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Unit 6- Aqueous Systems

Total questions: 113

Worksheet time: 3hrs 38mins

Name
Class
Date
1.
What is a "homogeneous mixture of two or more substances in a single phase"?
a)
Solution
b)
Solvent
c)
Solute
d)
Compound
2.
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.
3.
What is the unit for molarity?
a)
mass/liters
b)
moles
c)
liters
d)
moles/liter
4.
A measure of the amount of solute in a given amount of solvent or solution is...
a)
saturated
b)
solubility
c)
concentration
d)
miscible
5.
A saturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
6.
A supersaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
7.
An unsaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
8.
An electrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
9.
The dissolving medium in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
10.
The substance dissolved in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
11.
What is the molarity of a 2 liter solution containing 5 moles of NaCl?
a)
2.5
b)
0.4
c)
2.5 moles/liter
d)
10 moles/liter
12.
How many moles of NaCl are present in 6000. ml a 1.5 M NaCl solution?
a)
9 moles NaCl
b)
9000
c)
9
d)
4000  moles NaCl
13.

The process of dissolving a substance in solution

a)

solvotion

b)

salvation

c)

solvation

d)

salvution

14.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

15.

Gases are more soluble at ______temps and _____pressures

a)

high, low

b)

low , high

c)

high, high

d)

low, low

16.

Molarity concentration is abbreviated as _________

a)

MM.

b)

m.

c)

Mol.

d)

M.

17.

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

18.
How does a solution become supersaturated?
a)
dissolve lots of solvent 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. 
19.

How do you know when you have a saturated solution?

a)

You don't see anymore material in the solution. It has dissolved.

b)

The material dissolves and no more will dissolve because you see it collect at the bottom.

c)

The solution is bubbling and cloudy.

d)

The solution is clear and there is nothing at the bottom.

20.

You are given a small beaker of solution at room temp. You add a bit of solute to the solution and it dissolves. The solution was:

a)

saturated

b)

unsaturated

c)

concentrated

d)

warm

21.

In a sample of seawater, the solvent is:

a)

water

b)

sea

c)

salt

d)

air

22.
If you add more sugar to tea that is already saturated (without changing the temperature):
a)
some of the sugar will dissolve
b)
the sugar will fall out of the solution
c)
all of the sugar will dissolve
23.
Which solution is more concentrated?
a)
1 mole of solute in 1 liter of solvent
b)
3 moles of solute in 6 liters of solvent
c)
4 moles of solute in 2 liters of solvent
24.

Which of the following is the strongest base?

a)

oven cleaner - 13.5

b)

lemon juice - 2.5

c)

soap - 10

d)

blood - 7.4

25.

Which of the following is the strongest acid?

a)

oven cleaner - 13.5

b)

lemon juice - 2.5

c)

soap - 10

d)

blood - 7.4

26.

Solutions that have more OH– ions than H+ ions are

a)

acids

b)

bases

c)

enzymes

d)

neutral

27.

Solutions that have more H+ ions than OH- ions are

a)

acids

b)

bases

c)

enzymes

d)

neutral

28.

A scientist runs tests on an unknown substance. He finds that it is extremely corrosive. It produces H+ ions in solution. And, it has a pH of 1. What type of substance has he identified?

a)

weak acid

b)

strong acid

c)

weak base

d)

strong base

29.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

30.

What type of solution is formed when the H+ ions equal the OH- ions?

a)

acidic

b)

basic or alkaline

c)

neutral

d)

enzymatic

31.
Which of these solutions is an acid?
a)
Dish Soap: pH of 12
b)
Tomato Soup: pH of 4
c)
Baking Soda: pH of 9
d)
Drain Cleaner: pH of 14
32.
What does the pH scale measure?
a)
the concentration of acids and bases
b)
the malleability of a metal
c)
the temperature of the water in a swimming pool
d)
the amount of phosphorus in a compound
33.
The pH of vinegar is 2.5.  Vinegar is a _____________.
a)
strong acid
b)
strong base
c)
weak base
d)
weak acid
34.

Which of the following are properties of acids?

a)

They conduct electricity when dissolved in water

b)

They taste sour

c)

They react with metals to produce hydrogen gas

d)

All of the answer choices are correct

35.
What is an "indicator"?
a)
Liquid indicator that changes pink in the presence of a base
b)
A type of paper used to indicate the presence of acids and bases
c)
A chemical that changes color in the presence of acids and changes a different color in the presence of bases
d)
The amount of solute dissolved in solution
36.

Which of the following would be classified as an acid?

a)

NaCl

b)

Ca(OH)2

c)

H2CO3

d)

BaBr2

37.
What is a solution that has an excess of hydroxide (OH-) ions?
a)
pH=6.5
b)
acid
c)
neutral
d)
base
38.

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

a)

KNO3

b)

KBr

c)

NaCl

d)

Yb2(SO4)3

39.

