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Ocean Acidification Quiz

Total questions: 67

Worksheet time: 48mins

Name
Class
Date
1.
How much of the CO2 in the atmosphere will be absorbed by the oceans?
a)
all of it
b)
1/2
c)
1/4
d)
none of it
2.
Man made carbon dioxide comes from the burning of fossil fuels.  An example of a fossil fuel is
a)
wood
b)
oil
c)
shale
3.
Ocean acidification begins with 
a)
pollution from ships
b)
carbon dioxide released from combustion
c)
dumping of waste from cities into the ocean
4.
Carbon dioxide and seawater combine to form
a)
calcium carbonate
b)
carbon monoxide
c)
carbonic acid 
5.
The H+ ion is a(n)
a)
acid
b)
base
c)
neutral
6.
The process of burning fuel to drive a car or operate a factory is called 
a)
photosynthesis
b)
combustion
c)
respiration
7.
Very slight increases in the acidity of seawater __________  marine organisms that make shells.
a)
doesn't bother
b)
has no effect on 
c)
is unhealthy and stresses
8.
Carbon dioxide levels in the air have changed throughout earth's history.  The difference today is how ______ the change is happening.
a)
rapidly 
b)
slowly 
c)
wide spread
9.
A greenhouse gas which is present in very high quantity is
a)
propane
b)
ethane
c)
CO2
d)
Methane
10.

What happens to 1/4 of the greenhouse gases in the atmosphere?

a)

It is released into space.

b)

It gets absorbed by the ocean.

11.

When carbon dioxide ions react with water, what molecules do they release?

a)

Hydrogen Ions

b)

Carbonate Ions

12.
As the ocean becomes more acidic, the pH of the water
a)
increases
b)
decreases
13.

Ocean acidification raises the pH of the ocean .

a)

True

b)

False

14.

CO2 + H20 -->

a)

H2CO3

b)

CO3

c)

CO2

d)

H3O+

15.

What does a pH of 8.1 mean?

a)

Neutral

b)

weak base

c)

strong base

d)

strong acid

16.

As the pH decreases, what happens to the ocean?

a)

It becomes more acidic.

b)

It becomes more basic.

17.
2A + 3B  <---->  2AB
The forward reaction forms the substance __________.
a)
A
b)
B
c)
AB
d)
A + B
18.
For the reaction...
SO2 + O2  <−>  SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right 
d)
neither left nor right
19.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
20.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If  NO is removed  from the system, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
21.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the temperature is cooled, the _________ reaction will be favored.
a)
forward
b)
reverse
c)
forward and reverse
22.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
23.

What is the effect of increasing the pressure on the following equilibrium: 2NO(g) + O2 (g) ⇌2NO2(g)?

a)

The yield of NO2 increases

b)

The yield of NO2 decreases

c)

The reaction is slower

d)

The concentration of O2 increases.

24.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
25.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
26.
How do catalysts increase the rate of reaction?
a)
The frequency of collisions is the increased
b)
the activation energy is lowered
c)
the energy of collisions is increased
d)
Both the frequency and energy of collisions is increased
27.
2SO2(g)+O2(g)⇌2SO3(g)
Decreasing volume of container will
a)
shift equilibrium right
b)
shift equilibrium left
c)
change K
d)
have no change
28.

PCl3 (g) + Cl2 (g) ↔ PCl5 (g) + energy

Which of the following causes an increase in the moles of PCl5 present at equilibrium shown?

a)

decreasing the volume of the container

b)

raising the temperature

c)

adding a mole of He gas at constant volume

d)

adding a mole of He gas at constant pressure

29.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is removed from the chemical system, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
30.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the pressure in the system is increased, the equilibrium will _______.
a)
shift left
b)
shift right
c)
not shift
31.

H2(g)+Cl2(g)⇌2HCl(g)

The forward reaction is exothermic. What will happen to the equilibrium if the temperature is increased?

a)

equilibrium shifts right

b)

equilibrium shifts left

c)

You cannot predict the effect

d)

no change

32.
Identify the labels (a) and (b) on the graph.
a)
a is concentration of reactants and b is the concentration of product
b)
a is concentration of product and b is the concentration of reactant
c)
a is the volume of reactants and b is the volume of product
d)
a the mass of reactants and b is the mass of product
33.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
d)
plasma
34.
What are the two factors to look for when determining if the reaction is at equilibrium?
a)
Forward reaction rate is faster than the reverse and concentrations are equal
b)
Forward and reverse reaction rates are equal and concentration is constant
c)
Forward and revers reaction rates are equal and concentration is equal
d)
Forward reaction rate is faster than the reverse and concentration is equal
35.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
36.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Stoichiometry
d)
Chemical Reaction
37.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
38.

