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Solutions and Concentration Review

Total questions: 202

Worksheet time: 5hrs 47mins

Name
Class
Date
1.
What is a "homogeneous mixture of two or more substances in a single phase"?
a)
Solution
b)
Solvent
c)
Solute
d)
Compound
2.
What is the universal solvent?
a)
salt
b)
sugar
c)
water
d)
ice
3.

A mixture with more solute dissolved in the solvent than is usually soluble is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

4.

When you have added as much solute as can dissolve in the solvent, the solution is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

5.

Which of the following is NOT a unit used to express concentration?

a)

Molality

b)

Molarity

c)

Mass percent

d)

Density

6.

The moles of solute can be determined by multiplying the molarity of the solute by the volume of solvent.

a)

True

b)

False

7.

The formula M1V1 = M2V2 is used when:

a)

dissolving a solute in a solvent

b)

diluting a solution

c)

reacting an acid with a base

d)

determining the pH of an acid

8.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
9.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
10.

How does a solution become supersaturated?

a)

Vigorous stirring to dissolve more solute than usual.

b)

Heat the solution to increase the solute then let it cool.

c)

Add more solvent to lower the concentration.

d)

Keep pouring solute in the solvent until it goes in.

11.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
12.
When 20 grams of KNO3 is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
13.
The amount of solute actually dissolved in a given amount of solvent.
a)
dilution
b)
concentration
c)
saturated solution
d)
supersaturated mixture
14.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspensions
c)
Heterogeneous Mixtures
d)
Pure Substances
15.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
16.
What is a "homogeneous mixture of two or more substances in a single phase"?
a)
Solution
b)
Solvent
c)
Solute
d)
Compound
17.
What does it mean to be "Soluble" ?
a)
Capable of being a solid.
b)
To have soul.
c)
Capable of being dissolved.
d)
To sink.
18.
Which of the following are considered to be a homogeneous mixture?
a)
Colloid
b)
Solution
c)
Suspension
d)
All Mixtures
19.
What is the unit for molarity?
a)
mass/liters
b)
moles
c)
liters
d)
moles/liter
20.
A measure of the amount of solute in a given amount of solvent or solution is...
a)
saturated
b)
solubility
c)
concentration
d)
miscible
21.
A saturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
22.
A supersaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
23.
An unsaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
24.
An electrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
25.
The dissolving medium in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
26.
The substance dissolved in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
27.
What is the molarity of a 2 liter solution containing 5 moles of NaCl?
a)
2.5
b)
0.4
c)
2.5 moles/liter
d)
10 moles/liter
28.
How many moles of NaCl are present in 6000. ml a 1.5 M NaCl solution?
a)
9 moles NaCl
b)
9000
c)
9
d)
4000  moles NaCl
29.

The substance being dissolved is called the ________

a)

solvent

b)

solid

c)

solute

d)

solvate

30.

The process of dissolving a substance in solution

a)

solvotion

b)

salvation

c)

solvation

d)

salvution

31.

A non-electrolyte is composed of __________in solution

a)

molecules

b)

molecules and ions

c)

ions

d)

none of the above

32.

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

33.

When no more solute dissolves the solution is _________

a)

supersaturated

b)

unsaturated

c)

saturated

d)

supercalifragilisticexpialidocious

34.

Gases are more soluble at ______temps and _____pressures

a)

high, low

b)

low , high

c)

high, high

d)

low, low

35.

Molality is defined as ________ divided by _____________

a)

liters solution, mols solute

b)

mols solute, liters solvent

c)

kg solvent, mols solute

d)

mols solute, kg solvent

36.

Molarity concentration is abbreviated as _________

a)

MM.

b)

m.

c)

Mol.

d)

M.

37.

Molarity is defined as _________ divided by ___________

a)

mol, liters

b)

mol, kg

c)

kg, liters

d)

liters, kg

38.

How many mols of HCl are in 3 liters of 2.0M HCl solution?

a)

2.0

b)

1.5

c)

6.0

d)

0.66

39.

