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Chemistry OAT 1 (Chapter 12-16) Revision

Total questions: 122

Worksheet time: 5hrs 4mins

Name
Class
Date
1.
What two elements make up water?
a)
Helium and oxygen
b)
Hydrogen and oxygen
c)
helium and carbon
d)
oxygen and carbon
2.
In a water molecule the hydrogen and oxygen atoms hold together by sharing _________.
a)
protons 
b)
neutrons
c)
electrons
d)
nuclei
3.
Which end of the water molecule has a slightly positive charge?
a)
the oxygen end
b)
the hydrogen end
c)
both ends are slightly positive
d)
neither end is positive
4.
When a molecule has an opposite electrical charge on each end, it is known as what?
a)
cohesion
b)
polar molecule
c)
hydrogen bond
d)
solution
5.
Water is a universal solvent because it...
a)
It can be found anywhere
b)
It freezes when it gets cold
c)
floats when frozen
d)
Dissolves most substances
6.
Large bodies of water do not quickly fluctuate in temperature. Why?
a)
Water is a solvent.
b)
Water has a high heat capacity.
c)
Water acts as a buffer.
d)
Water is non-polar.
7.
The fact that ice floats on liquid water is due to the fact that water's solid is ___________ than it's liquid form
a)
less polar
b)
more polar
c)
less dense
d)
more dense
8.
Which statement explains why water molecules stick together?
a)
both sides are negative
b)
one side has a positive charge and the other side has a negative charge
c)
one side has a negative charge adn the other side has a neutral charge
d)
both sides are positive
9.
What is the chemical formula for water?
a)
H20
b)
h2o
c)
H2O2
d)
H2O
10.
Attractions between the negative Oxygen atom of one water molecule and the positive Hydrogen atom of another water molecule are called
a)
Covalent bonds
b)
Ionic bonds
c)
Polar bonds
d)
Hydrogen bonds
11.
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.
12.
Which of the following is LEAST likely to dissolve in water?
a)
nonpolar fats and oils
b)
polar sugar molecules
c)
salt made of a positive sodium ion and a negative chloride ion
d)
all of the substances will dissolve easily in water
13.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
14.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
15.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
16.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
17.
Does H2O have hydrogen bonding?
a)
yes
b)
no
18.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

19.

Which will heat up faster?

a)

copper

b)

granite

c)

iron

d)

basalt

20.

Which will heat up slower?

a)

water

b)

lead

c)

granite

d)

iron

21.

How much energy is needed to raise the temperature of 5.0 grams of lead from 25°C to 35°C? [specific heat (c) = 0.129 J/(g•°C)]

a)

6.45 J/(g•°C)

b)

6.45 J

c)

16.1 J/(g•°C)

d)

d.16.1 J

22.

The temperature of a 6.0 g sample of glass changed from 20.0°C to 45.0°C when it absorbed 550 J of heat. What is the specific heat of this glass?

a)

0.27 J/g °C

b)

3.7 J/g °C

c)

130 J/g °C

d)

12 J/g °C

23.

Which of the following best explains why the sand at the beach is hotter than the water?

a)

Sand has a higher specific heat than water.

b)

Sand has a lower specific heat than water.

c)

There is more water than sand at the beach.

d)

There is more sand than water at the beach.

24.
When a  piece of aluminum foil is taken out of the oven and cools from 100° to 50°, What is the change in temperature?
a)
50°
b)
0°
c)
100°
d)
150°
25.
The amount of energy required to raise the temperature 1ºC for every kilogram is called____?
a)
Thermal Energy
b)
Specific Heat
c)
Temperature
d)
Kinetic Energy
26.
Object A has a specific heat of 4.45 J/g⁰C and object B has a specific heat of 1.82 J/g⁰C. Which object will heat up faster?
a)
Object A, it has a lower spefici heat
b)
Object B, it has a lower specific heat
c)
Object A, it has a higher specific heat
d)
Object B, it has a higher specific heat
27.
Graphite has a specific heat of 0.709 J/g⁰C. If a 20 gram piece of graphite is cooled from 38⁰C to 18⁰C, how much energy was lost by the graphite?
a)
283.6 J
b)
183.6 J
c)
203 J
d)
109 J
28.

Latent heat is

a)

the heat absorbed or released at a boiling process during a change of phase

b)

the heat absorbed or released at a constant temperature during a change of phase

c)

the heat absorbed or released at a constant temperature during a change of phase of 1 kg object

d)

the heat absorbed or released by an object to increase or decrease its temperature by 1 degree Celcius

29.

The heat absorbed by melting a solid is known as

a)

latent heat of fusion

b)

latent heat of solid

c)

latent heat of liquid

d)

latent heat of vaporisation

30.

