"Chemistry in the Laboratory" by James M. Postma, Julian L. Roberts, J. Leland Hollenberg|
"Chemistry in the Laboratory" by James M. Postma, Julian L. Roberts, J. Leland Hollenberg
Seventh Edition
W. H. Freeman and Company | 2010 | ISBN: 1429219548 9781429219549 | 614 pages | PDF | 5 MB
This edition builds on that legacy while addressing cutting-edge trends in the chemistry laboratory—including forensic chemistry and environmental and green chemistry.
The new edition of Chemistry in the Laboratory offers precise, easy-to-follow instructions, helpful illustrations, and an emphasis throughout on laboratory safety. Again, throughout, a Consider This feature encourages users to expand the principles of the experiment into interesting applications, open-ended experiments, or unexplored corners. Most experiments in the manual can be completed in one lab session, but some can be linked or extended for a multi-lab project.
CONTENTS
Preface
FIRST-DAY INSTRUCTIONS
EXPERIMENT 1: Scientific Measurements
EXPERIMENT 2: Mass and Volume Relationships
EXPERIMENT 3: Forensic Chemistry: Crime Scene Investigation
EXPERIMENT 4: Observing the Reactions of Household Chemicals: Deductive Chemical Reasoning
EXPERIMENT 5: A Cycle of Copper Reactions
EXPERIMENT 6: Synthesis of a Chemical Compound: Making Alum from Aluminum
EXPERIMENT 7: The Chemistry of Oxygen: Basic and Acidic Oxides and the Periodic Table
EXPERIMENT 8: Determination of a Chemical Formula: The Reaction of Iodine with Zinc
EXPERIMENT 9: Determination of a Chemical Formula by Titration: The Reaction of Calcium with Water
STUDY ASSIGNMENT A: The Language of Chemistry: Chemical Nomenclature
EXPERIMENT 10: The Estimation of Avogadro's Number
EXPERIMENT 11: The Molar Volume of Dioxygen and Other Gases
EXPERIMENT 12: The Molar Mass of a Gas: A Reduced Scale Method
EXPERIMENT 13: The Reactivity of Metals with Hydrochloric Acid
EXPERIMENT 14: The Heat Capacity of Metals
EXPERIMENT 15: Enthalpy Changes in Chemical Reactions: Hess's Law
EXPERIMENT 16: The Enthalpy of Combustion of a Vegetable Oil
EXPERIMENT 17: Emission Spectra and the Electronic Structure of Atoms: The Hydrogen Atom Spectrum
EXPERIMENT 18: Ionic and Covalent Bonding: Conductivity of Solutions of Ionic and Covalent Compounds
STUDY ASSIGNMENT B: Writing Lewis Structures
EXPERIMENT 19: Models of Molecular Shapes: VSEPR Theory and Orbital Hybridization
EXPERIMENT 20: Intermolecular Forces: Slime Gel: Making and Killing Slime
EXPERIMENT 21: Liquids and Solids: The Vapor Pressure and Enthalpy of Vaporization of Water: The Enthalpy of Fusion of Water
EXPERIMENT 22: Colligative Properties: The Molar Mass of a Soluble Substance by Freezing-Point Depression
EXPERIMENT 23: Some Examples of Chemical Equilibria: Le Chatelier's Principle
EXPERIMENT 24: Determination of an Equilibrium Constant by Spectrophotometry: The lron(lll)-Thiocyanate Complex Ion
EXPERIMENT 25: Factors Affecting the Rates of Chemical Reactions
EXPERIMENT 26: The Rate of a Chemical Reaction: Chemical Kinetics
EXPERIMENT 27: The pH Scale and Acid-Base Titrations: Standardization of NaOH Solution: The Titration of Vinegar and Stomach Antacids
EXPERIMENT 28: Determination of the Molar Mass and Ionization Constant of a Weak Acid
EXPERIMENT 29: What's in Your Drinking Water? Comparing Tap Water and Bottled Water
EXPERIMENT 30: The Solubility Product Constant of Calcium lodate. Ca(l03)2
EXPERIMENT 31: Identification of the Alkaline Earth and Alkali Metal Ions: Analysis of Cations in Seawater
