wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Unit 6 Review

Total questions: 102

Worksheet time: 2hrs 45mins

Name
Class
Date
1.
What is the phase change of a solid to a liquid?
a)
freezing
b)
melting
c)
boiling
d)
condensation
2.
All changes in the state of matter of a substance requires
a)
vibration
b)
water
c)
permission
d)
energy
3.
What happens to particles when they are heated?
a)
They speed up and spread out
b)
They slow down and compress
c)
They stop moving
d)
They move closer together and speed up
4.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
5.

Which state of matter is shown?

a)

solid

b)

liquid

c)

gas

6.

The phase change from liquid to gas is _________

a)

Melting

b)

Evaporation

c)

Deposition

d)

Condensation

7.

Phase change from liquid to solid is ___________.

a)

Freezing

b)

Melting

c)

Sublimation

d)

Condensation

8.

Phase change going from a Gas to a Solid...

a)

Deposition

b)

Sublimation

c)

Condensation

d)

Vaporization

9.
What type of reaction occurs in a hand warmer
a)
exothermic
b)
endothermic
10.
Exothermic reactions...
a)
Absorb energy
b)
Release energy
c)
Release Color
d)
Absorb Color
11.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
12.

____ reactions usually feel cold.

a)

endothermic

b)

exothermic

13.

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

a)

Solution

b)

Miscibility

c)

Compound

d)

Solubility

14.

The substance that does the dissolving

a)

Solute

b)

Solvent

c)

Solution

d)

Miscibility

15.

The substance getting dissolved

a)

Solvent

b)

Solute

c)

Solution

d)

Mixture

16.
Which substance is SOLUBLE in water?
a)
sand
b)
oil
c)
salt (sodium chloride)
d)
sulfur
17.
Which substance is INSOLUBLE in water?
a)
salt (sodium chloride)
b)
sugar (sucrose)
c)
oil
d)
copper sulfate
18.
Contains the maximum amount of dissolved solute
a)
unsaturated solution
b)
supersaturated solution
c)
saturated solution
19.

Kool-Aid - flavoring, coloring, sugar, and water. Identify the solvent.

a)

water

b)

powder

c)

sugar

d)

powder and sugar

20.

Which sweet tea would you expect to taste the sweetest?

a)

1M

b)

3M

c)

5 M

d)

2.5M

21.

What is molarity?

a)

a concentration unit, defined to be number of atoms per moles of water

b)

a concentration unit, defined to be the number of moles of solute divided by the number of liters of solution.

c)

a conversion factor, used to change moles to grams

d)

a conversion factor, used to change milliliters to liters

22.

At 30'C, which substance has the lowest solubility?

a)

KNO3

b)

KBr

c)

NaCl

d)

Yb2(SO4)3

23.
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. 
24.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
25.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

26.

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

27.
What is a "homogeneous mixture of two or more substances in a single phase"?
a)
Solution
b)
Solvent
c)
Solute
d)
Compound
28.

Particles are very small, can pass through filter paper, looks the same throughout, doesn’t settle

a)

Suspension

b)

Colloid

c)

Solution

d)

Element

29.

Mixture consisting of particles that are in between the size of solutions and suspensions, cannot be filtered, includes foams and gels

a)

Suspension

b)

Colloid

c)

Solution

d)

Element

30.

A mixture in which the particles are so large that they settle unless stirred, can be filtered

a)

Suspension

b)

Colloid

c)

Solution

d)

Element

31.

Orange juice with pulp and Italian dressing are each an example of

a)

Suspension

b)

Colloid

c)

Solution

d)

Element

32.

A marshmallow is an example of

a)

Suspension

b)

Colloid

c)

Solution

d)

Element

33.

Milk and mayo are each an example of

a)

Suspension

b)

Colloid

c)

Solution

d)

Element

34.

Paint and jello are each an example of

a)

Suspension

b)

Colloid

c)

Solution

d)

Element

35.
What type of mixture separates upon standing?
a)
Solution
b)
Alloy
c)
Colloid
d)
Suspension
36.

This type of mixture that doesn't separate on its own but still contains undissolved particles.

a)
solution
b)
colloid
c)
suspension
37.