The amount of heat required to change the phase of a substance depends on two factors which are

a)

surrounding temperature

b)

temperature change

c)

material

d)

the mass

31.

specific latent heat of vaporisation is

a)

the amount of heat required to change 1 kg of the substance from the solid to liquid phase without change in temperature

b)

the amount of heat required to change 1 kg of the substance from the liquid to gaseous phase without change in temperature

c)

the amount of heat required to change the temperature 1 kg of the substance by 1 degree Celcius

32.

Select the correct equations.

a)

thermal energy = specific latent heat / mass

b)

thermal energy = specific latent heat x mass

c)

mass = specific latent heat / thermal energy

d)

specific latent heat = thermal energy / mass

e)

mass = specific latent heat x thermal energy

33.

Water is known as a _______ molecule

a)

non-polar

b)

cold

c)

polar

d)

warm

34.

Water is known as the universal __________

a)

solute

b)

solution

c)

solvent

d)

bonder

35.

The substance that does the dissolving is called the

a)

solvent

b)

solute

c)

solution

36.

The substance that is being dissolved is called the

a)

solvent

b)

solute

c)

solution

37.

A solution is an...

a)

uneven distribution of solids in a liquid

b)

even distribution of solids in a liquid

38.

An example of a solution is

a)

pebbles and water

b)

sand and water

c)

oil and water

d)

salt and water

39.

Water particles ___________________.

a)

are attracted to each other.

b)

repel against each other.

c)

stick to water striders.

d)

cannot be broken down.

40.

An aqueous solution is:

a)

any liquid with another compound dissolved in it.

b)

an ionic compound with water dissolved in it.

c)

water with another compound dissolved in it.

d)

none of the above

41.

Which of the following compounds is SOLUBLE?

a)

copper carbonate

b)

calcium carbonate

c)

potassium carbonate

d)

strontium carbonate

42.

In writing the chemical equation for a precipitation reaction, what abbreviation of the physical state must appear with one of the products?

a)

(s)

b)

(g)

c)

(l)

d)

(w)

43.

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

a)

K(NO3)2

b)

PbSO4

c)

PbK2

d)

H2O

44.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

Which compound would not form ions in the complete ionic equation?

a)

PbI2

b)

KNO3

c)

Pb(NO3)2

d)

KI

45.

Considering the following precipitation reaction:


Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)


Which ion would NOT be present in the complete ionic equation?

a)

Pb2+

b)

K+

c)

NO3-

d)

I-

e)

All the above ions are in the complete ionic equation.

46.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

What is the correct complete ionic equation?

a)

Pb2+ + (NO3)2- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

b)

Pb2+ + 2NO3- +2K+ + I- → PbI2(s) + 2K+ + NO3-

c)

Pb2+ + 2NO3- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

d)

Pb2+ + 2NO3- + 2K+ + 2I- → Pb2+ + 2I- + 2K+ + 2NO3-

47.

Which of the following compounds is INSOLUBLE?

a)

magnesium phosphate

b)

magnesium sulfate

c)

magnesium iodide

d)

magnesium nitrate

e)

none of the above

48.

What is the net ionic equation for the precipitation reaction between BaCl2 and Na2SO4?

a)

BaCl2(aq) + Na2SO4(aq) --> BaSO4(s) + 2NaCl(aq)

b)

Na+(aq) + Cl-(aq) --> NaCl(s)

c)

Ba2+(aq) + SO42-(aq) --> BaSO4(s)

d)

Ba2+(aq) + 2Cl-(aq) + 2 Na+(aq) + SO42-(aq) --> BaSO4(s) + 2Cl-(aq) + 2Na+(aq)

49.

Which of the following pairs of solutions produces a precipitate when combined?

a)

Cu(NO3)2 and NaCl

b)

Fe(NO3)3 and MgCl2

c)

Cu(NO3)2 and K2CO3

d)

CaCl2 and NaNO3

50.

When solutions of MgCO3 and Fe2(SO4)3 are combined, what precipitate(s) forms?

a)

MgSO4

b)

neither form a precipitate

c)

MgSO4 and Fe2(CO3)3

d)

Fe2(CO3)3

51.

Identify the spectator ion(s) in the equation: 2Ag+(aq) + 2NO3–(aq) + 2Na+(aq) + S2–(aq) --> Ag2S(s) + 2Na+(aq) + 2NO3–(aq)

a)

2Ag+(aq) + 2NO3–(aq)

b)

2Na+(aq) + 2NO3–

c)

2Na+(aq) + S2–(aq)

d)

Ag2S(s) + 2Na+(aq

52.

At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?

a)

60 ºC

b)

30 ºC

c)

50 ºC

d)

83 ºC

53.
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
54.