EXPERIMENT 32: The Qualitative Analysis of Some Common Anions: Analysis of Anions in Seawater
EXPERIMENT 33: An Introduction to Green Chemistry: Making Biodiesel and Soap from Vegetable Oils and Fats
EXPERIMENT 34: Oxidation-Reduction: Electron Transfer Reactions
EXPERIMENT 35: Redox Titrations: The Oxidizing Capacity of a Household: Cleanser or Liquid Bleach
EXPERIMENT 36: Electrochemical Cells
EXPERIMENT 37: Electrochemical Puzzles: Metal Corrosion and Anodic Protection: The Golden Penny Experiment
EXPERIMENT 38: The Chemistry of Some Nonmetals
EXPERIMENT 39: Equilibria of Coordination Compounds
EXPERIMENT 40: Atmospheric Chemistry of Nitrogen Monoxide: Smog and Acid Rain
EXPERIMENT 41: Ozone and the Atmosphere: A Web-Based Activity
EXPERIMENT 42: Ultraviolet Light, Sunscreens, and DNA
EXPERIMENT 43: Natural Radioactivity: The Half-Life of Potassium-40 in Potassium Chloride
APPENDIX: Tables of Data
TABLE 1: The International System (SI) of Units and Conversion Factors
TABLE 2: Fundamental Physical and Mathematical Constants
TABLE 3: Vapor Pressure of Water at Different Temperatures
TABLE 4: Concentration of Desk Acid and Base Solutions
TABLE 5: Color Changes and pH Intervals of Some Important Indicators
TABLE 6: Equilibrium Constants for the Ionization of Acids and Bases (25 °C)
TABLE 7: Equilibrium Constants for the Dissociation of Complex Ions, Amphoteric Hydroxides,and Weak Salts (25 °C)a
TABLE 8: Solubility of Some Common Salts and Hydroxides at Approximately 25 °C
TABLE 9: Solubility Product Constants (18-25 °C)
TABLE 10: Standard Reduction Potentials (25 °C)
TABLE 11: International Atomic Masses (based on C12 = 12 exactly)
TABLE 12: Twelve Principles of Green Chemistry
with TOC BookMarkLinks
[HIDE]
FPost • | • DepositF • | • RGator
UlNet • | • SiBi • | • TuBi[/HIDE]
"Chemistry in the Laboratory" by James M. Postma, Julian L. Roberts, J. Leland Hollenberg
Seventh Edition
W. H. Freeman and Company | 2010 | ISBN: 1429219548 9781429219549 | 614 pages | PDF | 5 MB
This edition builds on that legacy while addressing cutting-edge trends in the chemistry laboratory—including forensic chemistry and environmental and green chemistry.
The new edition of Chemistry in the Laboratory offers precise, easy-to-follow instructions, helpful illustrations, and an emphasis throughout on laboratory safety. Again, throughout, a Consider This feature encourages users to expand the principles of the experiment into interesting applications, open-ended experiments, or unexplored corners. Most experiments in the manual can be completed in one lab session, but some can be linked or extended for a multi-lab project.
CONTENTS
Preface
FIRST-DAY INSTRUCTIONS
EXPERIMENT 1: Scientific Measurements
EXPERIMENT 2: Mass and Volume Relationships
EXPERIMENT 3: Forensic Chemistry: Crime Scene Investigation
EXPERIMENT 4: Observing the Reactions of Household Chemicals: Deductive Chemical Reasoning
EXPERIMENT 5: A Cycle of Copper Reactions
EXPERIMENT 6: Synthesis of a Chemical Compound: Making Alum from Aluminum
EXPERIMENT 7: The Chemistry of Oxygen: Basic and Acidic Oxides and the Periodic Table
EXPERIMENT 8: Determination of a Chemical Formula: The Reaction of Iodine with Zinc
EXPERIMENT 9: Determination of a Chemical Formula by Titration: The Reaction of Calcium with Water
STUDY ASSIGNMENT A: The Language of Chemistry: Chemical Nomenclature
EXPERIMENT 10: The Estimation of Avogadro's Number
EXPERIMENT 11: The Molar Volume of Dioxygen and Other Gases
EXPERIMENT 12: The Molar Mass of a Gas: A Reduced Scale Method
