Chemistry
8th Edition by Jill Kirsten Robinson
Complete Chapter Solutions Manual
are included (Ch 1 to 50)
** Immediate Download
** Swift Response
** All Chapters included
** Lab Manuals included
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Table of Contents 1 Chemical Tools: Experimentation and Measurement
Chemistry: Solutions Manual-
1
Eighth Edition
Chemical Tools: Experimentation and Measurement
Chapter 1 Chemical Tools:
Experimentation and
Measurement
Chapter 2 Atoms, Molecules, and
Ions 1.1 5.0 × 10
−8
m; 5.0 × 10
−8
m = 50 × 10
−9
m = 50 nm
Chapter 3 Mass Relationships in
Chemical Reactions
1.2 (a) 7 × 10−5 m
(b) 2 × 1013 kg
Chapter 4 Reactions in Aqueous
Solution 1.3 5 5
°C = × (°F − 32) = × (1474 − 32) = 801 °C
9 9
Chapter 5 Periodicity and the K = °C + 273.15 = 801 + 273.15 = 1074.15 K or 1074 K
Electronic Structure of Atoms
1.4 The melting point of gallium is converted from 302.91 K to °F for comparison.
Chapter 6 Ionic Compounds: °C = K − 273.15 = 302.91 − 273.15 = 29.76 °C
Periodic Trends and Bonding 9 9
Theory °F = ( 5
× °C) + 32 = (
5
× 29.76) + 32 = 85.57 °F
The temperature in the compartment (88 °F) is above the melting point, so the liquid state exists.
Chapter 7 Covalent Bonding and
Electron-Dot Structures
1.5 Volume = 9.37 g ×
1 mL
= 6.32 mL
1.483 g
Chapter 8 Covalent Compounds:
Bonding Theories and Molecular 1.6 Bracelet mass = 80.0 g
Structure
Bracelet volume = 17.61 mL − 10.0 mL = 7.61 mL
80.0 g
Chapter 9 Thermochemistry: Bracelet density =
7.61 mL
= 10.5 g/mL
Chemical Energy
The density of the bracelet matches the density of silver. Since density is one way to identify an unknown substance, it is
likely that the bracelet is made of pure silver.
Chapter 10 Gases: Their
Properties and Behavior
1.7 6.6 × 10
−24
g = 6.6 × 10
−27
kg
Chapter 11 Liquids and Phase 2 −27 1.5×10
7
m
2
−13
kg⋅m
2
−13
EK = 1 1
Changes /2 mv = /2 (6.6 × 10 kg)
( s )
= 7.4 × 10
2
= 7.4 × 10 J
s
Chapter 12 Solids and Solid- 1.8 kg⋅m
2
State Materials 450 g = 0.450 kg; E K = 406 J = 406
s
2
2
EK = 1
/2 mv
Chapter 13 Solutions and Their
Properties ‾2×E
‾‾‾K‾ ‾‾‾‾‾‾‾‾
2×406 kg⋅m‾‾‾
/s ‾
2 2
v = = = 42.5 m/s
√ m √ 0.450 kg
Chapter 14 Chemical Kinetics
Chapter 15 Chemical Equilibrium
Page 1
Chapter 16 Aqueous Equilibria:
Acids and Bases
Chapter 17 Applications of
Aqueous Equilibria
Chapter 18 Thermodynamics:
Entropy, Free Energy, and
Spontaneity
Chapter 19 Electrochemistry
Chapter 20 Nuclear Chemistry
Chapter 21 Transition Elements
and Coordination Chemistry
Chapter 22 The Main-Group
Elements
Chapter 23 Organic and
Biological Chemistry
/
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Table of Contents 1 Chemical Tools: Experimentation and Measurement
Chemistry: Solutions Manual-
Eighth Edition 1.9 (a) 0.003 00 mL has 3 significant figures because zeros at the beginning of a number are not significant and zeros at the
end of a number and after the decimal point are always significant.
Chapter 1 Chemical Tools: (b) 2070 mi has 3 or 4 significant figures because a zero in the middle of a number is significant and a zero at the end of a
Experimentation and number and before the decimal point may or may not be significant.
Measurement (c) 47.60 mL has 4 significant figures because a zero at the end of a number and after the decimal point is always
significant.
Chapter 2 Atoms, Molecules, and
Ions 1.10 To indicate the uncertainty in a measurement, the value you record should use all the digits you are sure of plus one
additional digit that you estimate. The volume can be read to the tenths place and therefore the hundredths place should be
Chapter 3 Mass Relationships in estimated. The volume reported to the correct number of significant figures is 4.55 mL.
Chemical Reactions
1.11 In figure (c) darts are scattered (low precision) and are away from the bull’s-eye (low accuracy).
Chapter 4 Reactions in Aqueous
Solution
1.12 The three measurements are 0.7783 g, 0.7780 g, and 0.7786 g. There is little variation between the three measurements so
Chapter 5 Periodicity and the they have fairly high precision. However, the measurements are all lower than the true value and therefore, the accuracy is
Electronic Structure of Atoms low.
24.567 g
This result should be expressed with 3 decimal places.
