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Unit 9 Review - Acid, Base, and Ocean Acidification

Total questions: 90

Worksheet time: 54mins

Name
Class
Date
1.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
2.
When the system X + 2 Y <=> Z has reached equilibrium, which of the following is TRUE?
a)
Forward reaction and Backward reaction stop.
b)
Forward reaction has sped up and backward reaction has slowed down.
c)
Forward and backward reactions occur at the same rate.
d)
Forward reaction has slowed down and backward reaction has sped up.
3.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
4.
Le Chatelier's Principle states that.... 
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
a)
moves to increase the change
b)
moves to counteract the change
c)
does not change
5.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-14
d)
1-20
6.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
7.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
8.
A solution with a pH of 3.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
9.
A solution with a pH of 8.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
10.
According to the pH range which substance is more acidic than lemon juice
a)
Hydrochloric acid
b)
cabbage
c)
milk
11.
Feels slippery.
a)
Acids
b)
Bases
c)
All
12.
Ca(OH)2 is an example of a(n)
a)
Acid
b)
Base
c)
Neutral
13.
A solution with a pH of 7.0 would have...
a)
more H ions than OH ions
b)
more OH ions than H ions
c)
equal number of H and OH ions
d)
None of these.
14.

Which characteristics describe an acid?

a)

tastes sour, litmus indicator turns red

b)

tastes bitter, litmus indicator turns blue

c)

tastes sweet and sour, litmus indicator turns red

d)

tastes sour and bitter, litmus indicator turns blue

15.

Which characteristics describe a base?

a)

tastes sour, litmus indicator turns blue

b)

tastes bitter, litmus indicator turns blue

c)

tastes bitter sour, litmus indicator turns blue green

d)

tastes bitter sour, litmus indicator turns green

16.

Which statement is true?

a)

the lower the pH, the more H+ ions

b)

the higher the pH, the more H+ ions

c)

the lower the pH, the more neutral the acid

d)

the higher the pH, the amount of H+ and OH- ions are equal

17.

A very concentrated acid would have a pH of

a)

1

b)

7

c)

9

d)

14

18.

A dilute alkali would have a pH of

a)

8

b)

7

c)

6

d)

14

19.

When the concentration of hydrogen ions in a solution is decreased by a factor of ten, the pH of the solution

a)

increases by 1

b)

increases by 10

c)

decreases by 1

d)

decreases by 10

20.

Which change in the H⁺ ion concentration of an aqueous solution represents a decrease of one unit on the pH scale?

a)

a tenfold increase

b)

a tenfold decrease

c)

a hundredfold increase

d)

a hundredfold decrease

21.

Which pH change represents a hundredfold increase in the concentration of H₃O⁺?

a)

pH 5 to pH 7

b)

pH 13 to pH 14

c)

pH 3 to pH 1

d)

pH 4 to pH 3

22.

Vinegar, fruit juice, and cola are examples of:

a)

salts

b)

neutral substances

c)

bases

d)

acids

23.
An indicator will ______________ when it is in contact with an acid or base
a)
Bubble
b)
Form a new substance
c)
Change color
d)
Stay the same color
24.

This image demonstrates that

a)

There is a direct correlation with the atmospheric CO2 and the CO2 in seawater

b)

That pH of the ocean increases as the atmospheric CO2 increases

c)

That there is no correlation between pH of the ocean and atmospheric CO2

25.
As the ocean becomes more acidic, the pH of the water
a)
increases
b)
decreases
26.

In a more acidic ocean, the shells of organisms do not grow as easily.

a)

True

b)

False

27.
Marine organisms make their shells from calcium and
a)
chloride
b)
carbonate
c)
seawater
28.

Which statement accurately describes what this graph shows?

a)

As pH decreases, CO32- (carbonate) is less concentrated

b)

As pH increases, CO32- (carbonate) is less concentrated

c)

At pH 6-9, HCO3- is at a low concentration

d)

There is no correlation between carbonate ion concentration & pH

29.

~92% of the carbon dioxide dissolved in the ocean ends up as

a)

Bicarbonate

b)

Carbonic acid

c)

Carbon dioxide

d)

Carbonate

30.

CaCO3 _____ at a lower pH (image is results of an experiment placing the calcium carbonate shells of pterapods in seawater with a pH of 7.8, the projected ocean pH for the year 2100 under current rates of acidification)

a)

dissolves

b)

explodes

c)

increases

d)

is easier to obtain

31.

CO2 + H2O ->

a)

H2CO3

b)

HCO3-

c)

CO32-

d)

CaCO3

32.

Carbon dioxide (CO2) enters the ocean from the ______________________________.

a)

atmosphere

b)

photosynthesis of aquatic plants and algae

c)

melting of sea ice

d)

freezing of seawater

33.

