wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Q.4 (H.Chem) Final Exam Review

Total questions: 211

Worksheet time: 5hrs 22mins

Name
Class
Date
1.

Assuming that the number of moles is constant, gas laws involve what three variables?

a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
2.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
3.
What will happen to the volume of a gas if the pressure increases, with constant temperature ?
a)
Increase
b)
Decrease
c)
Nothing
d)
Explosion!
4.
If you increase the pressure, what will happen to the temperature, if volume is constant?
a)
Increase
b)
Decrease
c)
Stay the same
d)
It will Blow Up
5.
According to the Combined Gas Law, pressure and volume are inversely related which means that
a)
When pressure increases, volume increases
b)
When pressure decreases, volume decreases
c)
When pressure increases, volume decreases
d)
When pressure doubles, volume triples
6.
According to the Combined Gas Law, volume and temperature are directly related. This means that
a)
When volume increases, temperature increases
b)
When volume increases, temperature decreases
c)
When volume double, pressure triples
d)
When volume doubles, volume is reduced by 1/2
7.

If 6.0 L of gas at 293K is compressed to 4.0 L, what is the new temperature? 

a)
195K
b)
439.5K
c)
0.082K
d)
12.2K
8.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
9.

4.0L of a gas is contained at 300 kPa and 200K. What will its volume be in L at 140 kPa and 100K?

a)
4.3L
b)
4.8L
c)
6.2L
d)
8.5L
10.

A gas at 928 kpa, 129 °C occupies a volume of 569 L. Calculate the volume at 319 kpa and 32 °C.

a)
410.61 L
b)
418.18 L
c)
1255 L
d)
1400 L
11.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
12.

If the pressure of a gas starts at 200kPa and increases to 600kPa, what would the initial temperature be if it ended up at 300K?

a)
50K
b)
200K
c)
400K
d)
100K
13.
The energy of an object as it is in motion is defined as
a)
Kinetic Theory
b)
Kinetic energy
c)
Potential energy
d)
Electric energy
14.
The temperature at which all molecular motion stops is
a)

-460 °C

b)
-273K
c)
0K
d)

0 °C

15.
When a cold tire is inflated to a certain pressure and then is warmed up due to friction with the road, the pressure increases. This happens because the
a)

air molecules hit the walls of the tire less frequently.

b)

rubber in the tires reacts with oxygen in the atmosphere.

c)

air molecules speed up and collide with the tire walls more often.

d)
air molecules diffuse rapidly through the walls of the tire.
16.

The random molecular motion of a substance is greatest when the substance is..

a)
condensed
b)
frozen
c)

a gas

d)
a liquid
17.
The kinetic theory of matter states that all of the particles that make up matter are constantly
a)
growing
b)
shrinking
c)
crying
d)
moving
18.
At higher temperatures...
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
19.
If you place a balloon in a freezer what happens to the size of the balloon?
a)
Doubles
b)
increases
c)
decreases
d)
stays still
20.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
21.

Match the following units to their names.

a)

Pressure

1.

mmHg

b)

Volume

2.

L

c)

Temperature

3.

K

d)

Pressure

4.

atm

e)

Moles

5.

mol

22.

A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?

a)

60.0 mL

b)

15.0 mL

c)

27.5 mL

d)

32.5 mL

23.
If I have 4 containers with equal volume and the containers are under the pressures listed below. Which container would have the lowest temperature?
Container A: 760 torr
Container B: 1000 torr
Container C: 1500 torr
Container D: 2000 torr 
a)
Container A
b)
Container B
c)
Container C
d)
Container D
24.
A 135 mL sample of argon had its pressure changed from 75.0 kPa to 121 kPa. What is its new volume?
a)
83.7 mL
b)
98.3 mL
c)
76.4 mL
d)
5 mL
25.

Consider a sample of oxygen gas at 27 °C with a volume of 9.55L at a pressure if 2.97 atm. The pressure is changed to 8.25 atm and the gas is heated to 125 °C. What’s the new volume?

a)

4.56 L

b)

4.6 L

c)

15.9 L

d)

16 L

26.

Which law?

a)

Charles (V/T)

b)

Boyle (P•V)

c)

Avogadro's (P/n)

d)

Amonton's (P/T)

27.

Which container will have a lower pressure?

a)

left

b)

right

c)

they both have the same pressure

d)

I don't know

28.

Three gases, Ar, N2 and H2 are mixed in a 500 L container. Ar has a pressure of 255 torr, N2 has a pressure of 228 torr and H₂ has pressure of 752 torr. What is the total pressure in the container?

a)

483 torr

b)

270 torr

c)

1235 torr

29.
What does this picture represent? 
a)
solid
b)
liquid 
c)
gas
d)
plasma
30.

The total kinetic energy of a collection of gas molecules is inversely proportional to the absolute temperature of the gas.

a)

True

b)

False

31.

In the KMT, pressure is the force exerted against the wall of a container by the continual collision of molecules against it.

a)

True

b)

False

32.