This is a type of mixture where one substance dissolves into another

a)

Solution

b)

Miscibility

c)

Compound

d)

Solubility

40.

Which is an example of a solution?

a)

Salt and Sugar

b)

Salt Water

c)

Jelly beans

d)

Concrete

41.
What type of mixture separates upon standing?
a)
Solution
b)
Alloy
c)
Colloid
d)
Suspension
42.
Which are different types of mixtures
a)
suspension
b)
solution
c)
colloid
d)
all the above
43.
A colloid is a mixture that contains undissolved particles. 
a)
True
b)
False
44.
What is the solvent in a solution of kool-aid and water?
a)
glass
b)
kool-aid
c)
water
45.
What are the two types of Mixtures
a)
Elements and Subatomic Particles
b)
Protons and Electrons
c)
Atoms and Compounds
d)
Homogenous and Heterogeneous
46.
Cookies and cream ice cream would be classified as
a)
A homogenous mixture
b)
A heterogenous mixture
c)
An element
d)
A compound
47.

Two substances have been combined physically and appear the same throughout is called a.........

a)

A homogeneous mixture

b)

A heterogeneous mixture

c)

An element

d)

A compound

48.
___________ is a combination of substances that can be physically separated. 
a)
Colloid 
b)
Mixture 
c)
Suspension 
d)
Compound 
49.
This type of mixture has particles that settle. 
a)
Suspension
b)
Colloid 
c)
Emulsion
d)
Solution 
50.

The three types of mixtures are..

a)

solutions, solutes, solvents

b)

solutions, colloids, suspensions

c)

solutions, colloids, sediments

d)

concentrates, dilutes, dissolvers

51.

A feature of a colloid is that..

a)

they are cloudy

b)

they are transparent

c)

they are colourless

d)

they have a sediment

52.

Solutions has ______________ sized particles, colloids have _________________ sized particles, and suspensions have _________________________ sized particles.

a)

small, medium, large

b)

large, medium, small

c)

medium, small, large

d)

medium, large, small

53.
A mixture in which 2 liquids are mixed so evenly that it is not possible to see the separate particles 
a)
Solute 
b)
Solution
c)
Solvent 
d)
Suspension 
54.

Fog

a)

Solution

b)

Colloid

c)

Suspension

55.

Sand in water

a)

colloid

b)

solution

c)

suspension

56.
The light is spread out by flour and water, and does not go through the mixture.  What is the mixture called.
a)
Solution
b)
Suspension
c)
Colloid
57.

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

58.

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

59.

When CaBr2 is dissolved in water, how many particles will be in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

5

60.

At the same concentration, which salt will have the largest effect on the freezing point?

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

61.

The graph above is a heating curve of water. Which number in the graph represents the process of freezing?

a)

1

b)

2

c)

3

d)

4

e)

5

62.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
63.
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
64.
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
65.

Electrolytes have a greater effect on colligative properties than nonelectrolytes do because electrolytes

a)

are volatile

b)

have higher boiling points

c)

produce fewer moles of solute particles per mole of solvent

d)

produce more moles of solute particles per mole of solvent

66.

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

67.

Using the graph above, how many grams of KCl can be dissolved in 300g of water at 40° C?

a)

30g

b)

50g

c)

120g

d)

40g

68.

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

69.

When CaBr2 is dissolved in water, how many particles will be in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

5

70.

At the same concentration, which salt will have the largest effect on the freezing point?

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

71.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
72.
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
73.
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
74.

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)

75.

Which of the following compounds will be most effective in melting the ice on the roads when the air temperature is below zero?


a)

NaI

b)

MgO

c)

KBr

d)

all will be equally effective

76.

Which solution has the highest boiling point at standard pressure?

a)

0.10 M KCl(aq)

b)

0.10 M K2O(aq)

c)

0.10 M K3Al(aq)

d)

0.10 M KF(aq)

77.

Which one of the following diagrams has the highest boiling point?

a)

1

b)

2

c)

3

d)

4

e)

5

78.

