Question # 1

Which is not a colligative property?

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Osmotic pressure

Lowering of vapour pressure

Depression of freezing point

Elevation of boiling point

A homogeneous mixture of two or more than two chemical substances is called

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Solute

Solution

Solvent

Salvation

The number of moles of NH₄CI dissolved in 500 cm³of its 15%, W/N solution is

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1 mole

1.4 mole

2.0 mole

2.4 mole

The osmotic pressure of solution increases if

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Temperature is decreased

Solution constant is increased

Number of solute molecules are increased

Volume is increased

Which substances are mixed to form a buffer solution?

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A strong acid and its salt of a strong base

Strong acid and its salt of weak base

Weak acid and its salt of strong base

Weak acid and its salt of weak base

The term cryoscopy is used for

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Depression of freezing point

Elevation in boiling poing

Lowering of vapour pressure

Osmotic pressure

0.1 molar glucose (C₆H₁₂O₆) solution has the % W/N

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1.8%

18%

0.18%

2.8%

A solution consisting of 92 grams ethyl alcohol (C₂H₅OH) 96 grams methyl alcohol (CH₃OH) 90 grams water the mole fraction and mole percent of methyl alcohol is

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0.3. 30%

0.2, 30%

0.5, 30%

0.2, 20%

A solution containing 5.8 grams acetone (CH₃OCH₃), 4.6 gram ethyl alcohol (C₂H₅OH) and 12 grams chloroform (CHl₃) has mole fraction and mole percent of acetone

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0.11, 10%

0.33, 33%

0.22, 22%

0.11, 33%

The sum of mole percent of all the components of solution is always equal to :

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Less than 100

One

100

10

Aqueous solution of glucose C₆H₁₂O₆, boils at 100.052°C. The solution contains

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180 grams glucose in 1 kg water

18 grams glucose in 1 kg water

1.8 grams glucose in 1 kg water

3.6 grams glucose in 1 kg

Number of moles of solute dissolved in 1 Kg of solvent is knowns as

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Molarity

Formality

Molality

Mole fraction

Which one of the following has discontinuous solubility curve

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CaCI₂6H₂O

NaCI

KCI

NaNO₃

The osmotic pressure of 1 m solution at 27°C is

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2.46 atm

24.6 atm

1.21 atm

12.1 atm

The process of osmosis was first discovered by

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Nollet

Pfeffer

Traube

Dutrochet

A one thousand dm³sample of water contains one gram of iron (iii) ions what is the concentration in parts per million of Fe^3f(eq) in parts per million

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0.001

0.01

0.1

1.0

What happens when isotonic solution of A (mol.wt.342) and B (mol.wt 60) are put in to communication through semipermeable membrane?

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Transference of solvent from solution A to that of B take place

Transference of solvent from solution B to that of A takes place

No transference of solvent from solution A to that of B takes place

Change in temperature of solutions takes place

What will be the molarity of solution if 103 g (NH₄)₂SO₄is dissolved per 600 cm³of water

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2.32 M

3.32 M

4.32 M

1.30 M

Maximum freezing point falls in

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Camphor

Naphthalene

Benzene

Water

Which of the following mixture of liquids show negative deviation form Raults law

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Ethyl alcohol and ether

HCI and water

Phenol- water

Chlorobenene-bromobenene

Dust particles in smoke is a solution of the type

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Liquid is solute and solid is solvent

Solid is solute and liquid is solvent

Solid is solute and gas is solvent

Gas is solute and solid is solvent

The process in which the solvent molecules are surrounded and interact with solute ions or molecules is called

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Solvation

Hydration

Hydrogenation

None

Saturated solution of NaCl on heating becomes

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Super saturated

Unsaturated

Remains saturated

None

Number of moles of the solute dissolved per dm³of the solution is knows as

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Molarity

Formality

%age

None of these

The example of colligative property is

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Boiling point

Osmosis

Freezing point

Osmotic pressure

The osmotic pressure of a dilute solution is directly proportional to the

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Diffusion rate of the solute

Ionic concentration

Elevation in boiling point

Flow of solvent from a concentrated to a dilute solution

In which type of following solutions we don't know the total volume of the solutions :

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Percentage weight/weight

Percentage weight/volume

Percentage volume/volume

Percentage volume/weight

The ionic strength of a solution containing 0.1 mole/kg of KCl and 0.2 mole/kg of CuSO₄is

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0.3

0.6

0.9

0.2

To calculate volume of the solvent, we need to know, the :

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Density of solute

Normality of solute

Mass of solute

Molarity of solute

Osmotic pressure of a solution increases by

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Decreasing the temperature

Increasing the volume

Increasing the number of molecules of the solute

None of the above

Camphor is often used in molecular mass determination because

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It is solvent for organic substances

It is readily available

It has a very high cryoscopic constant

It is volatile

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