According to the kinetic molecular theory, the volume actually occupied by the molecules of a gas is negligibly small; the vast majority of the volume of the gas is empty space through which the gas molecules are moving.

a)

True

b)

False

33.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
34.
What about gasses can be measured?
a)
Pressure and Volume
b)
Temperature, Volume, and Pressure
c)
Volume and Temperature
d)
Pressure, Temperature, Volume, and Moles
35.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
36.

A student needs to know the temperature at which she should fill a balloon with 0.0470 mol of gas to 1.20 L so that the balloon reaches 0.998 atm of pressure. 

a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
37.

Calculate the partial pressure of H2 at 20oC when the vapor pressure of water is 17.5 torr. The total pressure of the gases is 750 torr.

a)

767.5torr

b)

732torr

c)

42.86torr

38.

The total pressure of a mixture of oxygen and nitrogen gas is 400.0 kPa. What is the partial pressure of nitrogen if the pressure of oxygen is 150.0 kPa?

a)

400.0 kPa

b)

550.0 kPa

c)

250.0 kPa

d)

101.3 kPa

39.
What does STP stand for?
a)
Standard Temperature and Pressure
b)
1.0 mmHg and 273 degree Kelvin
c)
1.0 degree Celcius and 0 atm
d)
1.0 atm 273 degree Celcius
40.
How many kPa are in 390 torr?
a)
51,983 kPa
b)
.51 kPa
c)
296,400 kPa 
d)
52 kPa
41.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

42.

Mg3N2 + 3H2O ––> 3 MgO + 2NH3

If 10.3 g of magnesium nitride is used, what volume of ammonia gas would be collected at 20˚C and 0.989 atm?

a)

4.9 L NH3

b)

4.96 L NH3

c)

0.261 L NH3

d)

0.26 L NH3

43.

1Mg + 2H2O --> Mg(OH)2 + H2

What volume of hydrogen will be produced at STP by the reaction 67.3 g of magnesium?

a)

62.0 L

b)

0.12 L

c)

2.77 L

d)

1.15 L

44.

2NaN3 → 2Na + 3N2

At what pressure(atm) is the nitrogen gas sample that is collected when 48.4 g of NaN3 decomposes? The temperature of the gas is 25.0°C and the volume is 18.4 L.

a)

151 atm

b)

1130 atm

c)

0.125 atm

d)

1.48 atm

45.

A student using a Styrofoam cup as a calorimeter added a piece of metal to distilled water and stirred the mixture as shown in the diagram. The student's data is shown in the table. Which statement correctly describes the heat flow in calories? (Ignore heat gained or lost by the calorimeter.)

a)

The water lost 1360 calories of heat and the metal gained 140 calories of heat.

b)

The water lost 350 calories of heat and the metal gained 350 calories of heat.

c)

The water gained 1360 calories of heat and the metal lost 140 calories of heat.

d)

The water gained 350 calories of heat and the metal lost 350 calories of heat.

46.

The diagrams shown represents two solids and the temperature of each. What occurs when the two solids are placed in contact with each other?

a)

Heat energy flows from solid A to solid B.

b)

Heat energy flows from solid A to solid B. Solid A increases in temperature.

c)

Heat energy flows from solid B to solid A. Solid B decreases in temperature.

d)

Heat energy flows from solid B to solid A.

47.

Two samples of gold that have different temperatures are placed in contact with one another. Heat will flow spontaneously from a sample of gold at 60°C to a sample of gold that has a temperature of (a)   .

Choose from the below words
50°C

60°C

70°C

80°C

48.

Which term represents a form of energy?

a)

heat

b)

degree

c)

kilocalorie

d)

temperature

49.

When a chemical bond is broken, energy is ​ (a)   .

Choose from the below words
only released

neither absorbed nor released

only absorbed
both absorbed and released
50.

Which form of energy is converted to thermal energy when propane burns in air?

a)

electromagnetic

b)

nuclear

c)

electrical

d)

chemical

51.

The temperature of a sample of water changes from 10°C to 20°C when the sample absorbs 418 joules of heat. What is the mass of the sample?

a)

1 g

b)

10 g

c)

100 g

d)

1000 g

52.

How many joules of heat are absorbed to raise the temperature of 435 grams of water at 1 atm from 25°C to its boiling point, 100°C?

a)

4.5 x 104 J

b)

1.4 x 105 J

c)

2.5 x 107 J

d)

7.4 x 107 J

53.

As a 15.1-gram sample of a metal absorbs 485.7 J of heat, its temperature increases 25.0 K. What is the specific heat capacity of the metal?

a)

0.129 J/g•K

b)

1.95 J/g•K

c)

1.29 J/g•K

d)

7.74 J/g•K

54.

The temperature of 15 grams of water increased 3.0 °C. How much heat was absorbed by the water?

a)

5.0 calories

b)

12 calories

c)

18 calories

d)

45 calories

55.

What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water. The water weighs 75. g and had an initial temperature of 20.00 °C? (Specific heat of water is 4.18 J/g⋅°C)

a)

0.111 J/g⋅°C

b)

1.29 J/g⋅°C

c)

0.129 J/g⋅°C

d)

22225.85 J/g⋅°C

56.