Which solution below has the highest boiling point?

a)

NaCl 1 M

b)

CaCl2 1 M

c)

C6H12O6 1 M

d)

AlCl3 1 M

79.

The freezing point of water is...

a)

100oC

b)

0oC

c)

-10oC

d)

150oC

80.

At the same concentration, which of the following will elevate (increase) boiling point the most?

a)

CH3OH

b)

C6H12O6

c)

KCl

d)

SrCl2

81.

Using the graph above, which compound would dissolve the fastest at 20° C, KCl, NaCl, KNO3, or KClO3?

a)

KCl

b)

NaCl

c)

KNO3

d)

KClO3

82.

Using the graph above, which compound would dissolve the fastest at 60° C, KCl, NaCl, KNO3, or KClO3?

a)

KCl

b)

NaCl

c)

K2Cr2O7

d)

KClO3

83.

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

a)

saturated

b)

supersaturated

c)

unsaturated

d)

suspension

84.

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

85.

Using the graph above, how many grams of KCl can be dissolved in 300g of water at 40° C?

a)

30g

b)

50g

c)

120g

d)

40g

86.

____________ 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

87.

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

a)

increase

b)

decrease

c)

stay the same

88.

Which of the following ONLY has the effect on the solubility of 'gas'?

a)

Pressure

b)

Temperature

c)

Molarity

d)

Volume

89.

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

a)

Temperature

b)

Pressure

90.

amount of solute in a given amount of solvent

a)

concentration

b)

saturated

c)

solution

d)

suspension

91.

two liquids or gases that will not dissolve in each other

a)

miscible

b)

immiscible

c)

suspension

d)

emulsion

92.

Which of these is NOT a factor that affects solvation?

a)

agitation/stirring

b)

increasing temperature

c)

increasing surface area

d)

adding dye

93.

any solution that can dissolve more solute at a given temperature

a)

saturated solution

b)

unsaturated solution

c)

supersaturated solution

d)

suspension

94.

a solution that holds more dissolved solute than is required to reach equilibrium at a given temperature

a)

supersaturated solution

b)

saturated solution

c)

unsaturated solution

d)

suspension

95.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
96.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
97.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
98.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
99.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
100.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
101.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
102.
How many grams of AgNO3 (MM = 169.87) are needed to prepare 0.125M solution in 250 mL of water? 
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
103.
Which of the following has the most NaCl (MM = 58.44)?
a)
100 mL of a 1.8 M solution
b)
50 mL of a 4.1 M solution
c)
9.35 grams
d)
1 mole
104.
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
105.
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
106.
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
107.
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
108.
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
109.
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
110.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

111.

Molar mass of NaOH is ______________________

a)

40 grams/mol

b)

50 grams/mol

c)

45 grams/mol

d)

38 grams/nol

112.

What is the molality of a solution made by dissolving 2 moles of NaOH in 400 grams of water?

a)

5 mol/kg. solvent

b)

4 mol/kg solvent

c)

3 mol/kg. solvent

d)

2.5 moles /kg solvent

113.

The elements present in sodium hydroxide are

a)

sodium oxygen and hydrogen

b)

sodium , oxygen and chlorine

c)

sodium, oxygen and boron

d)

sodium, oxygen and carbon

114.

molality is defined as ________________________

a)

the moles of solute per kilogram of solvent

b)

moles of solute per liter of solution

c)

mass of solute/ mass of solution

d)

mass of solute/ mass of solvent X 100

115.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
116.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
117.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

118.

The _____ is the thing being dissolved.

a)

solute

b)

solvent

119.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
120.

What is a solvent?

a)

The substance that does the dissolving in a solution.

b)

The substance that is being dissolved in a solution.

c)

The mixing of different substances.

d)

The process in which neutral molecules lose or gain electrons.

121.

A solution that is considered unsaturated would _____.

a)

be dark in color.

b)

have a strong scent.

c)

have a large amount of solute.

d)

have a small amount of solute.

122.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
123.

What do molarity and molality have in common?

a)

Both have "moles solute" in the numerator

b)

Both have "kg solvent" in the denominator

c)

Both have "L solution" in the denominator

d)

Both have "moles solution" in the denominator

124.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

125.