Ocean acidification occurs when too much _______________________________ enters the ocean from the atmosphere.

a)

calcium carbonate

b)

carbon dioxide

c)

sulfur dioxide

d)

nitrogen gas

34.

Carbon dioxide diffuses into the ocean and combines with water (H2O) to form carbonic acid (H2CO3). This ultimately breaks down and releases _________________________ , causing the water to be more acidic.

a)

sodium chloride

b)

calcium carbonate

c)

hydrogen ions

d)

chlorophyll

35.

______________________ is needed by corals, mollusks, sponges, and crustaceans to make their skeletons, shells, spicules, and structures.

a)

calcium carbonate

b)

sodium chloride

c)

carbon dioxide

d)

nitrogen gas

36.

What is the primary reason the ocean is becoming more acidic?

a)

Burning of fossil fuels releasing more CO2

b)

Oil spills from offshore drilling and transport

c)

CO2 seepage from deep seafloor vents

d)

Runoff from chemical plants in coastal areas

37.

What does pH measure (hint: there are two correct answers)?

a)

The acidity of a solution

b)

The amount of water in a solution

c)

How reactive a solution is

d)

How many extra hydrogen ions there are in a solution

38.

This image demonstrates that...

a)

There is a direct correlation with the atmospheric CO2 and the CO2 in seawater

b)

That pH of the ocean increases as the atmospheric CO2 increases

c)

That there is no correlation between pH of the ocean and atmospheric CO2

39.

As the ocean becomes more acidic, the pH of the water...

a)
increases
b)
decreases
40.

In a more acidic ocean, the shells of organisms do not grow as easily.

a)

True

b)

False

41.

Which is the product of this reaction: CO2 + H20 -->

a)

H2CO3

b)

CO3

c)

CO2

d)

H3O+

42.
Carbon dioxide and seawater combine to form
a)
calcium carbonate
b)
carbon monoxide
c)
carbonic acid 
43.
Marine organisms make their shells from calcium and
a)
chloride
b)
carbonate
c)
seawater
44.
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
45.
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
46.

According to this slide

a)

CO2 is causing marine life to die by "poisoning' the water

b)

CO2 is destroying sea shells

c)

CO2 is formed from the combustion of Octane

47.

What do some marine creatures do with the carbonate ion?

a)

use it as a food source

b)

use it as a defense mechanism

c)

use it to build shells and exoskeletons

d)

use it to cool body temperatures

48.

In a more acidic ocean, the shells of organisms do not grow as easily.

a)

True

b)

False

49.

Ocean acidification raises the pH of the ocean .

a)

True

b)

False

50.

Which is carbonate?

a)

HCO-

b)

H2CO3

c)

CO3-

d)

CO2

51.

All carbon dioxide gas found in the ocean is there because humans are causing pollution from burning fossil fuels.

a)

True

b)

False

52.

Carbon dioxide (CO2) enters the ocean from the ______________________________.

a)

atmosphere

b)

photosynthesis of aquatic plants and algae

c)

melting of sea ice

d)

freezing of seawater

53.

Ocean acidification occurs when too much _______________________________ enters the ocean from the atmosphere.

a)

calcium carbonate

b)

carbon dioxide

c)

sulfur dioxide

d)

nitrogen gas

54.

The pH of an acidic solution will be...

a)

Lower then 7

b)

Above 7

c)

Exactly 7

55.

Which best explains why the Ocean is called a carbon sink?

a)
The ocean has no impact on atmospheric carbon levels.
b)
The ocean absorbs and stores carbon dioxide from the atmosphere.
c)
The ocean releases carbon dioxide into the atmosphere.
d)
The ocean is primarily made of salt water, not carbon.
56.

Which best describes the relationship between levels of carbon dioxide in the atmosphere and ocean acidification:

a)
Higher levels of carbon dioxide in the atmosphere lead to increased ocean acidification.
b)
Higher levels of carbon dioxide decrease ocean acidity.
c)
Ocean acidification is unrelated to atmospheric carbon dioxide levels.
d)
Increased ocean temperatures reduce ocean acidification.
57.

Identify two problems associated with increased ocean acidification:

a)
Enhanced oxygen levels in ocean waters.
b)

Harm to marine organisms that rely on calcium carbonate for shells and skeletons.

c)

Decline in coral reef health and growth.

d)
Increased fish populations in coastal areas.
e)
Reduction of plastic pollution in the ocean.
58.

The concerns with ocean acidifcation are all of the following EXCEPT:

a)

a decrease in shell building material

b)

impacts to food webs that rely on marine life like pterapods

c)

increasing global temperatures

d)

impacts to economies who rely on fishing

59.

