Question # 1

A solutiion of 0.5 mole camphor in 100 grmas chloroform (K_b= 0.322) has rise in boiling point than that of chloroform by

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0.81°C

1.61°C

1.81°C

0.61°C

The process in which solvent particles surround solute particles is called

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Hydrolysis

Hydration

Solvation

Dissolution

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

The temperature at which the vapour pressure of a liquid becomes equal to external pressure is

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Melting point

Sublimation point

Inversion point

Boiling point

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

0.5 M of H₂SO₄is diluted from 1 litre to 10 litre, normality of resulting solution is

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1 N

0.1 N

10 N

11 N

Which of the following aqueous solutions have the lowest freezing point

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5.85% NaCI

6% urea

34.2 sucrose

All of them have same freezing points

Which is independent of temperature

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Molarity

Molality

Normality

Mole fraction

The vapour pressure of two liquids 'p' and 'Q' are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mol of Q would be

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140 torr

20 torr

68 torr

72 torr

Freezing point depression is measured by

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Beckmann's apparatus

Lands Berger's method

Antifreeze apparatus

All of the above

18 g glucose is dissolved in 90 g of water. The relative lowering vapor pressure is equal to :

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1/5

5.1

1/51

6

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

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Rault law

Henry law

Dalton law

Grahms law

Which of the statements given below concerning properties of solution, describe a colligative effect?

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Boiling point of pure water decreases by the addition of ethanol

Vapour pressure of pure water decreases by the addition of nitric acid

Vapour pressure of pure benzene decreases by the addition of naphthalene

Boiling point of pure benzene increases by the addition of toluene

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

The boiling point of an a zeotropic mixture of water and ethye alcohol is less than that of water and alcohol. The mixture shows

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That solution is highly saturated

No deviation from Raoult's law

Positive deviation from Raoult's law

Negative deviation from Raoult's law

Which one of the following is used as antifreeze in the radiator

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Methanol

Ethanol

Ethylene glycol

Glycerin

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

Which of the following half molar solutions will have lowest freezing point

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Solution of non-volatile, none electrolyte

Solution of non volatile, weak electrolyte

Solution of non volatile strong electrolyte

Solution of volatile, non electrolyte

A Solution containing 6.8 g of non-ionic solute in 100g of water was found to freeze at -0.93°C. If k_rfor water is 1.86 and molecular mars of solute is

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13.6

34

68

136

The depression of freezing point is directly proportional to

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Mole fraction of the solution

Molarity of the solution

Molality of the solution

Molarity of the solvent

The freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water in

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-1.86°C

-3.72°C

+1.86°C

+3.72°C

A solution contains 1.2046 x 10²⁴hydrochloric acid molecules in one dm³of the solution. The strength of the solution is

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6 N

2 N

4 N

8 N

What is the molarity of a solution containing 15.0 g urea in 500 cm³of solution

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0.5 M

1 M

1.5 M

2 M

50 cm³of 0.05 molar nrea (N₂H₄CO) solution has % W/N concentration

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6%

3%

0.3 %

0.6 %

Solution which distill without change in composition or temperature are called

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Amorphous

Azeotropic mixture

Ideal

Super saturated

A solution of two component is called

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Binary solution

Dilute solution

Original solution

Standard solution

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

The molarity of solution containing 14.5 grams urea (N₂H₄CO) dissolved in 100 cm³of the solution is

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1 molar

0.1 molar

0.2 molar

0.25 molar

Solubility cure of Na₂SO₄10H₂shows

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Constant increase of solubility

Constant decreases of solubility

Discontinuously solubility wit temperature

None of above

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

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