Which equation is used to find molality?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

126.

What do molarity and molality have in common?

a)

Both have "moles solute" in the numerator

b)

Both have "kg solvent" in the denominator

c)

Both have "L solution" in the denominator

d)

Both have "moles solution" in the denominator

127.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

128.

Which equation is used to find molality?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

129.

How do you convert from grams to moles?

a)

Divide by the molar mass

b)

Multiply by the molar mass

c)

Divide by Avogadro's number

d)

Multiply by Avogadro's number

130.

What are the units of molarity?

a)

M

b)

m

c)

Ml

d)

Mr

131.

What are the units of molality?

a)

M

b)

m

c)

Ml

d)

Mr

132.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

133.

Which of the following is the Dilution Formula?

a)

V1M1 = V2M2

b)

M = m/V

c)

V = mT

d)

PV = nRT

134.

A dilution is when

a)

solute is added to the volume of solution

b)

water is added to the volume of solution

c)

solute is removed from the volume of solution

d)

water is removed from the volume of solution

135.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

136.

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250.0 mL?

a)

15.9 M

b)

0.636 M

c)

0.642 M

d)

1.59 M

137.
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
138.
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
139.

If I have 340.0 mL of a 0.500 M NaBr solution, what will the concentration be if I add 560.0 mL more water to it? (Remember to use the total new volume)

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

140.

If I dilute 250 mL of 0.10 M lithium acetate solution to a volume of 750 mL, what will the concentration of this solution be?

a)

2 M

b)

0.02 M

c)

0.033 M

d)

0.08 M

141.
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
142.

125.0 mL of 2.00 M calcium hydroxide solution is diluted to a concentration of 1.50 M. How many mL of water was added to the original volume?

a)

167 mL

b)

42.0 mL

c)

93.8 mL

d)

0.0240 mL

143.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspension
c)
Colloid
d)
mixtures
144.
When a solution is saturated:
a)
No additional material will dissolve in it
b)
You need to stir it more 
c)
Two materials have combined to create a clear liquid
d)
Crystals form 
145.
Amount of solute in a given amount of solvent or solution
a)
Concentration
b)
Miscible
c)
Solute
d)
solubility
146.
Substance dissolved in a solution
a)
concentration
b)
solute
c)
solvent
d)
solution
147.
Capable of being dissolved
a)
Soluble
b)
concentration
c)
colloid
d)
molarity
148.
True or false? Insoluble means that two substances can dissolve in one another.
a)
true
b)
false
149.
amount of solute that can dissolve in a given amount of solvent at a given temperature
a)
saturated solution
b)
solubility
c)
pure substance
d)
colloid
150.
To dissolve more material in a saturated solution:
a)
Add water or boil it
b)
Shake or stir faster
c)
Evaporate it
d)
You can only add water. Boiling it won't help.
151.
A precipitate is:
a)
The solid material that forms as a product of a chemical reaction
b)
The dissolved liquid in a chemical reaction
c)
The fizzing during a chemical reaction
d)
None of these
152.
All _____ are mixtures, but not all mixtures are ______
a)
solutions; solutions
b)
solutions; saturated
c)
saturations; solutions
d)
solutions; dissolved
153.
air is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
154.
salt water is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
155.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
156.
what a solute dissolves in
a)
solvent
b)
mixture
c)
solute
157.
dissolves in the solvent
a)
solute
b)
solvent
c)
mixtures
158.
When solute dissolves into a solvent it is called a _____________.
a)
mixture
b)
solution
c)
element
159.
This type of mixture contains two or more substances that are visibly distinguishable. 
a)
homogeneous
b)
heterogeneous
c)
solution
d)
colloid
160.

A solution is.......

a)

a heterogeneous mixture

b)

a homogeneous mixture

c)

a pure substance

d)

a compound

161.

Water is known as

a)

the universal solute

b)

something you drink to stay young

c)

the universal solvent

d)

something you drink to get old

162.