What does the blue line show?

a)

CO2 in the water

b)

Air temperature

c)

Carbon emissions

d)

pH of the water

60.

What does the orange line show?

a)

CO2 in the water

b)

Air temperature

c)

Carbon emissions

d)

pH of the water

61.

Bases react with

a)

water to produce acids and salts.

b)

salts to produce acids and water.

c)

acids to produce salts and water

d)

neither acids, salts, nor water.

62.

Acids taste

a)

sour.

b)

sweet.

c)

bitter.

d)

salty

63.

When dissolved in water, acids produce _______.

a)

Calcium Ions (C-)

b)

Potassium Ions (K-)

c)

Hydroxide Ions (OH-)

d)

Hydrogen ions (H+)

64.

Acid turns litmus paper ______________.

a)

Purple

b)

Red

c)

Blue

d)

Yellow

65.

Acids usually taste_____________.

a)

Salty

b)

Bitter

c)

Sour

d)

Sweet

66.

Bases contain _________________ when reacting with water.

a)

Hydrogen Ions (H+)

b)

Oxygen Ions (O-)

c)

Hydroxide Ions (OH-)

d)

Sulfur Ions (S+)

67.

Bases turn litmus paper _______________.

a)

Red

b)

Blue

c)

Green

d)

Orange

68.

Solution A would be considered ________________.

a)

Neutral

b)

Acid

c)

Base

69.

Solution B would be considered _____________.

a)

Acid

b)

Base

c)

Neutral

70.

Solution C would be considered ________________.

a)

Acid

b)

Base

c)

Neutral

71.

A strong base is one that is

a)

very corrosive

b)

extremely sour

c)

highly ionized

d)

a good reducing agent

e)

very concentrated

72.

A strong acid is one that

a)

is concentrated

b)

is highly ionized

c)

is very corrosive

d)

tastes very sour

e)

is slippery

73.

The ion associated with a solution which has a bitter taste is

a)

H₃O⁺

b)

H₃O⁻

c)

OH⁻

d)

SO₄²⁻

74.

An acid solution

a)

reacts with all metals

b)

has a bitter taste

c)

has a pH less than 7

d)

affects all indicators

75.

The terms strong and weak refer to

a)

the concentration of the electrolyte

b)

the degree of ionization

c)

the amount of solvent

d)

the number of electron pairs

76.
Which of the following is most likely to be basic:
a)
Lemon juice
b)
Vinegar
c)
Laundry detergent
d)
Coke
77.
When dissolved in water, acids produce:
a)
bases
b)
salts
c)
hydrogen ions
d)
hydroxide ions
78.
Which type of ion does a base produce when it is dissolved in water?
a)
oxide
b)
oxygen
c)
hydrogen
d)
hydroxide
79.

The pH actually measures:

a)

the strength of an acid.

b)

the strength of hydrogen ions.

c)

the concentration of hydrogen ions.

d)

the strength of a base.

80.
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)
81.

Weak 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)
82.

Which of these images shows the strongest base?

a)
b)
c)
83.

What increases the solubility of a gas?

a)

Increasing the temperature of the solvent.

b)

Keeping the temperature of the solvent the same.

c)

Decreasing the temperature of the solvent.

84.

I dissolve some carbon dioxide in water. What will happen to the solubility of the carbon dioxide when I increase the temperature of the water?

a)

It will increase

b)

It will stay the same

c)

It will decrease

85.
Buffer is defined as
a)
ability to resist pH change
b)
ability to prevent pH from decreasing
c)
ability to resist a pH increase
d)

ability to neutralize a reaction

86.

The bicarbonate ions form equilibriums with both carbonic acid and carbonate ions. This allows acids and bases to be added to the ocean without causing much pH change. This makes the ocean water

a)

neutral

b)

easy to change the pH

c)

an indicator

d)

a buffer

87.

Carbonic acid (H2CO3) is

a)

a weak acid

b)

a strong acid

c)

a weak base

d)

a strong base

88.

An acid

a)

has more H30+ ions than H+ ions

b)

has more H30+ ions than OH- ions

c)

has fewer H30+ ions than OH- ions

d)

has equal amounts of H30+ ions and OH- ions

89.

A base

a)

has more H30+ ions than H+ ions

b)

has more H30+ ions than OH- ions

c)

has fewer H30+ ions than OH- ions

d)

has equal amounts of H30+ ions and OH- ions

90.

A neutral solution

a)

has more H30+ ions than H+ ions

b)

has more H30+ ions than OH- ions

c)

has fewer H30+ ions than OH- ions

d)

has equal amounts of H30+ ions and OH- ions

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