HARD

JEE Main

IMPORTANT

Earn 100

The observed osmotic pressure for a $0.10 M$ solution of $Fe ({NH}_{4})_{2} ({SO}_{4})_{2}$ at $25 ° C$ is $10.8 atm$ . The expected and experimental (observed) values of Van't Hoff factor ' $i$ ' will be respectively; $(R = 0.082 L atm k^{-} {mol}^{- 1})$

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Important Questions on Solutions

HARD

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 8 - Solutions>JEE Main - 19th April 2014>Q 67

Choose the correct statement with respect to the vapour pressure of a liquid among the following :

EASY

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 8 - Solutions>JEE Main - 16th April 2018>Q 68

The mass of a non-volatile, non-electrolyte solute (molar mass

= 50 g {mol}^{- 1}

) needed to be dissolved in

114 g

octane to reduce its vapour pressure by

75 %

, is:

HARD

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 8 - Solutions>JEE Main - 12th January 2019 Shift 2>Q 69

Molecules of benzoic acid

(C_{6} H_{5} COOH)

dimerise in

30 g

of benzene. '

w

g

of benzoic acid shows a depression in freezing point equal to

2 K

. If the percentage association of the acid to form dimer in the solution is

80

, then

w

is:

(

Given that

K_{f} = 5 K kg {mol}^{- 1}

, molar mass of benzoic acid

= 122 {gmol}^{- 1})

MEDIUM

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 8 - Solutions>JEE Main - 12th January 2019 Shift 1>Q 70

The freezing point of a

4 %

aqueous solution of

X

is equal to the freezing point of a

12 %

aqueous solution of

Y

. If the molecular weight of

X

A

, then the molecular weight of

Y

will be

MEDIUM

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 8 - Solutions>JEE Main - 12th April 2019 Shift 2>Q 71

A solution is prepared by dissolving 0.6 g of urea (molar mass

= 60 g m o l^{- 1}

) and

1.8 g

of glucose (molar mass

= 180 g m o l^{- 1}

) in 100 mL of water at

27^{o} C .

The osmotic pressure of the solution is:
(

R = 0.08206 L

atm

K^{- 1} m o l^{- 1}

)

MEDIUM

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 8 - Solutions>JEE Main - 11th April 2015>Q 72

Determination of the molar mass of acetic acid in benzene using freezing point depression is affected by:

MEDIUM

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 8 - Solutions>JEE Main - 10th January 2019 Shift 2>Q 73

The elevation in boiling point for

1

molal solution of glucose is

2 K

. The depression in freezing point for

2

molal solution of glucose in the same solvent is

2 K .

The relation between

K_{b}

and

K_{f}

is:

HARD

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 8 - Solutions>JEE Main - 10th January 2019 Shift 1>Q 74

Liquids

A

and

B

form an ideal solution in the entire composition range. At

350 K,

the vapour pressure of pure A and pure B are

7 \times 10^{3} Pa

and

12 \times 10^{3} Pa

, respectively. The composition of the vapour in equilibrium with a solution containing 40 mole percent of A at this temperature is:

The observed osmotic pressure for a 0.10 M solution of Fe(NH4)2(SO4)2 at 25°C is 10.8 atm. The expected and experimental (observed) values of Van't Hoff factor 'i' will be respectively; (R = 0.082 L atm k- mol-1)

Important Questions on Solutions

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The observed osmotic pressure for a $0.10 M$ solution of $Fe ({NH}_{4})_{2} ({SO}_{4})_{2}$ at $25 ° C$ is $10.8 atm$ . The expected and experimental (observed) values of Van't Hoff factor ' $i$ ' will be respectively; $(R = 0.082 L atm k^{-} {mol}^{- 1})$