chemistry MCQs - 11th class Chapter 09 Mcqs

1

The component of a solution present in a larger quantity is called the?

A

Solute

B

Solvent

C

Mixture

D

Phase

2

Which of the following concentration units is independent of temperature?

A

Molarity

B

Normality

C

Molality

D

Percentage w/v

3

The sum of the mole fractions of all components in a solution is always equal to?

A

0

B

1

C

100

D

Depends on the solution

4

A solution that obeys Raoult's law over the entire range of concentration is known as a(n)?

A

Saturated solution

B

Super-saturated solution

C

Ideal solution

D

Non-ideal solution

5

For an ideal solution, the enthalpy of mixing (ΔH_mix) is?

A

Positive

B

Negative

C

Zero

D

Always greater than 1

6

A mixture of ethanol and water is an example of a solution that shows?

A

Ideal behavior

B

Positive deviation

C

Negative deviation

D

No deviation

7

Azeotropic mixtures are liquid mixtures that?

A

Boil over a range of temperatures

B

Can be separated by fractional distillation

C

Boil at a constant temperature

D

Are always ideal

8

The solubility principle 'like dissolves like' refers to the fact that?

A

Polar solutes dissolve in non-polar solvents

B

Non-polar solutes dissolve in polar solvents

C

Polar solutes dissolve in polar solvents

D

All solutes dissolve in water

9

The critical solution temperature (or upper consulate temperature) for the phenol-water system is?

A

25.9°C

B

100°C

C

49.1°C

D

65.9°C

10

Which of the following is NOT a colligative property?

A

Lowering of vapour pressure

B

Elevation of boiling point

C

Refractive index

D

Depression of freezing point

11

Colligative properties of a solution depend primarily on the?

A

Nature of the solute

B

Nature of the solvent

C

Number of solute particles

D

Color of the solution

12

The ebullioscopic constant (Kb) is a property of the?

A

Solute

B

Solvent

C

Solution

D

Apparatus

13

The antifreeze used in car radiators, ethylene glycol, works by?

A

Increasing the freezing point and decreasing the boiling point

B

Lowering both the freezing and boiling points

C

Raising both the freezing and boiling points

D

Lowering the freezing point and raising the boiling point

14

A dissolution process that absorbs heat from the surroundings is called?

A

Exothermic

B

Isothermic

C

Endothermic

D

Adiabatic

15

The energy required to break the crystal lattice of an ionic solid into gaseous ions is called?

A

Hydration energy

B

Solution energy

C

Lattice energy

D

Kinetic energy

16

The process in which water molecules surround and interact with solute ions is known as?

A

Hydrolysis

B

Hydration

C

Crystallization

D

Precipitation

17

A solution of ammonium chloride (NH4Cl) in water will be?

A

Acidic

B

Basic

C

Neutral

D

Amphoteric

18

The molarity of pure water is approximately?

A

1 M

B

18 M

C

55.5 M

D

100 M

19

The relative lowering of vapour pressure is equal to the?

A

Mole fraction of the solvent

B

Mole fraction of the solute

C

Molality of the solution

D

Molarity of the solution

20

A solution showing negative deviation from Raoult's law will have a vapour pressure that is?

A

Higher than expected

B

Lower than expected

C

Equal to the expected value

D

Zero

21

Metal alloys like brass and steel are examples of?

A

Liquid in solid solutions

B

Solid in solid solutions

C

Gas in solid solutions

D

Liquid in liquid solutions

22

Beckmann's thermometer is specially designed to measure?

A

High temperatures

B

Low temperatures

C

Small temperature changes

D

Atmospheric pressure

23

The hydrolysis of a salt of a strong acid and a strong base, like NaCl, results in a solution that is?

A

Acidic

B

Basic

C

Neutral

D

A buffer

24

In the hydrate CuSO4.5H2O, how many water molecules are directly attached to the Cu(II) ion?

A

1

B

2

C

4

D

5

25

The heat of solution for LiCl is -35.0 kJ/mol, which indicates its dissolution in water is?

A

Endothermic

B

Exothermic

C

Isenthalpic

D

Slow

26

Landsberger's method is used for the experimental determination of?