Solutions are

a)

Homogenous

b)

Heterogenous

38.
What state of matter is X?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
39.
What state of matter is Y?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
40.
What state of matter is Z?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
41.
What is point B?
a)
triple point
b)
critical point
c)
equilibrium point
d)
normal melting point
42.
What change occurs from F to E?
a)
sublimation
b)
deposition
c)
melting
d)
condensation
43.
What change occurs from E to C?
a)
sublimation
b)
freezing
c)
melting
d)
boiling
44.
What change occurs from C to D?
a)
condensation
b)
vaporization
c)
melting
d)
sublimation
45.
What is the normal boiling point of this substance?
a)
150 °C
b)
100 °C
c)
-50 °C
d)
0 °C
46.
What is the normal melting point of this substance?
a)
150 °C
b)
100 °C
c)
-50 °C
d)
0 °C
47.

The temperature and pressure at which the gas and liquid states of a substance become identical and form one phase is called the

a)

Critical point

b)

Triple point

c)

Melting point

d)

Boiling point

48.

Using the supplied solubility curve diagram, determine the temperature at which KNO3 and NH4Cl have the same solubility.

a)

16°C

b)

39°C

c)

25°C

d)

73°C

49.

Using the supplied solubility curve diagram, determine what type of solution would be present if 50 grams of NH3 was dissolved in 100 grams of water at 30°C.

a)

saturated

b)

unsaturated

c)

supersaturated

50.

Using the supplied solubility curve diagram, determine which compound listed below is least soluble at 70°C.

a)

NH4Cl

b)

NaCl

c)

KCl

d)

KNO3

51.

Using the supplied solubility curve, determine the temperature that Ce2(SO4)3 and KClO3 have the same solubility.

a)

26°C

b)

3°C

c)

57°C

d)

80°C

52.

Using the supplied solubility curve, determine the type of solution that is formed if 80 grams of NaNO3 were dissolved in 100 grams of water at 30°C.

a)

saturated

b)

unsaturated

c)

supersaturated

53.

Using the supplied solubility curve, determine which compound listed below is most soluble at 20°C.

a)

NH3

b)

KCl

c)

KClO3

d)

NaNO3

54.

Using the supplied solubility curve, determine the type of solution formed if 10 grams of Ce2(SO4)3 were dissolved in 100 grams of water at 50°C.

a)

saturated

b)

unsaturated

c)

supersaturated

55.

Using the supplied solubility curve, determine how many grams of KNO3 will need to be dissolved in 100 grams of water at 60°C to make a saturated solution.

a)

103 grams

b)

85 grams

c)

124 grams

d)

140 grams

56.

Using the supplied solubility curve, determine the type of solution formed when 60 grams of NH4Cl are dissolved in 100 grams of water at 80°C.

a)

saturated

b)

unsaturated

c)

supersaturated

57.

The the supplied solubility curve shows that when 79 grams of NaNO3 is dissolved in 100 grams of water at 10°C, that a saturated solution will be formed.

a)

True

b)

False

58.

Develop a model to illustrate the process of dissolving table salt (NaCl) in water. Explain the roles of solvation and dissociation in this process.

a)

Solvation involves the breaking of ionic bonds in NaCl, while dissociation involves the formation of new covalent bonds with water molecules.

b)

Solvation involves water molecules surrounding Na+ and Cl- ions, while dissociation involves the separation of NaCl into Na+ and Cl- ions.

c)

Solvation involves the evaporation of water, while dissociation involves the condensation of NaCl.

d)

Solvation and dissociation both involve the formation of a new compound between NaCl and water.

59.

Calculate the molarity of a solution made by dissolving 5 moles of solute in 2 liters of solution.

a)

2.5 M

b)

5 M

c)

10 M

d)

2 M

60.

Communicate the steps required to prepare a 1 M solution of NaCl, including how to properly label the solution.

a)

Dissolve 58.44 g of NaCl in 1 L of water, label the solution as "1 M NaCl Solution."

b)

Dissolve 100 g of NaCl in 1 L of water, label the solution as "1 M NaCl Solution."

c)

Dissolve 58.44 g of NaCl in 500 mL of water, label the solution as "1 M NaCl Solution."

d)

Dissolve 100 g of NaCl in 500 mL of water, label the solution as "1 M NaCl Solution."

61.

Explain how you would use evidence to determine whether a solute dissociates or merely dissolves in a solvent.

a)

Measure the change in temperature of the solution.

b)

Observe the color change of the solution.

c)

Conduct an electrical conductivity test to see if ions are present in the solution.

d)

Measure the pH of the solution.

62.

What 2 ions appear on both sides of the equation?

