Question # 1

How many cm³of 1 M H₂SO₄required to neutralize 10 cm³of 1 M NaOH

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2 cm³

2.5 cm³

5 cm³

10 cm³

A solution has 92 g of ethyl alcohol, 96 g of methyl alcohol and 90 g of water. Mole percentage of ethyl alcohol in the solution is

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10

20

25

50

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

The molar boiling point constant is the ration of elevation in boiling point to :

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Molarity

Mole fraction of solvent

Mole fraction of solute.

If liquids A and B form an ideal solution

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The enthalpy of mixing is zero

The entropy of mixing is zero

The free energy of mixing is zero

The free energy as well as the entropy of mixing are each zero

The molal elevation constant is the ratio of the elevation in boiling point to

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Molarity

Molality

Mole fraction of solute

Mole fraction of solvent

The solubility of a gas in water depends upon

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Nature of the gas

Temperature

Pressure of the gas

All of the above

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

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

5g of glucose is dissolved fro 100 cm of solution. Percentage of solution is :

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5 % v/w

5 % w/v

5 % w/w

The weight of pure NaOH required to prepare 250 cm³of 0.1 N solution is

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4 g

1 g

2 g

5 g

Which of the following solutions has the highest boiling point ?

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5.85% solution of sodium chloride.

18.0% solution of glucose.

6.0% solution of urea.

All have same boiling points.

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 solutions of NaCl and KCl are prepared separately by dissolving same amount of solute in water, which of the following statements is true fro these solutions ?

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KCl solution will have higher boiling point than NaCl solution.

Both the solutions have same boiling points.

KCl and NaCl solutions possess same vapour pressure.

KCl solution possesses lower freezing point than NaCl solution.

Which one of the following is an ideal solution that obeys Rault's law

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Ethanol + water

Benzene + toluene

HCI + water

Acetone + chloroform

Which one of the following mixture shows positive deviation form Rault's law and forms an azetrope with minimum boiling point

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Methanol + CCI₄

Methanol + acetone

Ether + HCI

Acetone + chloroform

A solution of glucose is 10% The volume to which 1g mole of it dissolved will be :

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8.1 dm³

1.7 dm³

1.8 dm³

6.1 dm³

Two solutions of NaCl and KCl are prepared separately by dissolving 0.1 M of the solute in water. Which of the following statements is not true for these solution

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KCl solution will have higher boiling point than NaCl solution

Both the solutions have same boiling

KCl and NaCl solution possess same vapour pressure

KCl solution possess same freezing point at NaCl solution

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%

Compared to a 1.0M aqueous solution of calcium chloride will have

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The same freezing and boiling point

A lower freezing point and lower boiling point

A lower freezing point and higher boiling point

A higher freezing point and higher boiling point

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

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1.8%

18%

0.18%

2.8%

Hydrolysis of potassium acetate produces

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Acidic solution

Neutral solution

Basic solution

None of these

Elevation of boiling point is measured by

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Beckmann's apparatus

Lands Berger's method

Antifreeze apparatus

None of these above

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

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Molarity

Formality

Molality

Mole fraction

The vant Hoff factor (1) accounts for

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Degree of solubilisation of solute

The extent of dissolution of solute

The degree of decomposition of solution

Precipitation will occur until the ionic product becomes

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Equal to K_sp

Lesser than K_sp

Greater than K_sp

None of these

Colligative properties are the properties of :

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Dilute solutions which behave as nearly ideal solutions.

Concentrated solutions which behave as nearly non-ideal solutions.

Both(i) and (ii)

Neither (i) nor (ii)

Isotonic solutions have same

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Molar concentration

Molality

Normality

None of these

Which one of the following has continuous solubility curve

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NH₄NO₃

CaCI

CaCI₂. 6H₂O

Na₂SO₄. 10H₂O

Partial pressure of a solution component is directly proportional to its mole fraction. This statement is known as

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Henry's law

Raoult's law

Distribution law

Ostwald's dilution law

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