A

Molar mass

B

Depression of freezing point

C

Elevation of boiling point

D

Vapour pressure

27

Solutions that do not distill with a change in composition are called?

A

Zeotropic mixtures

B

Azeotropic mixtures

C

Ideal mixtures

D

Saturated mixtures

28

Percentage weight/volume is defined as?

A

Grams of solute per 100 cm³ of solvent

B

Grams of solute per 100 g of solution

C

Grams of solute per 100 cm³ of solution

D

cm³ of solute per 100 cm³ of solution

29

Which of the following solutions would have the highest boiling point?

A

0.1 m glucose

B

0.1 m NaCl

C

0.1 m CaCl2

D

0.1 m urea

30

The hydration energy of an ion increases with?

A

Increasing ionic size and decreasing charge

B

Decreasing ionic size and decreasing charge

C

Increasing ionic size and increasing charge

D

Decreasing ionic size and increasing charge

31

The solubility of cerium(III) sulfate, Ce2(SO4)3, in water?

A

Increases with temperature

B

Decreases with temperature

C

Remains constant with temperature

D

First increases then decreases

32

The unit ppm stands for?

A

Parts per mole

B

Parts per million

C

Pressure per molecule

D

Purity per mass

33

A solution containing less solute than required for saturation is called?

A

Dilute

B

Concentrated

C

Unsaturated

D

Supersaturated

34

The process of separating components from a liquid mixture based on differences in boiling points is called?

A

Fractional crystallization

B

Fractional distillation

C

Chromatography

D

Solvent extraction

35

According to Raoult's law, p = p°x1, what does x1 represent?

A

Mole fraction of solute

B

Mole fraction of solvent

C

Molality

D

Vapour pressure of solution

36

Mist and fog are examples of what type of solution?

A

Gas in liquid

B

Liquid in gas

C

Solid in gas

D

Gas in solid

37

Conjugate solutions are formed in the case of?

A

Completely miscible liquids

B

Immiscible liquids

C

Partially miscible liquids

D

Solid in liquid solutions

38

The number of moles of solute dissolved per dm³ of solution is?

A

Molality

B

Molarity

C

Normality

D

Mole fraction

39

The boiling point of an azeotropic mixture showing positive deviation is?

A

Higher than both components

B

Lower than both components

C

In between the two components

D

Equal to the higher boiling component

40

What happens to the total volume when two liquids form a non-ideal solution with positive deviation?

A

It decreases

B

It increases

C

It remains the same

D

It becomes zero

41

The cryoscopic constant (Kf) is also known as the?

A

Molal elevation constant

B

Ebullioscopic constant

C

Gas constant

D

Molal depression constant

42

The addition of NaCl or KNO3 to ice is used to?

A

Increase its melting point

B

Lower its melting point

C

Purify the ice

D

Make it boil faster

43

A solution of sugar in water is an example of a?

A

Binary solution

B

Ternary solution

C

Ionic solution

D

Gaseous solution

44

Which percentage composition is defined as the weight of solute per 100 parts by weight of solution?

A

w/v

B

v/v

C

w/w

D

v/w

45

A 10% v/w solution of alcohol in water means?

A

10 cm³ of alcohol in 100 cm³ of water

B

10 g of alcohol in 100 g of solution

C

10 cm³ of alcohol in 100 g of solution

D

10 cm³ of alcohol in 100 cm³ of solution

46

In a solution having 2 moles of A and 3 moles of B, the mole fraction of A is?

A

0.2

B

0.3

C

0.4

D

0.6

47

The value of concentration given in molality does not change with temperature because?

A

Volume is not involved in the expression

B

Mass is independent of temperature

C

Moles are independent of temperature

D

Both B and C

48

Which of the following is an example of a solid aerosol (solid in gas solution)?

A

Smoke

B

Fog

C

Milk

D

Paint

49

Water and benzene are examples of liquids that are?

A

Completely miscible

B

Partially miscible

C

Practically immiscible

D

Ideal partners

50

A solution of hydrochloric acid in water (20.24% HCl) boils at 110°C. This is an example of a(n)?

A

Ideal solution

B

Zeotropic mixture

C

Minimum boiling azeotrope

D

Maximum boiling azeotrope