,Solution manual for Foundations of College
Chemistry, 16th Edition Morris Hein
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, CHAPTER 1
AN INTRODUCTION TO CHEMISTRY
SOLUTIONS TO REVIEW QUESTIONS
1. (a) A hypothesis is a tentative explanation of certain facts to provide a basis for
further experimentation. A theory is an explanation of the general principles
of certain phenomena with considerable evidence to support it.
(b) A theory is an explanation of the general principles of certain phenomena with
considerable evidence to support it. A scientific law is a simple statement of
natural phenomena to which no exceptions are known under the given
conditions.
2. (a) hypothesis
(b) hypothesis
(c) observation
(d) theory
(e) observation
(f) scientific law
3. (a) A liquid has a definite volume but not a definite shape.
(b) A gas has an indefinite volume and high compressibility.
(c) A solid has a definite shape.
(d) A liquid has an indefinite shape and slight compressibility.
4. A crystalline solid has a regular, repeating, three-dimensional, geometric pattern.
An amorphous solid does not.
(a) A solid that has a regular, repeating pattern is a crystalline solid.
(b) A plastic solid is amorphous.
(c) A solid that has no regular repeating pattern is amorphous.
(d) Glass is an amorphous solid.
(e) Gold is a crystalline solid.
5. A phase is a homogeneous part of a system separated from other parts by a physical
boundary.
6. There are six phases present.
7. Another name for a homogeneous mixture is solution.
8. Alcohol, mercury, and water are the only liquids in the table which are not mixtures.
Mercury is an element; alcohol and water are compounds.
1
, – Chapter 1 –
9. Air is the only gas mixture found in the table. The other gases are elements or
compounds.
10. Three phases are present within the bottle; solid and liquid are observed visually,
while gas is detected by the immediate odor.
11. The system is heterogeneous as three phases are present.
12. A system containing only one substance is not necessarily homogeneous. Two
phases may be present. Example: ice in water.
13. A system containing two or more substances is not necessarily heterogeneous. In a
solution only one phase is present. Examples: sugar dissolved in water, dilute
sulfuric acid.
14. Homogeneous mixtures contain only one phase, while heterogeneous mixtures
contain two or more phases.
15. (a) sugar, a compound and (c) gold, an element
16. Using the steps of the scientific method to help determine why your cell phone has
stopped working.
(a) Observation: My cell phone has stopped working.
(b) Hypothesis: I think that the battery needs to be recharged.
(c) Experiment: Plug in the phone to recharge the battery and allow
sufficient time for the battery to fully recharge. Turn the
phone back on. The phone now works again.
(d) Theory: The battery in the phone has a limited charge time and
needs to be recharged on a regular basis in order to keep it
in working order.
2
, – Chapter 1 –
SOLUTIONS TO EXERCISES
1. Two states are present; solid and gas.
2. Two states are present; solid and liquid.
3. The photo represents a heterogeneous mixture.
4. The maple leaf represents a heterogeneous mixture.
5. (a) homogeneous
(b) heterogeneous
(c) heterogeneous
(d) heterogeneous
6. (a) homogeneous
(b) homogeneous
(c) heterogeneous
(d) heterogeneous
7. Typical answers could be
Substance Main or Active Ingredient
chocolate syrup high fructose corn syrup
margarine vegetable oil blend
nondairy creamer corn syrup solids
beef bouillon salt
toothpaste sodium fluoride
antibacterial soap triclocarban
first aid spray lidocaine HCl
sunblock lotion ethylhexyl p-methoxycinnamate
8. The steps of the scientific method can be used to predict the outcome of the semester
in the following way:
(a) Collect the facts or data. They include the number of classes you have
enrolled in, the amount of time you will give to each class, the number of
hours required for your off campus job, and the amount of time for social
activities.
(b) Formulate a hypotheses. You predict that the amount of time you have
allocated each week for class work will be sufficient to result in good grades at
the end of the semester.
(c) Plan and do additional experiments to test the hypothesis. In the first two
weeks of the semester keep a record of your performance in each class,
including grades on homework, quizzes, and exams.
(d) Modify the hypothesis. If your grades in any class are not good, your
hypothesis was incorrect. It will be necessary to increase the amount of time
allocated to that class.
3
, – Chapter 1 –
9. (a) water, a pure substance
(b) chicken stock, a mixture
(c) salt, a pure substance
(d) mustard flour, a mixture
10. Hypothesis – The soup is not a good source of nutrition because it contains 12
grams of fat per serving.
Test – Search for the number of grams of fat per day recommended for an adult.
Compare this number to the grams per fat on the label.
