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Chapter 12 Review - Colligative Properties

Total questions: 57

Worksheet time: 31mins

Name
Class
Date
1.

At the same concentration, which salt will have the largest effect on the freezing point? Remember the bigger the i value.... the more you multiply in the formula

 ΔTf = − i Kf m\Delta T_{f\ }=\ -\ i\ K_{f\ }m  

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

2.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
3.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
4.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
5.

Using the graph above, which compound would dissolve the most at 60° C, KCl, NaCl, or KClO3?

a)

KCl

b)

NaCl

c)

KClO3

6.

Using the graph above, solubility of which compound is influenced the most by changes in temperature?

a)

KCl

b)

NaCl

c)

K2Cr2O7

d)

KClO3

7.

A solution that has the maximum amount of solute dissolved in the solvent is called __________________.

a)

saturated

b)

supersaturated

c)

unsaturated

d)

suspension

8.

A solution that has less than the maximum amount of solute dissolved in the solvent is called __________________.

a)

saturated

b)

supersaturated

c)

unsaturated

d)

suspension

9.

Using the graph above, how many grams of KCl can be dissolved in 300g of water at 40° C? (Notice that the graph gives you amounts dissolves in 100 g of water.) (Because the graph says 100g and this asks for 300g you need to mulitply by 3.)

a)

30g

b)

50g

c)

120g

d)

40g

10.

A solution that has more than the maximum amount of solute dissolved in the solvent is called __________________.

a)

saturated

b)

supersaturated

c)

unsaturated

d)

suspension

11.

Dry air contains 78.09% nitrogen, 20.95% oxygen, 0.93% argon, 0.04% and carbon dioxide. What is the solvent in the solution we call air?

a)

nitrogen

b)

oxygen

c)

argon

d)

carbon dioxide

12.

Chloroform (CHCl3) and water


Like dissolves like!

a)

Soluble (miscible) CHCl3 is polar

b)

Insoluble (immiscible) CHCl3 is not polar

13.

Octane (C8H18) and water


Polar dissolves polar or ionic and non-polar dissolves non-polar

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

14.

NaCl in water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

15.

NaCl in hexane (C6H14)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

16.

Atoms of a polar molecule share their atoms ___________.

a)

Equally

b)

Unequally

17.

Polar molecules will dissolve in other polar molecules and nonpolar molecules will dissolve in other nonpolar molecules.

a)

True

b)

False

18.

Polar molecules have

a)

no charges.

b)

slight positive and negative charges on opposite ends of the molecules.

c)

only positive charges.

d)

either positive or negative charges, but not both.

19.

Why is it difficult to wash oil from your hands with plain water?

a)

Both substances are polar. Like polarities repel.

b)

Both substances are nonpolar. Like polarities repel.

c)

Water is nonpolar, and oil is polar, so they will not combine.

d)

Water is polar, and oil is nonpolar, so they will not combine.

20.

Why is the molecule nonpolar?

a)

There are nonbonding pairs on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

21.

Why is the molecule polar?

a)

There are nonbonding pairs on the central atom and it creates the bent shape.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

22.

Why is the molecule polar?

a)

There is a nonbonding pair on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

23.

Classify the following molecule.

a)

polar

b)

nonpolar

24.

Name the effect

a)

brownian

b)

tyndall

c)

suspension

d)

colloidal

25.

Which one is not a colloid

a)

Foam

b)

Gel

c)

Emulsion

d)

Coffee

26.

A snow globe would be an example of a __________________.

a)

colloid

b)

solution

c)

suspension

27.

Milk is an example of a

a)

solution

b)

colloid

c)

suspension

d)

solid

28.
Which are different types of mixtures
a)
suspension
b)
solution
c)
colloid
d)
all the above
29.

Which of the following appear to be clear (are not cloudy)?

a)

Solution

b)

Suspension

c)

Colloid

30.

The process in which a solvent moves across a semipermeable membrane.

a)

osmosis

b)

dissolving

c)

effusion

31.