Na+ (aq) + Cl- (aq) + Ag + (aq) + (NO3)+ (aq)→Na+ (aq) + (NO3) + AgCl(s)

a)

Ag and NO3

b)

Na and Cl

c)

Na and NO3

d)

Ag and Cl

63.

Write the chemical equation that represents the dissociation of the ionic compound Na2(SO4) .

a)

Na+2 + (SO4)-1

b)

Na+1 + (SO4)-1

c)

Na+2 + (SO4)-4

d)

Na+1 + (SO4)-2

64.

Which of the following shows the correct disassociation of the reaction for BaCl2?

a)

Ba 2+ (aq) + Cl2 - (aq) -> BaCl2 (s)

b)

Ba 2+ (aq) + 2 Cl - (aq) -> BaCl2 (s)

c)

BaCl2 (aq) -> Ba 2+ (aq) + 2 Cl - (aq)

d)

BaCl2(s) -> Ba 2+(aq)+ 2Cl (aq)

65.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
66.

Define: Net Ionic Equation

a)

a balanced chemical equation in which all the reactants and products are given by their chemical formulae.

b)

a chemical equation that shows all soluble species broken into their respective ions.

c)

a chemical equation showing only the species which are actively involved in the reaction.

67.

What is the net ionic equation for the reaction between K3PO4 (aq) and CuSO4 (aq)

a)

2 K+(aq) + SO42-(aq) → K2SO4 (s)

b)

K+(aq) + SO42-(aq) → KSO4 (s)

c)

2 Cu2+(aq) + 3 PO43-(aq) → Cu3(PO4)2 (s)

d)

Cu2+(aq) + PO43-(aq) → CuPO4 (s)

68.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
69.

Identify the correct net ionic equation for the reaction of AgNO3 and CaCl2?

a)

Ca2+(aq) + 2Cl- (aq) → CaCl(s)

b)

Ag+(aq) + Cl- (aq) → AgCl(s)

c)

Ag + Cl → AgCl

d)

Ag+ + Ca2+ →Ag2Ca (s)

70.

Define: Solubility

a)

What is dissolved

b)

What does the dissolving

c)

A measure of how much solute can dissolve in solvent

d)

a charged ion

71.

What is the correct net ionic equation for the reaction between HBr(aq) and LiOH(aq)?

a)

2 H+(aq) + O2-(aq) → H2O(l)

b)

2 H2 (aq) + O2(aq) → 2 H2O(l)

c)

2 H2 (g) + O2(g) → 2 H2O(l)

d)

H+(aq) + OH-(aq) → H2O(l)

72.

What is the net ionic equation for the reaction between K3PO4 (aq) and CuSO4 (aq)

a)

2 K+(aq) + SO42-(aq) → K2SO4 (s)

b)

K+(aq) + SO42-(aq) → KSO4 (s)

c)

3 Cu2+(aq) + 2 PO43-(aq) → Cu3(PO4)2 (s)

d)

Cu2+(aq) + PO43-(aq) → CuPO4 (s)

73.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
74.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
75.
Zinc Carbonate
a)
Soluble 
b)
Insoluble 
76.
KOH
a)
Soluble 
b)
Insoluble
77.
Silver acetate
a)
Soluble 
b)
Insoluble
78.

What of these is always soluble?

a)

Nitrates

b)

Phosphates

c)

Carbonates

d)

Hydroxides

79.

What is the precipitate of this reaction?


MgCl2 + 2 NaOH --> Mg(OH)2 + 2 NaCl

a)

MgCl2

b)

NaOH

c)

Mg(OH)2

d)

NaCl

80.

What is the precipitate of this reaction?


Na2O + NiF2 --> 2 NaF + NiO

a)

Na2O

b)

NiF2

c)

NaF

d)

NiO

81.

Mixing Fe(NO3)2 (aq) and Na2CO3 (aq) causes an orange precipitate to form. What is the chemical formula of the precipitate?

a)

Fe(NO3)2 (s)

b)

FeCO3 (s)

c)

NaNO3 (s)

d)

Na2(NO3)2 (s)

82.

According to the solubility rules (chart), compounds containing Ammonium cations, NH4+ are:

a)

Not Soluble

b)

Sometimes Soluble

c)

Always Soluble

d)

Always insoluble

83.

CaCl2(aq) + 2 AgNO3(aq) → Ca(NO3)2(aq) + 2 AgCl(s)


Which product above is the precipitate?

a)

CaCl2(aq)

b)

AgNO3(aq)

c)

Ca(NO3)2(aq)

d)

AgCl(s)

84.