Chapter 6 Ionic Compounds: 1.13 (a) + 0.044 78 g Because the digit to be dropped (7) is greater than 5, round up. The result is 24.612 g (5
Periodic Trends and Bonding ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯
significant figures).
Theory 24.611 78 g
Chapter 7 Covalent Bonding and (b) 4.6742 g/0.003 71 L = 1259.89 g/L
Electron-Dot Structures 0.003 71 has only 3 significant figures so the result of the division should have only 3 significant figures. Because the digit
to be dropped (first 9) is greater than 5, round up.
Chapter 8 Covalent Compounds:
The result is 1260 g/L (3 significant figures), or 1.26 × 103 g/L.
Bonding Theories and Molecular
Structure
1.14 NaCl mass = 36.2365 g − 35.6783 g = 0.5582 g
Chapter 9 Thermochemistry: NaCl concentration = 0.5582 g/25.0 mL = 0.0223 g/mL = 2.23 × 10
−2
g/mL
Chemical Energy
1.15 1 carat = 200 mg = 200 × 10
−3
g = 0.200 g
Chapter 10 Gases: Their 0.200 g
Properties and Behavior Mass of Hope Diamond in grams = 44.4 carats ×
1 carat
= 8.88 g
1 ounce = 28.35 g
Chapter 11 Liquids and Phase
1 ounce
Changes Mass of Hope Diamond in ounces = 8.88 g ×
28.35 g
= 0.313 ounces
Chapter 12 Solids and Solid-
1.16 1 cm
3
3
State Materials Volume of Hope Diamond = 8.88 g ×
3.52 g
= 2.52 cm
Chapter 13 Solutions and Their 1.17 4 2 3.28 ft 2
5 2
Properties area = 1.08 × 10 m × (
1m ) = 1.16 × 10 ft
Chapter 14 Chemical Kinetics
Page 2
Chapter 15 Chemical Equilibrium
Chapter 16 Aqueous Equilibria:
Acids and Bases
Chapter 17 Applications of
Aqueous Equilibria
Chapter 18 Thermodynamics:
Entropy, Free Energy, and
Spontaneity
Chapter 19 Electrochemistry
Chapter 20 Nuclear Chemistry
Chapter 21 Transition Elements
and Coordination Chemistry
Chapter 22 The Main-Group
Elements
Chapter 23 Organic and
Biological Chemistry
/
8th Edition by Jill Kirsten Robinson
Complete Chapter Solutions Manual
are included (Ch 1 to 50)
** Immediate Download
** Swift Response
** All Chapters included
** Lab Manuals included
, Skip Directly to Table of Contents | Skip Directly to Main Content
Change text size Show/Hide TOC Page
Table of Contents 1 Chemical Tools: Experimentation and Measurement
Chemistry: Solutions Manual-
1
Eighth Edition
Chemical Tools: Experimentation and Measurement
Chapter 1 Chemical Tools:
Experimentation and
Measurement
Chapter 2 Atoms, Molecules, and
Ions 1.1 5.0 × 10
−8
m; 5.0 × 10
−8
m = 50 × 10
−9
m = 50 nm
Chapter 3 Mass Relationships in
Chemical Reactions
1.2 (a) 7 × 10−5 m
(b) 2 × 1013 kg
Chapter 4 Reactions in Aqueous
Solution 1.3 5 5
°C = × (°F − 32) = × (1474 − 32) = 801 °C
9 9
Chapter 5 Periodicity and the K = °C + 273.15 = 801 + 273.15 = 1074.15 K or 1074 K
Electronic Structure of Atoms
1.4 The melting point of gallium is converted from 302.91 K to °F for comparison.
Chapter 6 Ionic Compounds: °C = K − 273.15 = 302.91 − 273.15 = 29.76 °C
Periodic Trends and Bonding 9 9
Theory °F = ( 5
× °C) + 32 = (
5
× 29.76) + 32 = 85.57 °F
The temperature in the compartment (88 °F) is above the melting point, so the liquid state exists.
Chapter 7 Covalent Bonding and
Electron-Dot Structures
1.5 Volume = 9.37 g ×
1 mL
= 6.32 mL
1.483 g
Chapter 8 Covalent Compounds:
Bonding Theories and Molecular 1.6 Bracelet mass = 80.0 g
Structure
Bracelet volume = 17.61 mL − 10.0 mL = 7.61 mL
80.0 g
Chapter 9 Thermochemistry: Bracelet density =
7.61 mL
= 10.5 g/mL
Chemical Energy
The density of the bracelet matches the density of silver. Since density is one way to identify an unknown substance, it is
likely that the bracelet is made of pure silver.
