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  • Cover

  • Title Page

  • Copyright

  • Contents

  • Chapter 1 Analytical Objectives, or: What Analytical Chemists Do

    • 1.1 What Is Analytical Science?

    • 1.2 Qualitative and Quantitative Analysis: What Does Each Tell Us?

    • 1.3 Getting Started: The Analytical Process

      • Defining the Problem——What do we Really Need to Know? (Not Necessarily Everything)

      • Obtaining a Representative Sample——We Can’t Analyze the Whole Thing

      • Preparing the Sample for Analysis——It Probably Needs to be Altered

      • Performing Necessary Chemical Separations

      • Performing the Measurement——You Decide the Method

      • Instrument Standardization

      • Method of Standard Additions

      • Internal Standard Calibration

      • Calculating the Results and Reporting the Data

    • 1.4 Validation of a Method-You Have to Prove It Works!

    • 1.5 Analyze Versus Determine-They Are Different

    • 1.6 Some Useful Websites

  • Chapter 2 Basic Tools and Operations of Analytical Chemistry

    • 2.1 The Laboratory Notebook-Your Critical Record

    • 2.2 Laboratory Materials and Reagents

    • 2.3 The Analytical Balance-The Indispensible Tool

      • Single-Pan Mechanical Balance

      • Semimicro-And Microbalances

      • Zero-Point Drift

      • Weight in a Vacuum——This is the Ultimate Accuracy

      • Sources of Error in Weighing

      • General Rules for Weighing

      • Weighing of Solids

      • Weighing of Liquids

      • Types of Weighing——What Accuracy do you Need?

    • 2.4 Volumetric Glassware-Also Indispensible

      • Volumetric Flasks

      • Pipets

      • Syringe Pipets

      • Burets

      • Care and Use of Volumetric Glassware

      • General Tips for Accurate and Precise Titrating

      • Tolerances and Precision of Glassware

      • Calibration of Glassware——For the Ultimate Accuracy

      • Techniques for Calibrating Glassware

      • Selection of Glassware——How Accurate Does it have to be?

    • 2.5 Preparation of Standard Base Solutions

    • 2.6 Preparation of Standard Acid Solutions

    • 2.7 Other Apparatus-Handling and Treating Samples

      • Blood Samplers

      • Desiccators

      • Furnaces and Ovens

      • Hoods

      • Wash Bottles

      • Centrifuges and Filters

      • Techniques of Filtration

    • 2.8 Igniting Precipitates-Gravimetric Analysis

    • 2.9 Obtaining the Sample-Is It Solid, Liquid, or Gas?

    • 2.10 Operations of Drying and Preparing a Solution of the Analyte

      • Drying the Sample

      • Sample Dissolution

      • Dissolving Inorganic Solids

      • Destruction of Organic Materials for Inorganic Analysis——Burning or Acid Oxidation

      • Microwave Preparation of Samples

      • Partial Destruction or Nondestruction of Sample Matrix

      • Protein-Free Filtrates

      • Laboratory Techniques for Drying and Dissolving

    • 2.11 Laboratory Safety

  • Chapter 3 Statistics and Data Handling in Analytical Chemistry

    • 3.1 Accuracy and Precision: There Is a Difference

    • 3.2 Determinate Errors-They Are Systematic

    • 3.3 Indeterminate Errors-They Are Random

    • 3.4 Significant Figures: How Many Numbers Do You Need?

      • Absolute and Relative Uncertainty

      • Propagation of Uncertainties

      • Addition and Subtraction——Think Absolute

      • Multiplication and Division——Think Relative

      • Putting it All Together

      • Logarithms——Think Mantissa

    • 3.5 Rounding Off

    • 3.6 Ways of Expressing Accuracy

      • Absolute Errors

      • Relative Error

    • 3.7 Standard Deviation-The Most Important Statistic

    • 3.8 Propagation of Errors-Not Just Additive

      • Addition and Subtraction——Think Absolute Variances

      • Multiplication and Division——Think Relative Variances

    • 3.9 Significant Figures and Propagation of Error

    • 3.10 Control Charts

    • 3.11 The Confidence Limit-How Sure Are You?

    • 3.12 Tests of Significance-Is There a Difference?

      • The Student t-Test——Are there Differences in the Methods?

    • 3.13 Rejection of a Result: The Q Test

    • 3.14 Statistics for Small Data Sets

      • The Median may be Better than the Mean

      • Range Instead of the Standard Deviation

      • Confidence Limits Using the Range

    • 3.15 Linear Least Squares-How to Plot the Right Straight Line

      • Least-Squares Plots

      • Standard Deviations of the Slope and Intercept——They Determine the Unknown Uncertainty

    • 3.16 Correlation Coefficient and Coefficient of Determination

    • 3.17 Detection Limits-There Is No Such Thing as Zero

    • 3.18 Statistics of Sampling-How Many Samples, How Large?