Predict the Products of the double-replacement (precipitate) reactions


K3PO4(aq) + AlCl3(aq) →

a)

K3PO4 (s) + AlCl (aq)

b)

KCl (aq) + Al2(PO4)3 (s)

c)

KCl (s) + Al2(PO4)3 (aq)

d)

K3AL (s) + Cl3PO4 (aq)

85.

What factor increases the dissolution rate due to more surface area being exposed to the solvent?

a)

Granulated sugar compared to a sugar cube

b)

Adding a solute with a common ion

c)

Decreasing the temperature

d)

Using a non-polar solvent for a polar solute

86.

What process allows fresh solvent molecules to come into contact with the solute, speeding up dissolution?

a)

Condensation

b)

Evaporation

c)

Agitation or stirring

d)

Freezing

87.

How does temperature affect the dissolution process?

a)

Increases molecule movement, aiding dissolution

b)

Decreases molecule movement

c)

Has no effect on dissolution

d)

Only affects gases

88.

What type of solutes dissolve well in polar solvents?

a)

Insoluble solutes

b)

Solid solutes only

c)

Polar solutes

d)

Non-polar solutes

89.

Which factor does NOT directly affect the rate of dissolution?

a)

Surface area of the solute

b)

Presence of other solutes

c)

Agitation of the solution

d)

Color of the solvent

90.

What is solubility?

a)

How much of a solute can dissolve in a given amount of solvent

b)

The color change when a solute dissolves

c)

The temperature at which a solute dissolves

d)

How quickly a solute dissolves in a solvent

91.
The universal solvent is ______. 
a)
sodium 
b)
acid 
c)
water 
d)
wind 
92.

In order to dilute a solution, you need to

a)

add more of the solid

b)

add more water

c)

find the mass

d)

find the volume

93.

A solution is prepared by dissolving 0.60 g of sodium chloride NaCl in 500 mL of water. Identify the solute.

a)

water

b)

sodium chloride

c)

NaCl solution

d)

distilled water

94.
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.
95.

What is required for a liquid to conduct an electric current?

a)

ions that are mobile

b)

ions in a strong bond

c)

covalent bonds

d)

shared protons

96.

Why are all ionic compounds electrolytes?

a)

because they are non-metals

b)

because they share electrons when they bond

c)

because they are electrically neutral

d)

because they dissociate into ions

97.

An atom that has lost or gained electrons.

a)

ion

b)

proton

c)

non-metal

d)

metalloid

98.

Why are molecular compounds nonelectrolytes?

a)

they do not have kinetic energy

b)

they do not contain atoms

c)

they do not have chemical bonds

d)

they are not composed of ions

99.

Which describes an Electrolyte?

a)

Substance that give out ions when dissolved in water, which are able to conduct electricity

b)

Substances that prehibit electricity from traveling across a solvent

c)

A chemical used to combust flames in a laboratory setting

d)

A type of current that is utilized to determine if there is a blockage anywhere in the system.

100.

Which of the following, when dissolved in water, would create a nonelectrolyte?

a)

C2H6O

b)

NH4NO3

c)

NaOH

d)

BaCl2

101.

As pressure increases in water

a)

gases are less able to dissolve

b)

gases are more able to dissolve

c)

gases are less able to stay dissolved

102.

How does an increase in temperature affect the solubility of gases?

a)

It increases the solubility of the gas.

b)

It decreases the solubility of the gas.

c)

It has no effect on the solubility of the gas.

Similar Resources on Wayground

Ionic Bonds

99 questions

Ionic Bonds

quiz

Worksheet

•

10th Grade

Final Review

103 questions

Final Review

quiz

Worksheet

•

10th - 11th Grade

Ch. 20 - Nuclear Reactions

104 questions

Ch. 20 - Nuclear Reactions

quiz

Worksheet

•

8th - 12th Grade

Chemical Compounds Review Quizizz

100 questions

Chemical Compounds Review Quizizz

quiz

Worksheet

•

8th - 12th Grade

Unit 1 Exam Review

100 questions

Unit 1 Exam Review

quiz

Worksheet

•

7th - 10th Grade

IIT-JEE & NEET LEVEL-3 (9-T)

100 questions

IIT-JEE & NEET LEVEL-3 (9-T)

quiz

Worksheet

•

9th Grade

Matter in our Surroundings

100 questions

Matter in our Surroundings

quiz

Worksheet

•

9th Grade

Hía

105 questions

Hía

quiz

Worksheet

•

10th Grade