Chapter 10 Gases: Their
Properties and Behavior
1.7 6.6 × 10
−24
g = 6.6 × 10
−27
kg
Chapter 11 Liquids and Phase 2 −27 1.5×10
7
m
2
−13
kg⋅m
2
−13
EK = 1 1
Changes /2 mv = /2 (6.6 × 10 kg)
( s )
= 7.4 × 10
2
= 7.4 × 10 J
s
Chapter 12 Solids and Solid- 1.8 kg⋅m
2
State Materials 450 g = 0.450 kg; E K = 406 J = 406
s
2
2
EK = 1
/2 mv
Chapter 13 Solutions and Their
Properties ‾2×E
‾‾‾K‾ ‾‾‾‾‾‾‾‾
2×406 kg⋅m‾‾‾
/s ‾
2 2
v = = = 42.5 m/s
√ m √ 0.450 kg
Chapter 14 Chemical Kinetics
Chapter 15 Chemical Equilibrium
Page 1
Chapter 16 Aqueous Equilibria:
Acids and Bases
Chapter 17 Applications of
Aqueous Equilibria
Chapter 18 Thermodynamics:
Entropy, Free Energy, and
Spontaneity
Chapter 19 Electrochemistry
Chapter 20 Nuclear Chemistry
Chapter 21 Transition Elements
and Coordination Chemistry
Chapter 22 The Main-Group
Elements
Chapter 23 Organic and
Biological Chemistry
/
,Copyright 2020 © Pearson Education, Inc. or its affiliate(s). All rights reserved. Privacy Policy | Terms of Use | Rights and Permissions
/
, Skip Directly to Table of Contents | Skip Directly to Main Content
Change text size Show/Hide TOC Page
Table of Contents 1 Chemical Tools: Experimentation and Measurement
Chemistry: Solutions Manual-
Eighth Edition 1.9 (a) 0.003 00 mL has 3 significant figures because zeros at the beginning of a number are not significant and zeros at the
end of a number and after the decimal point are always significant.
Chapter 1 Chemical Tools: (b) 2070 mi has 3 or 4 significant figures because a zero in the middle of a number is significant and a zero at the end of a
Experimentation and number and before the decimal point may or may not be significant.
Measurement (c) 47.60 mL has 4 significant figures because a zero at the end of a number and after the decimal point is always
significant.
Chapter 2 Atoms, Molecules, and
Ions 1.10 To indicate the uncertainty in a measurement, the value you record should use all the digits you are sure of plus one
additional digit that you estimate. The volume can be read to the tenths place and therefore the hundredths place should be
Chapter 3 Mass Relationships in estimated. The volume reported to the correct number of significant figures is 4.55 mL.
Chemical Reactions
1.11 In figure (c) darts are scattered (low precision) and are away from the bull’s-eye (low accuracy).
Chapter 4 Reactions in Aqueous
Solution
1.12 The three measurements are 0.7783 g, 0.7780 g, and 0.7786 g. There is little variation between the three measurements so
Chapter 5 Periodicity and the they have fairly high precision. However, the measurements are all lower than the true value and therefore, the accuracy is
Electronic Structure of Atoms low.
24.567 g
This result should be expressed with 3 decimal places.
Chapter 6 Ionic Compounds: 1.13 (a) + 0.044 78 g Because the digit to be dropped (7) is greater than 5, round up. The result is 24.612 g (5
Periodic Trends and Bonding ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯
significant figures).
Theory 24.611 78 g
Chapter 7 Covalent Bonding and (b) 4.6742 g/0.003 71 L = 1259.89 g/L
Electron-Dot Structures 0.003 71 has only 3 significant figures so the result of the division should have only 3 significant figures. Because the digit
to be dropped (first 9) is greater than 5, round up.
Chapter 8 Covalent Compounds:
The result is 1260 g/L (3 significant figures), or 1.26 × 103 g/L.
Bonding Theories and Molecular
Structure
1.14 NaCl mass = 36.2365 g − 35.6783 g = 0.5582 g
Chapter 9 Thermochemistry: NaCl concentration = 0.5582 g/25.0 mL = 0.0223 g/mL = 2.23 × 10
−2
g/mL
Chemical Energy
1.15 1 carat = 200 mg = 200 × 10
−3
g = 0.200 g
Chapter 10 Gases: Their 0.200 g
Properties and Behavior Mass of Hope Diamond in grams = 44.4 carats ×
1 carat
= 8.88 g
1 ounce = 28.35 g
Chapter 11 Liquids and Phase
1 ounce
Changes Mass of Hope Diamond in ounces = 8.88 g ×
28.35 g
= 0.313 ounces
Chapter 12 Solids and Solid-
1.16 1 cm
3
3
State Materials Volume of Hope Diamond = 8.88 g ×
3.52 g
= 2.52 cm
Chapter 13 Solutions and Their 1.17 4 2 3.28 ft 2
5 2
Properties area = 1.08 × 10 m × (
1m ) = 1.16 × 10 ft
Chapter 14 Chemical Kinetics
Page 2
Chapter 15 Chemical Equilibrium
Chapter 16 Aqueous Equilibria:
Acids and Bases
Chapter 17 Applications of
Aqueous Equilibria
Chapter 18 Thermodynamics:
Entropy, Free Energy, and
Spontaneity
Chapter 19 Electrochemistry
Chapter 20 Nuclear Chemistry
Chapter 21 Transition Elements
and Coordination Chemistry
Chapter 22 The Main-Group
Elements
Chapter 23 Organic and
Biological Chemistry
/
