Solutions Test

Result

Solutions Test - 29

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Weekly Quiz Competition

Question 1
4 / -1

Two aqueous solution S₁ and S₂ are separated by a semi-permeable membrane.S₂ has lower vapour pressure than S₁. Then

A
More solvent will flow from S₁ to S₂

B
More solvent will flow from S₂ to S₁

C
Solvent from S₁ and S₂ will flow at equal rates

D
No flow will take place
Question 2
4 / -1

Which statement is incorrect about osmotic pressure (P), volume (V) and temperature (T)?

A

B

C

D

Solution
Question 3
4 / -1

n moles of a solute are dissolved in w g of water. If K_f is the molal depression constant of water, the freezing point of the solution will be

A

B

C

D

Solution
Question 4
4 / -1

The molecular mass of a solute cannot be calculated by one of the following relations

A

B

C

D
Question 5
4 / -1

Molal depression constant is calculated from the enthalpy of fusion (∆H_f ) and b.pt. of solvent using the relation

A

B

C

D

Solution
Question 6
4 / -1

Which of the following aqueous solution do you expect to have the lowest freezing point?

A
0.1m glucose (C₆H₁₂O₆)

B
0.1 m NaCl

C
0.1 m sucrose (C₁₂H₂₂O₁₁)

D
0.1 m BaCl₂
Question 7
4 / -1

The van’t Hoff’s factor (i) for a 0.2 molal aqueous solution of urea is

A
0.2

B
0.1

C
1.2

D
1.0
Question 8
4 / -1

If a substance undergoes association or dissociation in the solution and i is the van’t Hoff factor, then the expression for osmotic pressure is

A
iP = CRT

B

C
PV = inRT

D
PV = nRT/i
Question 9
4 / -1

Benzoic acid undergoes dimerisation in benzene solution, the van’t Hoff factor ‘i’ is related to the degree of association ‘x’ of the acid as

A
i = (1 – x)

B
i = (1 + x)

C
i = (1 – x/2)

D
i = (1 + x/2)

Solution
Question 10
4 / -1

For a dilute solution, Raoult’s law states that

A
The lowering of vapour pressure is equal to the mole fraction of the solute

B
The relative lowering of vapour pressure is equal to the mole fraction of the solute

C
The relative lowering of vapour pressure is equal to the amount of the solute in the solution

D
The vapour pressure of the solution is equal to the mole fraction of the solvent.