11. Observations –
Calcite crystals have the ability to reflect light around an object rendering it
“unseeable”.
“Invisibility cloaks” work only with laser light aimed directly at the crystal.
Hypotheses –
If larger crystals were used, larger objects could be hidden.
These “invisibility cloaks” will improve in the future.
12. (a), (b), Picture (2) best represents a homogeneous mixture. Pictures (1) and (c) (3)
show heterogeneous mixtures, and picture (4) does not show a mixture, as only one
species is present.
Picture (1) likely shows a compound, as one of the components of the mixture is
made up of more than one type of “ball”. Picture (2) shows a component with more
than one part, but the parts seem identical, and therefore it could be representing a
diatomic molecule.
13. (a) two phases, solid and gas
(b) two phases, liquid and gas
(c) two phases, solid and liquid
4
, CHAPTER 2
STANDARDS FOR MEASUREMENT
SOLUTIONS TO REVIEW QUESTIONS
1. The exponent will be positive for a large number and negative for a small number.
2. The exponent will decrease.
3. The last digit in a measurement is uncertain because if the quantity were to be
measured multiple times, the last digit would vary.
4. It must be written in scientific notation as 6.420 × 105 g.
5. Zeroes are significant when they are between nonzero digits or at the end of a
number that includes a decimal point.
6. Rule 1. When the first digit after those you want to retain is 4 or less, that digit and
all others to its right are dropped. The last digit retained is not changed.
Rule 2. When the first digit after those you want to retain is 5 or greater, that digit
and all others to the right of it are dropped and the last digit retained is increased
by one.
7. No, the number of significant digits in the calculated value may not be more than
the number of significant figures in any of the measurements.
8. Yes, the number of significant digits depends on the precision of each of the
individual measurements and the calculated value may have more or fewer
significant figures than the original measurements as long as the precision is no
greater than the measurement with the lowest precision. An example of a
calculation with an increase in significant figures is in Example 2.9.
9. 100 cm = 1 m
1 m 1,000,000,000 nm
1,000,000,000 nm = 1 m (1 cm) = 10,000,000 nm
100 cm m
10. 1000 mg = 1 g
1000 g 1000 mg
1000 g = 1 kg (1 kg ) = 1,000,000 mg
kg g
11. Weight is a measure of how much attraction the earth’s gravity has for an object
(or person). In this case, the farther the astronaut is from the Earth the less
gravitational force is pulling on him or her. Less gravitational attraction means the
astronaut will weigh less. The mass of the astronaut is the amount of matter that
makes up him or her. This does not change as the astronaut moves away from the
Earth.
12. They are equivalent units.
(3.5 in.)
2.54 cm
13. = 8.9 cm
1 in.
14. Heat is a form of energy, while temperature is a measure of the intensity of heat
(how hot the system is).
1
, – Chapter 2 –
15. The number of degrees between the freezing and boiling point of water are
Fahrenheit 180°F
Celsius 100°C
Kelvin 100 K
16. The three materials would sort out according to their densities with the most dense
(mercury) at the bottom and the least dense (glycerin) at the top. In the cylinder,
the solid magnesium would sink in the glycerin and float on the liquid mercury.
17. Order of increasing density: ethyl alcohol, vegetable oil, salt, lead
18. The density of ice must be less than 0.91 g/mL and greater than 0.789 g/mL.
19. The density of water is 1.0 g/mL at approximately 4°C. However, when water
changes from a liquid to a solid at 0°C there is actually an increase in volume. The
density of ice at 0°C is 0.917 g/mL. Therefore, ice floats in water because solid
water is less dense than liquid water.
20. If you collect a container of oxygen gas, you should store it with the mouth up.
Oxygen gas is denser than air.
21. density of gold = 19.3 g/mL density of silver = 10.5 g/mL
1 mL
( 25 g gold ) = 1.3 mL
19.3 g
1 mL 25 g of silver has the greater volume.