Calorimetry Question:
A piece of metal with a mass of 32.8 g is heated to 100.5°C and dropped into 138.2 g of water at 20.0°C.  The final temperature of the system is 30.2°C.  What is the specific heat capacity of the metal? (Specific heat of water is 4.18 J/g⋅°C)

a)

2.56 J/g⋅°C

b)

0.391 J/g⋅°C

c)

5.29 J/g⋅°C

d)

3.50 J/g⋅°C

57.

Consider the reaction:

H2O (l) + energy → H2 (g) + 1/2 O2 (g)

Which phrase best describes this reaction?

a)

exothermic, releasing energy

b)

exothermic, absorbing energy

c)

endothermic, releasing energy

d)

endothermic, absorbing energy

58.

When a substance was dissolved in water, the temperature of the water increased. This process is described as

a)

endothermic, with the release of energy

b)

endothermic, with the absorption of energy

c)

exothermic, with the release of energy

d)

exothermic, with the absorption of energy

59.

Which potential energy diagram represents the reactions A + B → C + energy?

a)

b)

c)

d)

Diagram D

60.

A solid is dissolved in a beaker of water. Which observation suggests that the process is endothermic?

a)

The solution gives off a gas.

b)

The solution changes color.

c)

The temperature of the solution decreases.

d)

The temperature of the solution increases.

61.

Which phase change is exothermic?

a)

H2O(s) → H2O(l)

b)

H2O(l) → H2O(s)

c)

H2O(s) → H2O(g)

d)

H2O(l) → H2O(g)

62.

When NH4NO3 is dissolved in water, the temperature of the water decreases. When NaOH is dissolved in a separate water sample, the temperature of the water increases. Based on these observations, it can be concluded that the dissolving of

a)

both salts is endothermic

b)

both salts is exothermic

c)

NH4NO3 is endothermic and the dissolving of NaOH is exothermic

d)

NH4NO3 is exothermic and the dissolving of NaOH is endothermic

63.

Given the reaction: Fe + S → FeS + energy. Which statement about this reaction is true?

a)

It is endothermic

b)

It is exothermic

c)

The potential energy of the reactants is lower than the potential energy of the product.

d)

The potential energy of the reactants is the same as the potential energy of the product.

64.

Given the reaction:

2H2(g) + O2(g) → 2H2O(l) + 571.6kJ

What is the approximate ΔH for the formation of 1 mole of H₂O(l)?

a)

−285.8 kJ

b)

+285.8 kJ

c)

−71.6 kJ

d)

+571.6 kJ

65.

The potential energy diagram shown represents the reaction

A + B → AB

Which statement correctly describes this reaction?

a)

It is endothermic and energy is absorbed.

b)

It is endothermic and energy is released.

c)

It is exothermic and energy is absorbed.

d)

It is exothermic and energy is released.

66.

Which potential energy diagram represents an exothermic reaction?

a)

b)

c)

d)

67.

Which statement describes characteristics of an endothermic reaction?

a)

The sign of ΔH is positive, and the products have less potential energy than the reactants.

b)

The sign of ΔH is positive, and the products have more potential energy than the reactants.

c)

The sign of ΔH is negative, and the products have less potential energy than the reactants.

d)

The sign of ΔH is negative, and the products have more potential energy than the reactants.

68.

As a result of dissolving a salt in water, a student found that the temperature of the water increased. From this observation alone, the student should conclude that the dissolving of the salt (a)   .

Choose from the below words

produced an acid solution

produced a basic solution

was endothermic

was exothermic
69.

Which phase change is endothermic?

a)

gas → solid

b)

gas → liquid

c)

liquid → solid

d)

liquid → gas

70.

Given the reaction:

H2O(l) + 68.3kcal ⇌ H2(g) + O2(g)

Which statement describes the reverse reaction?

a)

It is endothermic and releases 68.3 kilocalories.

b)

It is endothermic and absorbs 68.3 kilocalories.

c)

It is exothermic and releases 68.3 kilocalories.

d)

It is exothermic and absorbs 68.3 kilocalories.

71.

Which statement correctly describes this reaction?

a)

It is endothermic and energy is absorbed.

b)

It is endothermic and energy is released.

c)

It is exothermic and energy is absorbed.

d)

It is exothermic and energy is released.

72.

Which statement correctly describes this reaction?

a)

It is endothermic and energy is absorbed.

b)

It is endothermic and energy is released.

c)

It is exothermic and energy is absorbed.

d)

It is exothermic and energy is released.

73.

The forward reaction is best described as an (a)   .

Choose from the below words

exothermic reaction in which energy is released

exothermic reaction in which energy is absorbed

endothermic reaction in which energy is released

endothermic reaction in which energy is absorbed
74.