EXPERIMENT 13: The Reactivity of Metals with Hydrochloric Acid
EXPERIMENT 14: The Heat Capacity of Metals
EXPERIMENT 15: Enthalpy Changes in Chemical Reactions: Hess's Law
EXPERIMENT 16: The Enthalpy of Combustion of a Vegetable Oil
EXPERIMENT 17: Emission Spectra and the Electronic Structure of Atoms: The Hydrogen Atom Spectrum
EXPERIMENT 18: Ionic and Covalent Bonding: Conductivity of Solutions of Ionic and Covalent Compounds
STUDY ASSIGNMENT B: Writing Lewis Structures
EXPERIMENT 19: Models of Molecular Shapes: VSEPR Theory and Orbital Hybridization
EXPERIMENT 20: Intermolecular Forces: Slime Gel: Making and Killing Slime
EXPERIMENT 21: Liquids and Solids: The Vapor Pressure and Enthalpy of Vaporization of Water: The Enthalpy of Fusion of Water
EXPERIMENT 22: Colligative Properties: The Molar Mass of a Soluble Substance by Freezing-Point Depression
EXPERIMENT 23: Some Examples of Chemical Equilibria: Le Chatelier's Principle
EXPERIMENT 24: Determination of an Equilibrium Constant by Spectrophotometry: The lron(lll)-Thiocyanate Complex Ion
EXPERIMENT 25: Factors Affecting the Rates of Chemical Reactions
EXPERIMENT 26: The Rate of a Chemical Reaction: Chemical Kinetics
EXPERIMENT 27: The pH Scale and Acid-Base Titrations: Standardization of NaOH Solution: The Titration of Vinegar and Stomach Antacids
EXPERIMENT 28: Determination of the Molar Mass and Ionization Constant of a Weak Acid
EXPERIMENT 29: What's in Your Drinking Water? Comparing Tap Water and Bottled Water
EXPERIMENT 30: The Solubility Product Constant of Calcium lodate. Ca(l03)2
EXPERIMENT 31: Identification of the Alkaline Earth and Alkali Metal Ions: Analysis of Cations in Seawater
EXPERIMENT 32: The Qualitative Analysis of Some Common Anions: Analysis of Anions in Seawater
EXPERIMENT 33: An Introduction to Green Chemistry: Making Biodiesel and Soap from Vegetable Oils and Fats
EXPERIMENT 34: Oxidation-Reduction: Electron Transfer Reactions
EXPERIMENT 35: Redox Titrations: The Oxidizing Capacity of a Household: Cleanser or Liquid Bleach
EXPERIMENT 36: Electrochemical Cells
EXPERIMENT 37: Electrochemical Puzzles: Metal Corrosion and Anodic Protection: The Golden Penny Experiment
EXPERIMENT 38: The Chemistry of Some Nonmetals
EXPERIMENT 39: Equilibria of Coordination Compounds
EXPERIMENT 40: Atmospheric Chemistry of Nitrogen Monoxide: Smog and Acid Rain
EXPERIMENT 41: Ozone and the Atmosphere: A Web-Based Activity
EXPERIMENT 42: Ultraviolet Light, Sunscreens, and DNA
EXPERIMENT 43: Natural Radioactivity: The Half-Life of Potassium-40 in Potassium Chloride
APPENDIX: Tables of Data
TABLE 1: The International System (SI) of Units and Conversion Factors
TABLE 2: Fundamental Physical and Mathematical Constants
TABLE 3: Vapor Pressure of Water at Different Temperatures
TABLE 4: Concentration of Desk Acid and Base Solutions
TABLE 5: Color Changes and pH Intervals of Some Important Indicators
TABLE 6: Equilibrium Constants for the Ionization of Acids and Bases (25 °C)
TABLE 7: Equilibrium Constants for the Dissociation of Complex Ions, Amphoteric Hydroxides,and Weak Salts (25 °C)a
TABLE 8: Solubility of Some Common Salts and Hydroxides at Approximately 25 °C
TABLE 9: Solubility Product Constants (18-25 °C)
TABLE 10: Standard Reduction Potentials (25 °C)
TABLE 11: International Atomic Masses (based on C12 = 12 exactly)
TABLE 12: Twelve Principles of Green Chemistry
with TOC BookMarkLinks
[HIDE]
FPost • | • DepositF • | • RGator
UlNet • | • SiBi • | • TuBi[/HIDE]