( 25 g silver ) = 2.4 mL
10.5 g
2
, – Chapter 2 –
SOLUTIONS TO EXERCISES
1. (a) kilogram = 1000 grams
(b) centimetre = 1/100 of a meter (0.01 m)
(c) microliter = 1/1,000,000 of a liter (0.000001 L)
(d) millimetre = 1/1000 of a meter (0.001 m)
(e) decilitre = 1/10 of a liter (0.1 L)
2. (a) 1000 meters = 1 kilometer (d) 0.01 meter = 1 centimeter
(b) 0.1 gram = 1 decigram (e) 0.001 liter = 1 milliliter
(c) 0.000001 liter = 1 microliter
3. (a) gram = g (d) micrometer = μm
(b) microgram = μg (e) millilitre = mL
(c) centimetre = cm (f) decilitre = dL
4. (a) milligram = mg (e) angstrom= Å
(b) kilogram = kg (f) microlitre = μL
(c) meter = m
(d) nanometer = nm
5. (a) 2050 the first zero is significant; the last zero is not
significant
(b) 9.00 × 102 zeros are significant
(c) 0.0530 the first two zeros are not significant; the last
zero is significant
(d) 0.075 zeros are not significant
(e) 300. zeros are significant
(f) 285.00 zeros are significant
6. (a) 0.005 zeros are not significant
(b) 1500 zeros are not significant
(c) 250. zero is significant
(d) 10.000 zeros are significant
(e) 6.070 × 104 zeros are significant
(f) 0.2300 the first zero is not significant; the last two zeros
are significant
3
, – Chapter 2 –
7. Significant figures
(a) 0.025 (2 sig. fig.) (c) 0.0404 (3 sig. fig.)
(b) 22.4 (3 sig. fig.) (d) 5.50 × 103 (3 sig. fig.)
8. Significant figures
(a) 40.0 (3 sig. fig.) (c) 129,042 (6 sig. fig.)
−3
(b) 0.081 (2 sig. fig.) (d) 4.090 × 10 (4 sig. fig.)
9. Round each of the following numbers to four significant figures:
(a) 47.70 (c) 100.2
(b) 1.026 (d) 16.50
10. Round each of the following numbers to four significant figures:
(a) 0.07794 (c) 5.005
(b) 21.63 (d) 74.29
11. Exponential notation
(a) 6.7 × 104 (c) 7.8 × 10−3
(b) 6.54 × 10−2 (d) 4.11 × 105
12. Exponential notation
(a) 4.56 × 10−2 (c) 4.030 × 101
(b) 4.0822 × 103 (d) 1.2 × 107
13. (a) 12.62
1.5
0.25
14.37 = 14.4
(b) (2.25 × 103)(4.80 × 104) = 10.8 × 107 = 1.08 × 108
( 452 )( 6.2 ) = 195.97 = 2.0×102
(c)
14.3
(d) (0.0394) (12.8) = 0.504
0.4278
(e) = 0.00718 = 7.18×10 −3
59.6
(f) 10.4 + (3.75)(1.5 × 104) = 5.6 × 104
4
Chemistry, 16th Edition Morris Hein
Hello all ,
We have all what you need with best price
Our email :
Our website :
testbanks-store.com
, CHAPTER 1
AN INTRODUCTION TO CHEMISTRY
SOLUTIONS TO REVIEW QUESTIONS
1. (a) A hypothesis is a tentative explanation of certain facts to provide a basis for
further experimentation. A theory is an explanation of the general principles
of certain phenomena with considerable evidence to support it.
(b) A theory is an explanation of the general principles of certain phenomena with
considerable evidence to support it. A scientific law is a simple statement of
natural phenomena to which no exceptions are known under the given
conditions.
2. (a) hypothesis
(b) hypothesis
(c) observation
(d) theory
(e) observation
(f) scientific law
3. (a) A liquid has a definite volume but not a definite shape.
(b) A gas has an indefinite volume and high compressibility.
(c) A solid has a definite shape.
(d) A liquid has an indefinite shape and slight compressibility.
4. A crystalline solid has a regular, repeating, three-dimensional, geometric pattern.
An amorphous solid does not.
(a) A solid that has a regular, repeating pattern is a crystalline solid.
(b) A plastic solid is amorphous.
(c) A solid that has no regular repeating pattern is amorphous.
(d) Glass is an amorphous solid.
(e) Gold is a crystalline solid.
5. A phase is a homogeneous part of a system separated from other parts by a physical
boundary.
6. There are six phases present.
7. Another name for a homogeneous mixture is solution.
8. Alcohol, mercury, and water are the only liquids in the table which are not mixtures.
Mercury is an element; alcohol and water are compounds.
1
, – Chapter 1 –
9. Air is the only gas mixture found in the table. The other gases are elements or
compounds.
10. Three phases are present within the bottle; solid and liquid are observed visually,
while gas is detected by the immediate odor.
11. The system is heterogeneous as three phases are present.
12. A system containing only one substance is not necessarily homogeneous. Two
phases may be present. Example: ice in water.
13. A system containing two or more substances is not necessarily heterogeneous. In a
solution only one phase is present. Examples: sugar dissolved in water, dilute
sulfuric acid.
14. Homogeneous mixtures contain only one phase, while heterogeneous mixtures
contain two or more phases.
15. (a) sugar, a compound and (c) gold, an element
16. Using the steps of the scientific method to help determine why your cell phone has
stopped working.