Given the balanced equation representing a reaction at 101.3 kPa and 298K:

N2 (g) + 3H2 (g) → 2NH3 (g) + 91.8 kJ

Which statement is true about this reaction?

a)

It is exothermic and ΔH equals –91.8kJ.

b)

It is exothermic and ΔH equals +91.8kJ.

c)

It is endothermic and ΔH equals –91.8kJ.

d)

It is endothermic and ΔH equals +91.8kJ.

75.

The enthalpy change for a chemical reaction can be calculated using which of the following formulas?

a)

ΔH=Hproducts−Hreactants\Delta H = H_{products} - H_{reactants}

b)

ΔH=Hreactants+Hproducts\Delta H = H_{reactants} + H_{products}

c)

ΔH=Hreactants−Hproducts\Delta H = H_{reactants} - H_{products}

d)

ΔH=Hproducts/Hreactants\Delta H = H_{products} / H_{reactants}

76.

Organize these options into the correct types of energy use.

Categorize the following

absorbs energy

releases energy

splitting a molecule

forming a molecule

melting ice

NH4NO3 (s) + H2O(l) + 23.8 kJ → NH4OH(aq) + HNO3NH_4NO_3\ \left(s\right)\ +\ H_2O\left(l\right)\ +\ 23.8\ kJ\ \rightarrow\ NH_4OH\left(aq\right)\ +\ HNO_3  

6SOCl2 + CoCl2⋅6H2O → CoCl2 + 6SO2 + 12HCl    ΔH=+6SOCl_2\ +\ CoCl_2\cdot6H_2O\ \rightarrow\ CoCl_2\ +\ 6SO_2\ +\ 12HCl\ \ \ \ \Delta H=+  

H2SO4 (aq) + 2NaOH (aq) → Na2SO4 (aq) + H2O (l)   ΔH = −H_2SO_4\ \left(aq\right)\ +\ 2NaOH\ \left(aq\right)\ \rightarrow\ Na_2SO_4\ \left(aq\right)\ +\ H_2O\ \left(l\right)\ \ \ \Delta H\ =\ -  

Endothermic
Exothermic
77.

Are the products or reactants of this reaction storing more energy in their chemical bonds?

a)

Both storing the same

b)

No way to tell

c)

Products

d)

Reactants

78.
Breaking chemical bonds will always _______ energy and forming chemical bonds will always _______ energy.
a)
absorb, release
b)
release, absorb
c)
absorb, absorb
d)
release, release
79.

Some chemical reactions are ​ (a)   where the heat energy is absorbed. Other chemical reactions release heat energy are known as ​ (b)   .​

Choose from the below words
endothermic
exothermic
thermal
geothermal
80.

In the figure, the reactants have​ (a)   energy than the products. This indicates that energy has been ​ (b)   , making this an ​ (c)   reaction.

Choose from the below words

more

less
absorbed
endothermic
exothermic
released
activation energy
81.

In the figure, heat energy is (a)   during the reaction. This makes this an ​ (b)   reaction.

Choose from the below words
released
exothermic
absorbed
endothermic
activation energy
82.

In an exothermic chemical reaction:

a)

the mass of the products is greater than the mass of the reactants.

b)

the mass of the products is less than the mass of the reactants.

c)

heat is released as the reaction proceeds.

d)

heat is absorbed as the reaction proceeds.

83.

Based on the reaction CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (g) and its energy profile, the reaction (a)   .

Choose from the below words
is exothermic.

has a high activation energy.

is nonspontaneous.

violates the first law of thermodynamics.

84.

Toasting a piece of bread is an example of an ​ (a)   .

Choose from the below words
endothermic reaction
exothermic reaction
isoenergetic reaction
energetic physical change
85.

What factor determines whether a reaction will be exothermic or endothermic?

a)

the difference in energy between reactants and products

b)

the activation energy of the reaction

c)

the speed of the reaction

d)

the relative concentrations of reactants and products in solution

e)

the heat properties of the products

86.

An endothermic reaction corresponds to one in which

(a)  

Choose from the below words
the system absorbs energy from the surroundings.

the system releases energy to the surroundings.

the system neither absorbs nor releases energy.

the system's energy remains constant.

87.

In chemical thermodynamics, a system is defined as ​ (a)   .

Choose from the below words
any part of the universe that is under study
one mole of the substance
one kg of the mixture
containing one kg of the solvent
88.

Which line on this diagram represents the enthalpy (potential energy) of the reactants?

a)

A

b)

B

c)

C

d)

D

89.

Which line on the diagram represents the enthalpy (potential energy) of the products?

a)

A

b)

B

c)

C

d)

D

90.

Does this diagram represent an endothermic or exothermic overall reaction?

a)

Endothermic, the products are higher in potential energy than the reactants.

b)

Endothermic, the products are lower in potential energy than the reactants.

c)

Exothermic, the products are lower in potential energy than the reactants.

d)

Exothermic, the products are higher in potential energy than the reactants.

91.

Choose the pair that correctly indicates the sign of ΔT and ΔH for the reaction in this diagram.

a)

ΔH +, ΔT +

b)

ΔH +, ΔT –

c)

ΔH –, ΔT +

d)

ΔH –, ΔT –

92.