Is a colloid a solution?

a)

No, it is a mixture that contains small particles dispersed in a medium.

b)

Yes, because you can mix it with something.

32.

Which contains the largest particles?

a)

solution

b)

colloid

c)

suspension

33.

When two liquids mix to form a homogeneous solution

a)

solvation

b)

Miscible

c)

Immiscible

d)

Amalgam

34.

Octane (C8H18) and water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

35.

Ethanol (CH3CH2OH) and water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

36.

A mixture of medium-sized particles that do not settle out of solution is known as

a)

Miscible

b)

Immiscible

c)

Colloids

d)

Suspensions

37.

Which of the following terms is the substance that does the dissolving in solution

a)

Miscible

b)

Immiscible

c)

Solute

d)

Solvent

38.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

39.
Capable of being dissolved
a)
Soluble
b)
concentration
c)
colloid
d)
molarity
40.

____________ is the process whereby particles of a solvent completely surround the particles of a solute, disperse them throughout the solvent particles, and hold them in solution.

a)

solvation

b)

immisciblation

c)

dissolution

d)

saturation

41.

Which one of the following should be increased in order to increase the solubility of a gas?

a)

Temperature

b)

Pressure

42.

amount of solute in a given amount of solvent

a)

concentration

b)

saturated

c)

solution

d)

suspension

43.

any solution that can dissolve more solute at a given temperature

a)

saturated solution

b)

unsaturated solution

c)

supersaturated solution

d)

suspension

44.

As you put in more solute in the solution, the concentration of the solution will...

a)

increase

b)

decrease

c)

stay the same

45.

The separation of ions that occurs when an ionic compound dissolves is

a)

ionization

b)

dissociation

c)

electronegativity

d)

spectation

46.

They process in which ions are formed from molecules when they are dissolved in solution.

a)

dissociation

b)

ionization

c)

spetation

d)

electronegativity

47.

Which of the following would result in being able to dissolve a greater amount of solid in a solution?

a)

Lower the temperature.

b)

Decrease the pressure of the solution.

c)

Increase the pressure of the solution.

d)

Heat the solution.

48.

Which of the following would result in being able to dissolve a greater amount of gas in a solution?

a)

Lower the temperature of the solution.

b)

Decrease the pressure of the solution.

c)

Stir the solution.

d)

Heat the solution.

49.

Which of the following statements is true?

a)

An increase in temperature decreases the solubility of most solids, but increases the solubility of gases.

b)

An increase in temperature increases the solubility of most solids and gases.

c)

An increase in temperature decreases the solubility of most solids and gases.

d)

An increase in temperature increases the solubility of most solids, but decreases the solubility of gases.

50.

Which of the following would increase the rate of dissolution of a solid?

a)

Cool the solid solute and the solution.

b)

Shake the solution.

c)

Evaporate the solvent.

d)

Break the solvent into smaller particles.

51.

What is known as the universal solvent?

a)

water

b)

acetone

c)

vinegar

d)

soy sauce

52.

Which factor is shown in the picture?

a)

temperature

b)

particle size

c)

stirring

d)

use of spoon

53.

What are the factors that affect solubility?

a)

rate of stirring

b)

particle size

c)

temperature

d)

all of these

54.
Stirring the solution increases or decreases the solubility?
a)
increases
b)
decreases
55.

Which one of the following diagrams has the lowest vapor pressure?

a)

1

b)

2

c)

3

d)

4

e)

5

56.

Which of the following solutions will have the lowest freezing point?

a)

1.0 mol/L sucrose (C12H22O11)

b)

1.0 mol/L lithium chloride (LiCl)

c)

1.0 mol/L sodium phosphide (Na3P)

d)

1.0 mol/L magnesium fluoride (MgF2)

57.

Which sample, when dissolved in 1.0 liter of water, produces a solution with the lowest freezing point?

a)

0.1 mol of C2H5OH

b)

0.1 mol of LiBr

c)

0.2 mol of C6H12O6

d)

0.2 mol of CaCl2

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