At which temperature do KBr and KNO3 have the same solubility?

a)

60

b)

55

c)

50

d)

Never

40.

At 80'C, KBr's solubility is:

a)

100

b)

90

c)

80

d)

0

41.

At 10'C, NaNO3's solubility is 80 g/100 g of H2O. Based on this information, what would the solubility be in 50 g of H2O.

a)

40

b)

80

c)

160

d)

16

42.

Identify if the following solution would be saturated, unsaturated, or supersaturated: 103 g KBr at 70'C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

43.

How could you change a saturated solution to an unsaturated solution?

a)

Add solvent

b)

Add solute

44.

Identify a method to decrease the dissolving rate of a solution:

a)

decrease the temperature

b)

add KE

c)

stir the solution

d)

increase the temperature

45.

Which substance is least soluble at 0 ºC?

a)

KI

b)

KNO3

c)

KClO3

d)

Ce2(SO4)3

46.

When 40 grams of NaCl is dissolved in 100 grams of water at 90 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

47.
What will allow more solute to be dissolved in a solvent.
a)
adding more solute
b)
stiring
c)
cooling solution
d)
heat
48.

Which would NOT increase the rate at which a sugar cube dissolves?

a)

Reducing the amount of solvent

b)

Crushing the sugar cube

c)

Stirring the solution

d)

Heating the solvent

49.

Three 10 g samples of sugar are represented below.


Sample A dissolves in water more slowly than sample B.

Sample B dissolves more slowly than sample C.

Which of the following best explains why sample A dissolves more slowly than the other two?

a)

It has the most volume.

b)

It has the smallest surface area.

c)

It has the largest number of sugar molecules.

d)

It has the fewest bonds between sugar modules.

50.

A technican prepared a solution by heating 100 mL of distilled water while adding KCl crystals until no more KCl would dissolve. She then capped the clear solution and set it aside on the lab counter. After several hours she noticed the solution had become cloudly and some solid had settled to the bottom of the flask. Which statement best describes what happened?

a)

As the solution cooled, evaporation of water increased the KCl concentration beyond its solubility.

b)

Water molecules, trapped with the KCl crystals, were released after heating.

c)

At lower temperatures the solubility of KCl decreased so some of the solute comes out of solution.

d)

At increased temperatures the solubility of KCl increased and remained too high after cooling.

51.
Which of the following is true about acids and bases?
a)
The lower the pH, the stronger the acid
b)
the higher the pH, the stronger the acid
c)
The lower the pH, the more neutral the acid
d)
The higher the pH, the weaker the base
52.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

53.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

54.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

55.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
56.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
57.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
58.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

59.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
60.
What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?
a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
61.
If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
a)
20.9 mol
b)
0.021 mol
c)
0.02 mol
d)
0.0209 mol
62.
What is the molarity in 650. ml of solution containing 63 grams of sodium chloride?
a)
2.4 M
b)
0.86 M
c)
1.7 M
d)
0.54 M
63.

What is the percent by mass of a solution made by dissolving 20.0 g of NaCl into 180.0 g of water?

a)

10.0 %

b)

11.1 %

c)

80.0 %

d)

20.0 %

64.

What mass of water should be added to 22.0 g of KCl to make 5.50% by mass solution?

a)

400 g

b)

40 g

c)

0.25 g

d)

25 g

65.

How many grams of NaNO3 are needed to prepare 100 g of 15.0 % by mass NaNO3 solution? (MM = 85 g/mol)

a)

15 g

b)

1275 g

c)

12.75 g

d)

150 g

66.

What is the molarity of 0.068 mol of NaCl in 3.8 L of solution?

a)

0.018 M

b)

0.0011 M

c)

1.052 M

d)

0.062 M

67.

How many grams of solute are dissolved in 0.125 L of 5.00 M NaCl (MM = 58.45)?

a)

0.625 g NaCl

b)

625 g NaCl

c)

36.5 g NaCl

d)

0.04 mol NaCl

68.

Calculate the mass percent of solution, if there is 100 g of sugar and 400 g of water

a)

30

b)

25

c)

20

d)

15

69.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

70.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

71.

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

72.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

73.

If the pH of a solution is 8 the [H3O+] is

a)

1.0 x 106 M

b)

8.0 x 101 M

c)

1.0 x 108 M

d)

1.0 x 10-8 M

74.

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

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

75.

If the [H3O+] of a solution is 9.3 x 10-3 M, the pOH of the solution will be

a)

2.03

b)

1.02

c)

11.97

d)

12.98

76.

If a solution has a pOH of 3.7 the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

77.

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

78.