Which statement would be a correct interpretation of the First Law of Thermodynamics?

a)

Energy can be transformed from one type to another (e.g., potential to kinetic).

b)

Energy can be created spontaneously from nothing.

c)

Energy cannot be transformed from one type to another (e.g., potential to kinetic).

d)

Matter can be transformed into energy in a chemical reaction.

93.

Which of the following will best help determine the direction of heat flow in a system?

a)

temperature

b)

pressure

c)

enthalpy

d)

work

e)

internal energy

94.

What mass of propane, C3H8 (g), must be burned to supply 2775 kJ of heat? The standard enthalpy of combustion of propane at 298 K is −2220 kJ·mol-1.

a)

35.3 g

b)

55.1 g

c)

102 g

d)

75.9 g

e)

44.1 g

95.

The heat of combustion of butane, C4H10, is −2623 kJ/mol. How much heat would be absorbed or evolved when 90. g butane is burned?

a)

4062 kJ evolved

b)

4062 kJ absorbed

c)

2623 kJ absorbed

d)

2623 kJ evolved

96.

Consider the reaction: C2H5OH (l) + O2 (g) → 2CO2 (g) + 3H2O (g), ΔH = −1.37x10³ kJ/molrxn

When a 21.1 g sample of ethyl alcohol, C2H5OH, is burned, what is the change in enthalpy? The molar mass of ethanol is 46.07 g/mol.

a)

−0.458 kJ

b)

0.627 kJ

c)

−6.27x10² kJ

d)

2.89x10⁴ kJ

97.

Consider the reaction:

CH4 (g) + 4Cl2 (g) → CCl4 (g) + 4HCl (g); ΔH = −434 kJ/molrxn

What is the change in enthalpy, ΔH, when 43.7 g of Cl₂ reacts completely as shown above?

a)

−286 kJ

b)

−66.9 kJ

c)

−535 kJ

d)

−134 kJ

98.

When the volume of solvent increases, the mass of solute that can dissolve in a saturated solution...

a)

increases

b)

decreases

c)

stays the same

99.

When the volume of solvent increases, the solubility of a solute at a given temperature...

a)

increases

b)

decreases

c)

stays the same

100.

In general as temperature of a mixture of a solid in a liquid decreases, what happens to the solubility of the substance...

a)

it increases

b)

it decreases

c)

it stays the same

d)

it may increase or decrease depending on whether the solid is ionic or molecular

101.
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
102.

I have an unsaturated solution of 15.0 grams of KNO3 in 100. grams of water. I can make it saturated by adding what?

a)

KNO3 (s)

b)

H2O (l)

c)

KCl (s)

d)

Ca(NO3)2 (s)

103.

Calculate the molarity of a solution containing 1.5 moles of NaCl in 0.50 L of solution.

a)

1.5 M

b)

0.33 M

c)

30. M

d)

3.0 M

104.

How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?

a)

68.7 mmol

b)

68.7 mol

c)

1.07 mol

d)

14.5 mmol

105.

What is the molarity of a solution which contains 224.1 milligrams of NaCl in 50.0 mL of solution?

a)

0.448 M

b)

0.192 M

c)

3.83 M

d)

0.0767 M

106.

How many moles of a solute are needed to make 2.5 L of a 0.38 M solution?

a)

0.95 mol

b)

6.6 mol

c)

0.15 mol

d)

1.5 mol

107.

What is the molarity of a solution of NaOH that contains 2.5 mol in 12.0 L of solution?

a)

0.21 M

b)

0.30 M

c)

4.8 M

d)

3.0 M

108.

A 360. mg sample of aspirin, C9H8O4, (molar mass 180. g), is dissolved in enough water to produce 200. mL of solution. What is the molarity of aspirin in a 50.0 mL sample of this solution?

a)

0.0800 M

b)

0.0400 M

c)

0.0200 M

d)

0.0100 M

e)

0.00250 M

109.

A 40.0 mL sample of 0.25 M KOH is added to 60.0 mL of 0.15 M Ba(OH)2. What is the molar concentration of OH-(aq) in the resulting solution? (Assume that the volumes are additive.)

a)

0.10 M

b)

0.19 M

c)

0.28 M

d)

0.40 M

e)

0.55 M

110.

Any salt that dissolves in water breaks up entirely into ions. How many mmoles of Na+ ions are in 100. mL of 0.100 M Na3PO4 (aq)?

a)

0.300 mmol

b)

10.0 mmol

c)

30.0 mmol

d)

0.0100 mmol

111.

How many grams of CaCl2 (molar mass = 111 g/mol) are needed to prepare 100. mL of 0.100 M Cl-(aq) ions?

a)

0.555 g

b)

1.11 g

c)

2.22 g

d)

5.55 g

112.