(a) Observation: My cell phone has stopped working.
(b) Hypothesis: I think that the battery needs to be recharged.
(c) Experiment: Plug in the phone to recharge the battery and allow
sufficient time for the battery to fully recharge. Turn the
phone back on. The phone now works again.
(d) Theory: The battery in the phone has a limited charge time and
needs to be recharged on a regular basis in order to keep it
in working order.
2
, – Chapter 1 –
SOLUTIONS TO EXERCISES
1. Two states are present; solid and gas.
2. Two states are present; solid and liquid.
3. The photo represents a heterogeneous mixture.
4. The maple leaf represents a heterogeneous mixture.
5. (a) homogeneous
(b) heterogeneous
(c) heterogeneous
(d) heterogeneous
6. (a) homogeneous
(b) homogeneous
(c) heterogeneous
(d) heterogeneous
7. Typical answers could be
Substance Main or Active Ingredient
chocolate syrup high fructose corn syrup
margarine vegetable oil blend
nondairy creamer corn syrup solids
beef bouillon salt
toothpaste sodium fluoride
antibacterial soap triclocarban
first aid spray lidocaine HCl
sunblock lotion ethylhexyl p-methoxycinnamate
8. The steps of the scientific method can be used to predict the outcome of the semester
in the following way:
(a) Collect the facts or data. They include the number of classes you have
enrolled in, the amount of time you will give to each class, the number of
hours required for your off campus job, and the amount of time for social
activities.
(b) Formulate a hypotheses. You predict that the amount of time you have
allocated each week for class work will be sufficient to result in good grades at
the end of the semester.
(c) Plan and do additional experiments to test the hypothesis. In the first two
weeks of the semester keep a record of your performance in each class,
including grades on homework, quizzes, and exams.
(d) Modify the hypothesis. If your grades in any class are not good, your
hypothesis was incorrect. It will be necessary to increase the amount of time
allocated to that class.
3
, – Chapter 1 –
9. (a) water, a pure substance
(b) chicken stock, a mixture
(c) salt, a pure substance
(d) mustard flour, a mixture
10. Hypothesis – The soup is not a good source of nutrition because it contains 12
grams of fat per serving.
Test – Search for the number of grams of fat per day recommended for an adult.
Compare this number to the grams per fat on the label.
11. Observations –
Calcite crystals have the ability to reflect light around an object rendering it
“unseeable”.
“Invisibility cloaks” work only with laser light aimed directly at the crystal.
Hypotheses –
If larger crystals were used, larger objects could be hidden.
These “invisibility cloaks” will improve in the future.
12. (a), (b), Picture (2) best represents a homogeneous mixture. Pictures (1) and (c) (3)
show heterogeneous mixtures, and picture (4) does not show a mixture, as only one
species is present.
Picture (1) likely shows a compound, as one of the components of the mixture is
made up of more than one type of “ball”. Picture (2) shows a component with more
than one part, but the parts seem identical, and therefore it could be representing a
diatomic molecule.
13. (a) two phases, solid and gas
(b) two phases, liquid and gas
(c) two phases, solid and liquid
4
, CHAPTER 2
STANDARDS FOR MEASUREMENT
SOLUTIONS TO REVIEW QUESTIONS
1. The exponent will be positive for a large number and negative for a small number.
2. The exponent will decrease.
3. The last digit in a measurement is uncertain because if the quantity were to be
measured multiple times, the last digit would vary.
4. It must be written in scientific notation as 6.420 × 105 g.
5. Zeroes are significant when they are between nonzero digits or at the end of a
number that includes a decimal point.
6. Rule 1. When the first digit after those you want to retain is 4 or less, that digit and
all others to its right are dropped. The last digit retained is not changed.
Rule 2. When the first digit after those you want to retain is 5 or greater, that digit
and all others to the right of it are dropped and the last digit retained is increased
by one.
7. No, the number of significant digits in the calculated value may not be more than
the number of significant figures in any of the measurements.
8. Yes, the number of significant digits depends on the precision of each of the
individual measurements and the calculated value may have more or fewer
significant figures than the original measurements as long as the precision is no
greater than the measurement with the lowest precision. An example of a
calculation with an increase in significant figures is in Example 2.9.
9. 100 cm = 1 m
1 m 1,000,000,000 nm
1,000,000,000 nm = 1 m (1 cm) = 10,000,000 nm
100 cm m
10. 1000 mg = 1 g
1000 g 1000 mg
1000 g = 1 kg (1 kg ) = 1,000,000 mg
kg g
11. Weight is a measure of how much attraction the earth’s gravity has for an object
(or person). In this case, the farther the astronaut is from the Earth the less
gravitational force is pulling on him or her. Less gravitational attraction means the
astronaut will weigh less. The mass of the astronaut is the amount of matter that
makes up him or her. This does not change as the astronaut moves away from the
Earth.