H2(g)+Cl2(g)⇌2HCl(g)

Removing Cl2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

39.

H2(g)+Cl2(g)⇌2HCl(g)

Increasing the pressure will

a)

shift equilibrium right

b)

shift equilibrium left

c)

You cannot predict the effect

d)

have no change

40.
If an acid is combined with a base of equal strength, the result will most likely be
a)
a neutral solution.
b)
a stronger acid.
c)
impossible to tell without testing the pH.
d)
a stronger base
41.
The pH of a solution is tested, and it is found to be a basic solution. Of the following choices, what could the pH have been?
a)
3
b)
9
c)
7
d)
5
42.
Pure water has a pH of 7. Pure water _______.
a)
is a base
b)
is a neutral substance
c)
could be either an acid or a base
d)
is an acid
43.
Values from 0-14 that determine the acidity of a solution
a)
Punnett Square
b)
Matrix
c)
pH scale
d)
Math number line 
44.
What is the range of pH values in an acidic solution?
a)
0-7
b)
7-14
c)
15-239058204958
d)
pH = 7
45.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13
46.
Which of the following is a basic solution?
a)
household ammonia
b)
HCl dissolved in water
c)
Vinegar
d)
Pure water
47.
Which has a pH below 7?
a)
Acid
b)
Base
48.

What pH is the strongest base?

a)

1

b)

7

c)

4

d)

14

49.
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
a)
strongly acidic
b)
slightly acidic
c)
strongly basic
d)
slightly basic
50.
Which of these pH values would indicate that a solution is a weak base?
a)
4
b)
5.6
c)
8
d)
13
51.
When dissolved in water, acids produce:
a)
bases
b)
salts
c)
hydrogen ions
d)
hydroxide ions
52.
Which type of ion does a base produce when it is dissolved in water?
a)
oxide
b)
oxygen
c)
hydrogen
d)
hydroxide
53.

The pH scale is a range from:

a)

1-7

b)

1-5

c)

0-14

d)

1-14

54.

Neutralization is the process of an acid and a base reacting to form what? Select all that apply

a)

An ionic salt

b)

Hydronium ions

c)

NaCl

d)

Water

55.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
56.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
57.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

58.

What is the concentration of H+ in a solution with a pH of 3?

a)

1.0 x 10-3

b)

3.0 M

c)

10.3 M

d)

103 M

59.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
60.

If the [H+] of a solution is 1 x 10-9 mol/L the pH is

a)

5

b)

-9

c)

9

d)

1

61.

If the [H+] of a solution is 1 x 10-10 mol/L the pOH is

a)

10

b)

4

c)

-10

d)

1

62.

If the [OH-] of a solution is 1 x 10-2 mol/L the pH is

a)

2

b)

-2

c)

12

d)

-12

63.

If the [OH-] of a solution is 1 x 10-3 mol/L the pOH is

a)

3

b)

-3

c)

-11

d)

7

64.

What is the [ H+H^+ ] if the pH is 6

a)

8

b)

1.0x10−61.0x10^{-6}  

c)

1.0x10−81.0x10^{-8}  

d)

6

65.

What is the [OH−]\left[OH^-\right]  of a solution with a pH of 2?

a)

2

b)

1.0x1021.0x10^2  

c)

1.0x10−21.0x10^{-2}  

d)

1.0x10−121.0x10^{-12}  

66.

What is the [OH−]\left[OH^-\right]   of a solution with a pOH of 4?

a)

4

b)

1.0x10−41.0x10^{-4}  

c)

1.0x1041.0x10^4  

d)

1.0x10−101.0x10^{-10}  

67.

What is the [H+]\left[H^+\right]  of a solution with a pOH of 7

a)

7

b)

-7

c)

1.0x10−71.0x10^{-7}  

d)

1.0x1071.0x10^7  

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