Solid Al(NO3)3 is added to distilled water to produce a solution in which the concentration of nitrate, [NO3-], is 0.10 M. What is the concentration of aluminum ion, [Al3+], in this solution?

a)

0.010 M

b)

0.033 M

c)

0.10 M

d)

0.30 M

113.
What word describes when water is attracted to other substances?
a)
cohesion
b)
adhesion
c)
capillary action
d)
surface tension
114.
Why does ice float?
a)
As water freezes, it expands and its density decreases.
b)
As water freezes, it takes up more hydrogen from the atmosphere, causing it to have a greater buoyancy.
c)
As water freezes, air becomes trapped between the hydrogen bonds of water molecules.
d)
As water freezes, it takes up more oxygen from the atmosphere, causing it to have a greater buoyancy.
115.
True or false water is a polar molecule? 
a)
True 
b)
False 
116.
The attraction that causes water and other liquids to form drops is called ________________. This is also water’s ability to be attracted to other water molecules.
a)
adhesion
b)
capillary action
c)
cohesion
d)
surface tension
117.
The substance that gets dissolved is called solvent.
True or False?
a)
True.
b)
False.
118.
Type of mixture in which all substances are evenly distributed is a?
a)
Solution
b)
Solute
c)
Solvent
119.
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
120.
This is the part of a solution that dissolves
a)
Solute
b)
Solvent
c)
Solution
d)
Mixture 
121.
In the above picture, a powder is about to be poured into the liquid. Which of the following should be done to make this powder dissolve faster?

a)
stir the powder in the liquid
b)
freeze the mixture
c)
add more powder to the liquid
d)
store the mixture in a dark place
122.
A solution that is considered dilute would be....
a)
Dark in color
b)
Have a strong scent
c)
Have a large amount of solute
d)
Have a small amount of solute
123.
air is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
124.

When Koolaid mix is light colored and tastes watery it is a _______ solution.

a)

concentrated

b)

dilute

125.

When a Koolaid mix in water is dark in color and very sweet it is a __________ solution.

a)

Concentrated

b)

Dilute

126.
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
127.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
128.
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
129.
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
130.
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
131.
mixture of two or more substances; dissolved particles are spread evenly throughout the mixture
a)
solvent
b)
solute
c)
mixture
d)
solution
132.
Which process could be used to separate iron filings and sugar?
a)
boiling
b)
evaporation
c)
filtration
d)
magnetism
133.

According to Brønsted-Lowry acid base theory, an acid ___.

a)

is a proton donor

b)

is a proton acceptor

c)

produces H+ when added to water

d)

turns phenolphthalein pink

134.

According to Arrhenius acid-base theory, an acid ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces H+ in water

d)

turns litmus paper blue

135.

Which reactant in the following equation is acting as a Brønsted-Lowry acid?

a)

ammonium

b)

ammonia

c)

hydroxide

d)

water

136.

HSO4-(aq) + H2O(l) → H3O+(aq) + SO42-(aq)

Identify the Brønsted-Lowry acid in the above reaction.

a)

HSO4-

b)

H2O

c)

H3O+

d)

SO42-

137.

CO32-(aq) + H2O(l) → HCO3-(aq) + OH-(aq)

Using the above reaction, which species is the conjugate base?

a)

CO32-

b)

H2O

c)

HCO3-

d)

OH-

138.
A substance that remains when a base has accepted an H+ ion is
a)
An acid
b)
A Base
c)
A Conjugate Acid
d)
A Conjugate Base
139.

Choose the conjugate acid of OH-

a)

HCO3-

b)

OH-

c)

CO32-

d)

H2O

140.

Choose the conjugate base of HNO3

a)

HNO3

b)

H2O

c)

H3O+

d)

NO3-

141.

True or False: All Arrhenius acids are also Brønsted-Lowry acids.

a)

True

b)

False

142.

Which of the following substances is both a Brønsted-Lowry acid and an Arrhenius base?

a)

NH3(aq)

b)

LiOH(aq)

c)

HCl(g)

d)

HCl(aq)

143.

Which of the following is a polyprotic acid?

a)

HCl

b)

H2SO4

c)

HNO3

d)

HF

144.

Which of the following is the hydronium ion?

a)

H+

b)

H2O

c)

OH–

d)

H3O+

145.

Which substance is an Arrhenius base?

a)

KCl

b)

CH3Cl

c)

KOH

d)

CH3OH

146.

The conjugate acid for NH3 is

a)

NH2

b)

N

c)

H3

d)

NH4+

147.

According to Arrhenius acid-base theory, a base ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces OH- in water

d)

turns litmus paper red

148.

According to Brønsted-Lowry acid base theory, a base ___.

a)

is a proton donor

b)

is a proton acceptor

c)

produces OH- when added to water

d)

has a bitter taste

149.
Which of the following substances contain an alkali?
a)
Baking powder
b)
Coca cola
c)
Distilled water
d)
Vinegar
150.
Which of the following pH numbers indicates a strong acid?
a)
1
b)
5
c)
7
d)
14
151.

Which of the following pH numbers indicate a strong (base)alkali?

a)
1
b)
5
c)
7
d)
14
152.
What is the pH of pure water?
a)
pH 7
b)
pH 3
c)
pH 12
d)
pH 8
153.
What substance could you use to test if a substance is an acid or alkali?
a)
Indicator
b)
Salt
c)
Catalyst
d)
Water
154.