25 grams of NaCl are dissolved in 100 mL of water at 60 C. How many more grams need to be dissolved for the solution to be saturated?

a)

13 grams

b)

25 grams

c)

6 grams

d)

38 grams

55.

How many grams of K2Cr2O7, are soluble in 100 g of water at 90 ºC?

a)

85 grams

b)

70 grams

c)

40 grams

d)

15 grams

56.

How many grams of K2Cr2O7, are soluble in 50 g of water at 90ºC?

a)

70 grams

b)

35 grams

c)

140 grams

d)

105 grams

57.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
58.

How much KNO3 solute is saturated at 40 degrees?

a)

75

b)

55

c)

65

d)

85

59.

How much C12H22O11 solute is saturated at 40 degrees?

a)

240

b)

220

c)

230

d)

250

60.

How much Ce2(SO4)3 solute is saturated at 80 degrees?

a)

20

b)

15

c)

30

d)

2

61.

At what temperature can you fully dissolve 140g of NaNO3?

a)

62

b)

73

c)

81

d)

You cannot determine this

62.

What type of a solution is 60g NaNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

63.

What type of a solution is 100g KNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

64.

Which solution is more concentrated?

Solution 1:

500 mL of water

100 g of salt


Solution 2:

500 mL of water

90 g of salt

a)

Solution 1

b)

Solution 2

c)

They have the same concentration

d)

I have no idea

65.
What is the molarity of 4 grams of sodium chloride (NaCl) in 3,800 mL of solution?
a)
0.018 M
b)
0.018 m
c)
1.052 M
d)
1.052 m
66.
How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?
a)
1.074 mol
b)
62.7 mol
c)
1.07 mol
d)
62.7 grams
67.
What is the molarity of a solution which contains 22.41 grams of NaCl in 50.0 mL of solution?
a)
0.488 M
b)
7.66 M
c)
7.67 M
d)
0.00767 M
68.
How many grams of solute are dissolved in 125.0 mL of 5.00M NaCl?
a)
0.625 g NaCl
b)
36.52 g NaCl
c)
36.5 g NaCl
d)
0.625 mol NaCl
69.
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
70.
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. 
71.
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. 
72.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Supersaturated
d)
Homogeneous solution
73.
What is the molarity of 2.5 mol of NaOH in 12.0 L of solution?
a)
0.21 M
b)
30 M
c)
4.8 M
d)
20.8 M
74.
What is the molarity of 122.5 g of AlCl3 in 1.0 L of solution?
a)
1.225 M
b)
0.92 M
c)
0.1225 M
75.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
76.
What is the concentration, in percent by volume, of 15.3 mL of solute in 2.65 L of solution?
a)
0.58%
b)
0.0058%
c)
5.8%
77.
What is the volume of solution needed to make a 3.5% by volume solution using 2.0mL of solvent?
a)
57 mL
b)
0.57 mL
c)
7 mL
78.
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
79.

How many liters of 0.88 M solution can be made with 25.5 grams of lithium fluoride (LiF)? **Remember to convert grams to another unit**

a)

0.87 L

b)

29 L

c)

1.1 L

d)

0.46 L

80.

If I add water to 100.0 mL of a 0.15 M NaOH solution until the final volume is 150.0 mL, what will the molarity of the diluted solution be?

a)

0.23 M

b)

0.10 M

c)

1.0 x 105 M

d)

1.0 M

81.

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

82.

Which is a characteristic of a base?

a)

tastes sour

b)

found mostly in foods

c)

feels slippery

d)

turn litmus paper red

83.

pH is the measure of the concentration of ______.

a)

Acids

b)

H+ ion

c)

OH- ion

d)

Bases

84.

According to Bronsted-Lowry, what is the definition of an BASE?

a)

a substance that donates a hydrogen (H+) ion

b)

a substance that donates a hydroxide (OH-) ion

c)

a substance that accepts a hydrogen (H+) ion

d)

a substance that accepts a hydroxide (OH-) ion

85.

What is being donated/accepted between conjugate acid-base pairs?

a)

a hydrogen (H+) ion

b)

a hydroxide (OH-) ion

c)

water

d)

a neutron

86.

What is the conjugate base in the following reaction?

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl-

87.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
88.
If a solution is basic which ion will be more present?
a)
H+
b)
K+
c)
OH-
d)
H-
89.

Stronger acids have a pH closer to...

a)

7

b)

0

c)

14

d)

9

90.

Weaker bases have a pH closer to...

a)

8

b)

0

c)

14

d)

4

91.

What would be considered the weakest base?

a)

3

b)

14

c)

8.2

d)

11.6

92.
H2O is amphiprotic, can act as acid or base. Which of the following is TRUE ?
a)
H2O is an acid because it is a proton donor
b)
H2O is an base because it is a proton acceptor
c)
H2O can gain or lose a proton, H+
d)
H2O can easily form hydronium ion, H3O+
93.