What is the pOH of a solution with [H+] = 1.24 x 10 -2?

a)

1.91

b)

1.61

c)

12.09

d)

12.39

79.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

a)

4.60

b)

2.5

c)

5.0

d)

7

80.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-14 M

c)

1.0 x 10-4 M

d)

1.0 x 10-7 M

81.

What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?

a)

-1.14

b)

1.14

c)

2.01

d)

11.99

82.

What is the [OH-] if the [H+] is 1.0 x 10-3M?

a)

1.0 x 10-3 M

b)

1.0 x 10-14 M

c)

6.02 x 10-23 M

d)

1.0 x 10-11 M

83.

What is the [OH-] if the pH is 4.9?

a)

4.9 x 10-10 M

b)

1.0 x 10-4 M

c)

1.25 x 10-5 M

d)

7.94 x 10-10 M

84.

A solution of KOH is 2.5 x 10-5 M. What is the [H+] concentration? (Hint: Find pOH, then pH, then [H+].)

a)

4.60

b)

9.40

c)

3.98 x 10-10

d)

1.0 x 10-4.60

85.

The pH of a solution is 8.43. What is the hydrogen ion H+ concentration?

a)

3.7 x 10-9 M

b)

2.7 x 10-6 M

c)

1.0 x 10-8.43 M

d)

1.0 x 10-14

86.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
87.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

88.

What is the energy of the activated complex?

a)

75 kJ

b)

225 kJ

c)

300 kJ

d)

50 kJ

89.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
90.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
91.
Why does a higher temperature increase the rate of a reaction?
a)
it increases both the frequency and energy of particle collisions
b)
it only increases the frequency of particle collisions
c)
it only increases the energy of particle collisions
d)
it reduces the activation energy of the reaction
92.
Why does a higher concentration increase the rate of reaction?
a)
it increases the amount of reactants
b)
it lowers the activation energy
c)
it increases the energy of particle collisions
d)
it increases the frequency of particle collisions because there are more collision sites
93.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
94.

In a chemical reaction, how quickly or slowly reactants turn

into products is called the

a)

Catalyst

b)

Reaction Rate

c)

Concentration

d)

Temperature

95.

What is the name given to a catalyst in the human body?

a)

Biology

b)

Catalyst

c)

Chemical

d)

Enzyme

96.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
97.

If the reactant particles collide with less energy than the activation energy, the particles will be rebound, and no reaction will occur.

a)

True

b)

False

98.

The collisions which bring about a chemical reaction are called:

a)

Consistent collisions

b)

Normal collisions

c)

Effective collisions

99.

More collisions correspond to a:

a)

Faster reaction rate

b)

Slower reaction rate

c)

Constant reaction rate

100.
Which of the following is/are the fundamental idea(s) of collision theory?
a)
Molecules react by colliding together
b)
The effective collisions must occur with certain minimum amounts of energy 
c)
In a large sample, the greater the number of effective collisions, and the faster the rate of reaction
d)
All of the above
101.
The rate of a chemical reaction is NOT affected by which of the following:
a)
temperature
b)
concentration
c)
particle size (surface area)
d)
All of these affect reaction rates
102.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
103.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
104.

Catalysts permit reactions to proceed along a ___________energy path.

a)

lower

b)

higher

c)

magnetic

d)

psycho's

105.

Smaller particle size allows for a _________ surface area to be exposed for the reaction.

a)

larger

b)

smaller

c)

rectangular

d)

spherical

106.

Increasing the ____ causes the particles (atoms

or molecules) of the reactants to move more quickly so that

they collide with each other more frequently and with more

energy.

a)

Catalyst

b)

Surface Area

c)

Temperature

d)

Concentration

107.

________ is the measure of how much area of an

object is exposed.

a)

Surface Area

b)

Catalyst

c)

Temperature

d)

Concentration

108.

Grains of sugar have a greater _______ than a solid cube of

sugar of the same mass, and therefore will dissolve quicker in water.

a)

Surface Area

b)

Catalyst

c)

Temperature

d)

Concentratrion

109.

Pick the TWO (2) options that will INCREASE the rate of a reaction.

a)

Reducing Heat

b)

Adding Catalyst

c)

Adding Heat

d)

Removing Catalyst

110.

Which of the following will lower the rate

of reaction?

a)

adding an enzyme to the reaction

b)

decreasing the temperature from 40°C to

10°C

c)

breaking a chunk of calcium up into

smaller pieces

d)

increasing the amount of solute

dissolved in a solution

111.
What is the activation energy of the reverse reaction?
a)
75 kJ
b)
300 kJ
c)
150 kJ
d)
225 kJ
112.
In an endothermic reaction the products have 
a)
more energy than the reactants
b)
less energy than the reactants
c)
the same energy as the reactants
d)
no energy
113.
In an exothermic reaction the products have
a)
more energy than the reactants
b)
the same energy as the reactants
c)
less energy than the reactants
d)
no energy

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