Which of the following is alkali?

a)
b)
c)
155.

Which of the following is neutral?

a)
b)
c)
156.

... are used to neutralise acid in the stomach.

a)

Toothpastes

b)

Bacterias

c)

Antacids

d)

More strong acids

157.

What is the purpose of an "indicator"?

a)

changes color if a chemical reaction occurs

b)

changes color if a physical change occurs

c)

changes color in the presence of an acid or base

d)

changes color when a salt dissolves in water

158.

WHAT ARE THE PROPERTIES OF ACID ?

a)

Acids are corrosive, sour,

b)

Lemon

c)

Mint

d)

tastes bitter

159.
Which of the following substances contain acid?
a)
An orange
b)
Bleach
c)
Distilled water
d)
Washing powder
160.
Which of the following pH numbers indicate a strong alkali?
a)
1
b)
5
c)
7
d)
14
161.

How to neutralise wasp sting

a)

baking soda

b)

vinegar

c)

Lime water

d)

Drain cleaner

162.
Which of the following pH numbers indicates a neutral substance?
a)
1
b)
5
c)
7
d)
14
163.

A STRONG ACID is one that...

a)

completely dissociates in water & produces H3O+

b)

completely dissociates in water & produces OH-

c)

partially dissociates in water & produces H3O+

d)

partially dissociates in water & produces OH-

164.

If something has a pH of LESS THAN 7, it is...

a)

an acid

b)

a base

c)

neutral

d)

not on the pH scale

165.

If a formula has an "O" in it, will it say HYDRO in the name?

a)

no

b)

yes

c)

depends on the other element

d)

yes, if it is combined with a halogen

166.

-ate = ______

a)

-ite

b)

-ic

c)

-ous

d)

-ide

167.

When you add the pH and the pOH it should equal what?

a)

14

b)

20

c)

7

d)

15

168.

Which one is the CONJUGATE BASE in the equation?


HCl + H2O--> Cl- + H3O+

a)

HCl

b)

H2O

c)

Cl-

d)

H3O

169.

If something has a pH of GREATER THAN 7, it is...

a)

an acid

b)

a base

c)

neutral

d)

not on the pH scale

170.

Is HBr a strong or weak acid or base?

a)

strong acid

b)

strong base

c)

weak acid

d)

weak base

171.

If [OH-] = 1.7 x 10-3 M, what is the pOH of the solution?

a)

2.77

b)

1.99

c)

9.96

d)

5.01

172.

Is LiOH a strong or weak acid or base?

a)

strong acid

b)

strong base

c)

weak acid

d)

weak base

173.

Which one is the ACID in the equation?


HCl + H2O--> Cl- + H3O+

a)

HCl

b)

H2O

c)

Cl-

d)

H3O+

174.

Which one is the CONJUGATE ACID in the equation?


HCl + H2O--> Cl- + H3O+

a)

HCl

b)

H2O

c)

Cl-

d)

H3O+

175.

Which one is the BASE in the equation?


HCl + H2O--> Cl- + H3O+

a)

HCl

b)

H2O

c)

Cl-

d)

H3O+

176.
HNO3
a)
Acid
b)
Base
177.
Al(OH)3
a)
Acid
b)
Base
178.
What is the pH of a 1 x 10-8 solution of HNO3?
a)
8
b)
6
c)
7
d)
7.5
179.
What is the pOH of a 1 x 10-8 solution of HNO3?
a)
8
b)
6
c)
7
d)
7.5
180.
HNO3
a)
Acid
b)
Base
181.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-14
d)
1-20
182.
What does pH measure?
a)
Amount of Oxygen Ions
b)
Amount of Hydrogen Ions
c)
The amount of salt in a solution
d)
The density
183.
What is the [H+] if the pH is 4.0?
a)
1.0 x 10-10  M
b)
1.0 x 10-4  M
c)
1.0 x 10-14  M
d)
1.0 x 10-7  M
184.
What is the [OH-] if the pH is 4.9?
a)
7.94 x 10-10 M
b)
1.0 x 10-4  M
c)
7.94 x 10-14 M
d)
4.9 x 10-10 M
185.
The lower the pH, the greater the concentration of :
a)
OH-
b)
H+
186.
The conjugate base of H2SO4 is ___. (HINT...bases are proton acceptors)
a)
H2SO3
b)
HSO4-
c)
H3SO4+
d)
SO4-2
187.