A solute is........

a)

any substance that will dissolve in a solvent

b)

anysubstance that will not dissolve in a solvent

c)

the same as a solvent

d)

is always a solid

163.

How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?

a)

83 grams

b)

75 grams

c)

40 grams

d)

12 grams

164.

Which substance is MOST soluble at 0 ºC?

a)

KI

b)

NaNO3

c)

NaCl

d)

Ce2(SO4)3

165.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
166.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
167.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
168.
When 20 grams of KNO3 is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
169.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
170.

When 42 grams of potassium chloride ( KCl), is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

171.

How many grams of CaCl2, are soluble in 100 g of water at approximately 17 ºC?

a)

58 grams

b)

70 grams

c)

0 grams

d)

12 grams

172.

In a solution, the part of the mixture in which other substance are dissolved

a)

Strainer

b)

Solvent

c)

Solute

d)

Magnetism

173.

The substance which dissolved in the solvent

a)

Dissolve

b)

Solubility

c)

Solvent

d)

Solute

174.
Which of these solutes does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
175.
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 solvent in it. 
176.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Mixture
d)
Homogeneous solution
177.
Describe a solute.
a)
part of solution present in largest amount
b)
gets dissolved
c)
water
d)
surrounds and breaks apart
178.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspensions
c)
Heterogeneous Mixtures
d)
Pure Substances
179.
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
180.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
181.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
182.
What is able to dissolve other substances?
a)
Solute
b)
Salt
c)
Suspension
d)
Solvent
183.
If I dissolve sugar in water, what is the solute?
a)
Water
b)
Hydrogen
c)
Sugar
d)
Carbon
184.
If I dissolve carbon dioxide in water, what is my solvent?
a)
Carbon Dioxide
b)
There is no solvent
c)
Oxygen
d)
Water
185.

How many moles of particles (what is "i") for the substance Na2CO3?

(a)  

186.

Which of the following is a colligative property?

a)

boiling point elevation

b)

vapor pressure elevation

c)

molarity depression

d)

vapor pressure lowering

187.

Which of the following is a colligative property?

a)

boiling point stability

b)

freezing point depression

c)

molar dissociation

d)

ions dissolving

188.

What is the value of "i" for CCl4?

a)

1

b)

5

c)

3

d)

0

189.

What is the value of "i" for KNO3?

a)

1

b)

5

c)

3

d)

2

190.

An equal number of moles of NaCl and CaCl2 are dissolved in equal volumes of water. Which solution has the lower freezing point?

a)

CaCl2

b)

NaCl

c)

They are the same.

d)

No way to tell.

191.

An equal number of moles of NaCl and CaCl2 are dissolved in equal volumes of water. Which solution has the lower BOILING point?

a)

CaCl2

b)

NaCl

c)

They are the same.

d)

No way to tell.

192.
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
193.

The freezing point of a solution is ______ the freezing point of the pure solvent.

a)

higher than

b)

the same as

c)

lower than

d)

higher or lower than

194.

Colligative properties of solutions are those properties that depend on

a)

the amount of solute only

b)

the identity of solute only

c)

both the identity and the amount of solute

195.

Molality is

a)

the moles of solute in 1g of solvent

b)

the moles of solute in 1g of solution

c)

the moles of solute in 1kg of solvent

d)

the moles of solute in 1kg of solution

196.

The boiling point of a solution is ___________ that of a pure solvent

a)

more than

b)

less than

c)

equal to

197.

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

198.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
199.

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.

200.

What is the boiling point elevation of a solution of 1 molal NaCl? The Kb for water is .51 °C/m.

a)

100 °C

b)

101.2°C

c)

1.02°C

d)

-0.51°C

201.

For a 0.262 m solution of sucrose, a covalent compound, in water, calculate the boiling point of the solution. Given that Kb = 0.51

a)

0.13 oC

b)

10.13 oC

c)

90.13 oC

d)

100.13 oC

202.

When CaBr2 is dissolved in water, what is the Van't Hoff Factor?

a)

1

b)

2

c)

3

d)

4

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