Concentration is

a)

the amount of solute in the solvent

b)

the amount of solvent in the solute

c)

a measure of how strong an acid or base is

d)

the size of the particles in a solution

94.

In order to dilute a solution, you need to

a)

add more of the solid

b)

add more water

c)

add more acid/base

d)

reduce the volume

95.
Strong acids and bases...
a)
do not break apart into ions (non-electrolyte)
b)
partially break apart into ions (weak electrolyte)
c)
completely break apart into ions (non-electrolyte)
d)
completely break apart into ions (strong electrolyte)
96.

What is the pH of a solution where the [H+] is 1.0 x 10-11?

a)

11

b)

13

c)

14

d)

1

97.

The system on the left is:

a)

Pure

b)

Diluted

c)

Concentrated

d)

Acidic

98.

The pH of a solution is 8.43. What is the [H3O+]concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

99.

If the [OH-] of a solution is 2.7 x 10-4 M, the pH of the solution is:

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

100.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

101.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
102.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

103.
What are the products of the following reaction?
H2SO4  +  KOH  -->  
a)
HK  +  HSO4
b)
H2O  +  KSO4
c)
H2O  +  K2SO4
d)
H2  +  K2SO4
104.

Complete the following reaction:

HNO3 + Ca(OH)2 -->

a)

Ca(NO3)2 + H2O

b)

Ca +H2O

c)

Ca(NO3)2 + H2

d)

Ca(NO3)2 + H2O + CO2

105.
What element is being Oxidized?
a)
N
b)
H
c)
O
d)
S
106.
What element is being Reduced?
a)
N
b)
H
c)
O
d)
S
107.
What are the coefficients when the equation is balanced?
a)
2 + 3 --> 2 + 3 + 4
b)
1 + 3 --> 1 + 3 + 2
c)
2 + 4 --> 2 + 3 + 2
d)
1 + 1 --> 1 + 1 + 1
108.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
109.
Another name for a "oxidation-reduction" reaction is
a)
chemical reaction
b)
neutralization reaction
c)
redox reaction
d)
nuclear reaction
110.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)
Iron
b)
Fluorine
c)
Oxygen
111.

Defined as the loss of electrons.

a)

oxidation

b)

reduction

c)

redox

d)

OIL RIG

112.

Defined as the gain of electrons.

a)

oxidation

b)

redox

c)

reduction

d)

LEO GER

113.

Cl2 + 2e- --> 2Cl - is an example of:

a)

a chemical reaction

b)

redox

c)

oxidation

d)

reduction

114.

What is a half-reaction of this equation, Na + Cl --> NaCl ?

a)

Cl + e- --> Cl-

b)

Cl - e- --> Cl-

c)

Na --> Na + e-

d)

Na° + Cl°--> Na+1Cl-1

115.

When a gas changes iron (III) oxide to iron (II) oxide, it shows that the gas is

a)

a reducing agent

b)

an oxidizing agent

c)

a combustible gas

d)

a diffusible gas

116.

Which of the following represents oxidation?

a)

C → CH4

b)

Fe3+ → Fe2+

c)

Cl2 → 2Cl-

d)

Zn → ZnO

117.
Which of the following represents reduction?
a)
C →  CO
b)
N2 →  NH3
c)
Zn  →   Zn2+ 
d)
H2 →  H2O
118.

What does displacement mean?

a)

A chemical reaction where a less reactive metal takes the place of a more reactive metal in a compound.

b)

A chemical reaction where a more reactive metal takes the place of a less reactive metal in a compound.

c)

A more reactive metal is removed from a compound.

119.

Magnesium chloride + Sodium → ?

a)

Sodium chloride + Magnesium

b)

Magnesium chloride + Sodium (No change)

c)

Sodium magnesium + Chlorine

120.
Which one of the following equations correctly represents the reaction of silver nitrate with copper metal?
a)
CuNO3(aq) + Ag(s) → Cu(s) + AgNO3(aq)
b)
Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s)
c)
Cu(s) + AgNO3(aq) → CuNO3(aq) + Ag(s)
d)
Cu(s) + Ag(NO3)2(aq) → Cu(NO3)2(aq) + Ag(s)
121.

What will be the reaction if a less reactive metal is added in a solution with a more reactive metal compound?

a)

vigorous reaction

b)

fizzing gas produced

c)

burns moderately

d)

no reaction

122.

Which of the following will NOT undergo a reaction?

a)

zinc metal + zinc oxide

b)

iron metal + copper oxide

c)

zinc metal + iron oxide

d)

magnesium + iron oxide

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