12. They are equivalent units.
(3.5 in.)
2.54 cm
13. = 8.9 cm
1 in.
14. Heat is a form of energy, while temperature is a measure of the intensity of heat
(how hot the system is).
1
, – Chapter 2 –
15. The number of degrees between the freezing and boiling point of water are
Fahrenheit 180°F
Celsius 100°C
Kelvin 100 K
16. The three materials would sort out according to their densities with the most dense
(mercury) at the bottom and the least dense (glycerin) at the top. In the cylinder,
the solid magnesium would sink in the glycerin and float on the liquid mercury.
17. Order of increasing density: ethyl alcohol, vegetable oil, salt, lead
18. The density of ice must be less than 0.91 g/mL and greater than 0.789 g/mL.
19. The density of water is 1.0 g/mL at approximately 4°C. However, when water
changes from a liquid to a solid at 0°C there is actually an increase in volume. The
density of ice at 0°C is 0.917 g/mL. Therefore, ice floats in water because solid
water is less dense than liquid water.
20. If you collect a container of oxygen gas, you should store it with the mouth up.
Oxygen gas is denser than air.
21. density of gold = 19.3 g/mL density of silver = 10.5 g/mL
1 mL
( 25 g gold ) = 1.3 mL
19.3 g
1 mL 25 g of silver has the greater volume.
( 25 g silver ) = 2.4 mL
10.5 g
2
, – Chapter 2 –
SOLUTIONS TO EXERCISES
1. (a) kilogram = 1000 grams
(b) centimetre = 1/100 of a meter (0.01 m)
(c) microliter = 1/1,000,000 of a liter (0.000001 L)
(d) millimetre = 1/1000 of a meter (0.001 m)
(e) decilitre = 1/10 of a liter (0.1 L)
2. (a) 1000 meters = 1 kilometer (d) 0.01 meter = 1 centimeter
(b) 0.1 gram = 1 decigram (e) 0.001 liter = 1 milliliter
(c) 0.000001 liter = 1 microliter
3. (a) gram = g (d) micrometer = μm
(b) microgram = μg (e) millilitre = mL
(c) centimetre = cm (f) decilitre = dL
4. (a) milligram = mg (e) angstrom= Å
(b) kilogram = kg (f) microlitre = μL
(c) meter = m
(d) nanometer = nm
5. (a) 2050 the first zero is significant; the last zero is not
significant
(b) 9.00 × 102 zeros are significant
(c) 0.0530 the first two zeros are not significant; the last
zero is significant
(d) 0.075 zeros are not significant
(e) 300. zeros are significant
(f) 285.00 zeros are significant
6. (a) 0.005 zeros are not significant
(b) 1500 zeros are not significant
(c) 250. zero is significant
(d) 10.000 zeros are significant
(e) 6.070 × 104 zeros are significant
(f) 0.2300 the first zero is not significant; the last two zeros
are significant
3
, – Chapter 2 –
7. Significant figures
(a) 0.025 (2 sig. fig.) (c) 0.0404 (3 sig. fig.)
(b) 22.4 (3 sig. fig.) (d) 5.50 × 103 (3 sig. fig.)
8. Significant figures
(a) 40.0 (3 sig. fig.) (c) 129,042 (6 sig. fig.)
−3
(b) 0.081 (2 sig. fig.) (d) 4.090 × 10 (4 sig. fig.)
9. Round each of the following numbers to four significant figures:
(a) 47.70 (c) 100.2
(b) 1.026 (d) 16.50
10. Round each of the following numbers to four significant figures:
(a) 0.07794 (c) 5.005
(b) 21.63 (d) 74.29
11. Exponential notation
(a) 6.7 × 104 (c) 7.8 × 10−3
(b) 6.54 × 10−2 (d) 4.11 × 105
12. Exponential notation
(a) 4.56 × 10−2 (c) 4.030 × 101
(b) 4.0822 × 103 (d) 1.2 × 107
13. (a) 12.62
1.5
0.25
14.37 = 14.4
(b) (2.25 × 103)(4.80 × 104) = 10.8 × 107 = 1.08 × 108
( 452 )( 6.2 ) = 195.97 = 2.0×102
(c)
14.3
(d) (0.0394) (12.8) = 0.504
0.4278
(e) = 0.00718 = 7.18×10 −3
59.6
(f) 10.4 + (3.75)(1.5 × 104) = 5.6 × 104
4