Which of the following contains acids?

a)

Milk

b)

Bleach

c)

Ammonia

d)

Chalk

188.
A strong acid:  
a)
completely dissociates in water
b)
partly dissociates in water
c)
doesn't dissociate in water
d)
has a really high pH
189.
What is the pOH of a 1 x 10-8 M solution of HNO3?
a)
8
b)
6
c)
7
d)
7.5
190.
If the solution of Al(OH)3 has a pH of 11.5 and a pOH of 2.5. Is it an acid, base, or neutral?
a)
acid
b)
base
c)
neutral
191.
What is the [OH-] if the [H+] is
1.0 x 10-3M?
a)
1.0 x 10-3 M
b)
6.02 x 10-23 M
c)
1.0 x 10-14 M
d)
1.0 x 10-11 M
192.
What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?
a)
-1.14
b)
2.0
c)
1.14
d)
7.3
193.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
194.
The following statement is true for Bronsted Lowry Conjugate Acid Base pair EXCEPT
a)
Bronsted Lowry Acid is a proton donor
b)
Bronsted Lowry Acid is a electron pair acceptor
c)
Conjugate acid has 1 hydrogen atom more than base
d)
Conjugate base has 1 hydroxide more than base
195.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
196.
What is the conjugate acid to NO3- ? (HINT...acids contain what ion?)
a)
HNO3
b)
OH-
c)
H+
d)
NO3-2
197.
What is not a conjugate base to acid pair? (HINT...follow the H+!!!)
a)
OH- : H2O
b)
H2O : H3O+
c)
CN- : HCN
d)
HSO4- : SO4-2
198.
The conjugate base of H2SO4 is ___. (HINT...bases are proton acceptors)
a)
H2SO3
b)
HSO4-
c)
H3SO4+
d)
SO4-2
199.
In this reaction...
CH3NH2 + H2O --> CH3NH3+ + OH-
CH3NH2 can be classified as which of the following? (HINT...follow the H+!!!)
a)
A Brønsted-Lowry base
b)
A Brønsted-Lowry acid
c)
A Lewis acid
d)
An Arrhenius acid
200.
The conjugate acid of HCO3- is ___ and the conjugate base of HCO3- is ___.  (remember that H+ ion? well, follow it!!)
a)
H2CO3; CO3-2
b)
CO3-2; CO3-2
c)
H2CO3; H2O
d)
H2O; H2CO3
201.
Identify the acid in the following reaction...
2 HI(aq) + CaO(s) → CaI2(aq) + H2O(l)
(HINT... acid + base → conj.acid + conj.base)
a)
HI
b)
CaO
c)
CaI2
d)
H2O
202.
Which of the following liquids would turn blue litmus paper red?
a)
orange juice (citric acid)
b)
distilled water (neutral)
c)
oven cleaner (base)
d)
Peptobismol (base)
203.
According to Brønsted-Lowry theory of acids and bases, a base is ___.
a)
a proton acceptor
b)
a proton donor
c)
a compound that dissolves in water to produce OH-
d)
an electron donor
204.
Acids do which of the following?
(HINT...check your notesheet "properties of acids & bases")
a)
produce H+ in solution
b)
taste bitter
c)
feel slippery & soapy
d)
produce OH- in solution
205.
Ammonia reacts slightly with water in the reaction given.  What would you expect the solution to be?
NH3(g) + H2O(l) → NH4+(aq) + OH-(aq)
a)
acidic
b)
basic
c)
neutral
206.
An Arrhenius base must contain ___ and ionize to produce ___.
a)
hydrogen ions; a solution with a pH greater than 7
b)
hydrogen; hydrogen ions
c)
hydroxide ion; hydroxide ions
d)
hydroxide ion; a solution with a pH greater than 7
207.
Which of the following is NOT a strong acid?
(HINT...use your notes that you copied off the board for warm-up today)
a)
HF
b)
HBr
c)
HNO3
d)
HCl
208.
Which of the following substances has the highest concentration of hydrogen ions in solution?
a)
bleach (pH = 11-13)
b)
water (pH = 7)
c)
tomato juice (pH = 4-5)
d)
vinegar (pH = 3-4)
209.
Which of the following solutions is most basic?
(HINT...be careful! Acidity and basicity are determined by the point measured on the pH scale. And don't forget [H+] = 10-pH)
a)
[H+] = 1 x 10-11
b)
[OH-] = 1 x 10-4
c)
[H+] = 1 x 10-2
d)
[OH-]= 1 x 10-13
210.
The pH of a solution is 4.00.  What is the hydroxide ion concentration?
(HINT...pH + pOH = 14 and
[OH-] = 10-pOH)
a)
[OH-] = 1 x 10-4
b)
[OH-] = 1 x 10-6
c)
[OH-] = 1 x 10-10
d)
[OH-] = 1 x 10-14
211.
What is the pH of a solution with a hydrogen ion concentration of 1.0 x 10-8 M?
(HINT...use the calculator...
pH = -log [H+] )
a)
-8
b)
6
c)
8
d)
14

Similar Resources on Wayground

Chemistry IGCSE

212 questions

Chemistry IGCSE

quiz

Worksheet

•

10th Grade

AP Final Revu Quizizz

214 questions

AP Final Revu Quizizz

quiz

Worksheet

•

12th Grade

Summer School Solution Exam Practice

208 questions

Summer School Solution Exam Practice

quiz

Worksheet

•

10th Grade

ÔN THI TN THPT HÓA 2023

214 questions

ÔN THI TN THPT HÓA 2023

quiz

Worksheet

•

12th Grade