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114 Honors Solutions Test Review

Total questions: 60

Worksheet time: 4hrs 29mins

Name
Class
Date
1.

Which solute is MOST likely a gas?

a)

KNO3

b)

NaNO3

c)

KCl

d)

Ce2(SO4)3

2.

In general as temperature decreases, the solubility...

a)

increases

b)

decreases

c)

stays the same

3.
When a solvent contains as much of the solute as it can hold, the solution is said to be
a)
supersaturated
b)
diluted
c)
saturated
d)
unsaturated
4.
Which is an example of a solute?
a)
Egg whites
b)
Sugar
c)
Water
d)
Acetone
5.
What is a solvent
a)
the liquid in which a solute is dissolved to form a solution.
b)
Another word for solution
c)
A thing that make drinks turn colors
d)
Its a metal molecole
6.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
7.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
8.
mixture of two or more substances; dissolved particles are spread evenly throughout the mixture
a)
solvent
b)
solute
c)
mixture
d)
solution
9.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Supersaturated
d)
Homogeneous solution
10.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
11.
What does the solute dissolve in?
a)
solvent
b)
mixture
c)
solute
12.

True or False: Molarity can be determined by knowing either the number of moles OR the volume of the solution alone.

a)

True

b)

False

13.

Calculate the molarity of a solution containing 1.5 moles of NaCl in 0.5 L of solution

a)

1.5

b)

0.33 M

c)

30 M

d)

3 M

14.
How does a solution become supersaturated?
a)
dissolve lots of solute in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 
15.

a solution in which more solute can be added and dissolved; below the maximum amount of solute

a)

saturated

b)

unsaturated

c)

supersaturated

16.
In a solution which of the following is the solvent?
a)
sugar
b)
water
c)
salt
d)
carbon dioxide
17.
Which of the following would dissolve the slowest?
a)
a sugar cube in hot water
b)
a sugar cube in cool water
c)
powdered sugar in cool water
d)
powdered sugar in hot water
18.
Which cube(s) has the most surface area?
a)
left cube
b)
middle cubes
c)
right cubes
19.
What type of solution is holds more than the maximum amount of solute when it is rapidly heated & then cooled slowly producing crystals?
a)
unsaturated 
b)
saturated 
c)
supersaturated 
20.

Which factor affecting solubility is shown in the picture?

a)

temperature

b)

height

c)

stirring

d)

particle size

21.

Which factor is shown in the picture?

a)

temperature

b)

particle size

c)

stirring

d)

use of spoon

22.

Why do sugar particles dissolve faster in hot water?

a)

water particles move slow

b)

water particles move fast

c)

water particles settle down

d)

water particles stay on top

23.

How does particle size affect solubility?

a)

bigger particles dissolve faster

b)

smaller particles can occupy the space in water faster

c)

bigger particles spread faster than smaller particles

24.

What are the factors that affect solubility?

a)

rate of stirring

b)

particle size

c)

temperature

d)

all of these

25.

Which of the following does not affect solubility of solutes?

a)

Tempearture

b)

Color

c)

Size particles

d)

Kind of solute

26.

Two liquids that can be mixed together but separate shortly after are:

a)

immiscible

b)

insoluble

c)

miscible

d)

soluble

27.

Two liquid substances that are soluble in each other in any proportion are said to be:

a)

insoluble

b)

immiscible

c)

miscible

d)

soluble

28.
a solute whose water solution conducts electricity is called a(n)
a)
nonconductor
b)
electrolyte
c)
nonelectrolyte
d)
aqueous solution
29.
Solutions in which electric currents cannot run through are said to be
a)
noncolloidal
b)
electrolytes
c)
nonelectrolytes
d)
conductors
30.
An example of a nonelectrolyte is
a)
sugar water
b)
salt water
c)
sodium chloride
d)
hydrogen chloride
31.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
32.
What is the formula for molarity?
a)
moles/grams
b)
moles/kilograms
c)
moles/milliliters
d)
moles/liters
33.
How many L are required to make 3.5 M hydrochloric acid using 1.1 moles? 
a)
3.18 L
b)
0.31 L
c)
3.85 L
d)
4.6 L
34.
If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
a)
20.9 mol
b)
0.021 mol
c)
0.02 mol
d)
0.0209 mol
35.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
36.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
37.
Calculate the molarity of the following solution:  1.0 mole of KCl in 750.0 mL of solution.
a)
0.750 M
b)
99 M
c)
1.3 M
d)
2.0 M
38.
What volume of 1.50 M KBr can be made from 15.6 mL of concentrated KBr with a molarity of 9.65 M?
a)
150. mL
b)
151 mL
c)
1.00 L
d)
100. mL
39.
What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M
40.
How many moles are needed to make 2.5 L of a 3.8 M solution? 
a)
9.5 mol
b)
0.66 mol
c)
1.5 mol
d)
15 mol
41.
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
42.
Colligative properties depend on the _________ of the solute but not the __________ of the solute.
a)
 concentration; identity
b)
identity; concentration
c)
reactivity; nature
d)
nature; reactivity
43.

Which salt below has the largest effect on freezing point?

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

44.
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
45.
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
46.

The vapor pressure of a pure solvent is ___________ that of a solution

a)

more than

b)

less than

c)

equal to

47.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
48.

Which of the following is a colligative property

a)

vapor pressure elevation

b)

vapor pressure lowering

c)

pressure

d)

boiling point depresssion

49.

When CH3OH is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

3

c)

4

d)

5

e)

6

50.

When KCl (potassium chloride) is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

6

51.

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

a)

1

b)

2

c)

3

d)

4

e)

5

52.

The vapor pressure of a pure solvent is ___________ that of a solution

a)

more than

b)

less than

c)

equal to

53.

While making homemade ice cream, you add rock salt to the ice. Which choice below provides the best explanation for why this is done?

a)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is lower than just the ice.

b)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is higher than just the ice.

c)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is lower than just the ice.

d)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is higher than just the ice.

54.

Which solute is the most soluble at 10 ⁰C?

a)

KI

b)

NH3

c)

KClO3

d)

NH4Cl

55.

John dissolves 54 grams of a solute in a solution he has gently heated near boiling. After a couple of hours he checks the temperature and finds that only 48 grams of solute should dissolve at the present temperature. The solution appears normal otherwise. What type of solution has John made?

a)

unsaturated

b)

saturated

c)

super saturated

d)

unable to determine

56.

How many grams of SO2 can dissolve at 50 ⁰C?

a)

5 g

b)

10 g

c)

20 g

d)

39 g

57.

How would you describe a solution where the plotted point falls below the line on a solubility curve?

a)

saturated

b)

unsaturated

c)

super saturated

58.

Which type of concentration can forms crystals?

a)

saturated

b)

unsaturated

c)

supersaturated

59.

Engine cooolant, also known as antifreeze, is mixture with mixture in the radiator of car. Why is the coolant added to the water?

a)

All of these.

b)

It lowers the concentration of water in the radiator.

c)

It raises the boiling point of water in the radiator.

d)

It lowers the freezing point of water in the radiator.

60.

the minimum amount of pressure required to nullify process of osmosis is called...?

a)

permeable pressure

b)

osmotic pressure

c)

concentration of pressure

d)

surface pressure

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