of the same acid when titrated, after dissolution in water, requires

37.5 mL

N 10

alkali. Calculate the degree of dissociation of the acid

(K_{f}

for water

= 1.86 ° C {mol}^{- 1})

5 litre of a solution of H2O2 with x N strength is diluted to 5.5 litre. This 5.5 litre H2O2 solution gives 28 litre O2 at NTP. Find the value of x.

Important Questions on Solutions

Learn and Prepare for any exam you want !

$5$ litre of a solution of $H_{2} O_{2}$ with $x N$ strength is diluted to $5.5$ litre. This $5.5$ litre $H_{2} O_{2}$ solution gives $28$ litre $O_{2}$ at NTP. Find the value of $x$ .