      • The Precision of a Result——Sampling is the key

      • The "True Value"

      • Minimum Sample Size

    • 3.19 Powering a Study: Power Analysis

    • 3.20 Use of Spreadsheets in Analytical Chemistry

      • Filling the Cell Contents

      • Saving the Spreadsheet

      • Printing the Spreadsheet

      • Relative Vs. Absolute Cell References

      • Use of Excel Statistical Functions

      • Useful Syntaxes

      • Text Website Examples

    • 3.21 Using Spreadsheets for Plotting Calibration Curves

    • 3.22 Slope, Intercept, and Coefficient of Determination

    • 3.23 LINEST for Additional Statistics

    • 3.24 Statistics Software Packages

  • Chapter 4 Good Laboratory Practice: Quality Assurance and Method Validation

    • 4.1 What Is Good Laboratory Practice?

    • 4.2 Validation of Analytical Methods

      • Hierarchy of Methodology

      • Validation Process

      • Selectivity

      • Linearity

      • Accuracy

      • Precision

      • Sensitivity

      • Range

      • Limit of Detection (LOD)

      • Limit of Quantitation (LOQ)

      • Ruggedness/Robustness

    • 4.3 Quality Assurance-Does the Method Still Work?

      • Control Charts

      • Documenting and Archiving

      • Proficiency Testing

    • 4.4 Laboratory Accreditation

    • 4.5 Electronic Records and Electronic Signatures: 21 CFR, Part 11

      • Electronic Records

      • Electronic Signatures

      • Epa: Cromerr

    • 4.6 Some Official Organizations

  • Chapter 5 Stoichiometric Calculations: The Workhorse of the Analyst

    • 5.1 Review of the Fundamentals

      • The Basics: Atomic, Molecular, and Formula Weights

      • What is a Dalton?

      • Moles: The Basic Unit for Equating Things

    • 5.2 How Do We Express Concentrations of Solutions?

      • Molarity——The Most Widely Used

      • Normality

      • Formality——Instead of Molarity

      • Molality——The Temperature-Independent Concentration

      • Density Calculations——How do we Convert to Molarity?

      • Analytical and Equilibrium Concentrations——They are not the Same

      • Dilutions——Preparing the Right Concentration

      • More Dilution Calculations

    • 5.3 Expressions of Analytical Results-So Many Ways

      • Solid Samples

      • Liquid Samples

    • 5.4 Volumetric Analysis: How Do We Make Stoichiometric Calculations?

      • Titration——What are the Requirements?

      • Standard Solutions——There are Different Kinds

      • Classification of Titration Methods——What Kinds are there?

    • 5.5 Volumetric Calculations-Let's Use Molarity

      • Some Useful Things to know for Molarity Calculations

      • Standardization and Titration Calculations——They are the Reverse of one Another

      • What if the Analyte and Titrant can React in Different Ratios?

      • If the Reaction is Slow, do a Back-Titration

    • 5.6 Titer-How to Make Rapid Routine Calculations

    • 5.7 Weight Relationships-You Need These for Gravimetric Calculations

  • Chapter 6 General Concepts of Chemical Equilibrium

    • 6.1 Chemical Reactions: The Rate Concept

    • 6.2 Types of Equilibria

    • 6.3 Gibbs Free Energy and the Equilibrium Constant

    • 6.4 Le Cha^telier's Principle

    • 6.5 Temperature Effects on Equilibrium Constants

    • 6.6 Pressure Effects on Equilibria

    • 6.7 Concentration Effects on Equilibria

    • 6.8 Catalysts

    • 6.9 Completeness of Reactions

    • 6.10 Equilibrium Constants for Dissociating or Combining Species-Weak Electrolytes and Precipitates

    • 6.11 Calculations Using Equilibrium Constants-Composition at Equilibrium?

      • Chemical Reactions

      • Excel Goal Seek for Iterative Problem Solving

      • Using Goal Seek to Solve an Equation

      • Dissociation Equilibria

      • Shortcomings of Excel-Based Approaches and how to get around them

    • 6.12 The Common Ion Effect-Shifting the Equilibrium

    • 6.13 Systematic Approach to Equilibrium Calculations-How to Solve Any Equilibrium Problem

      • Mass Balance Equations

      • Charge Balance Equations

      • Equilibrium Calculations Using the Systematic Approach——The Steps

    • 6.14 Some Hints for Applying the Systematic Approach for Equilibrium Calculations

      • Solving Example 6.13 Using Goal Seek

    • 6.15 Heterogeneous Equilibria-Solids Don't Count

    • 6.16 Activity and Activity Coefficients-Concentration Is Not the Whole Story

      • The Activity Coefficient

      • Ionic Strength

      • Calculation of Activity Coefficients

    • 6.17 The Diverse Ion Effect: The Thermodynamic Equilibrium Constant and Activity Coefficients

  • Chapter 7 Acid-Base Equilibria

    • 7.1 The Early History of Acid-BaseConcepts

    • 7.2 Acid-Base Theories-Not All Are Created Equal

      • Arrhenius Theory——H+ and oh−

      • Theory of Solvent Systems——Solvent Cations and Anions

      • Brønsted—Lowry Theory——Taking and Giving Protons

      • Lewis Theory——Taking and Giving Electrons

    • 7.3 Acid-Base Equilibria in Water

    • 7.4 The pH Scale

    • 7.5 pH at Elevated Temperatures: Blood pH

    • 7.6 Weak Acids and Bases-What Is the pH?

    • 7.7 Salts of Weak Acids and Bases-They Aren't Neutral

    • 7.8 Buffers-Keeping the pH Constant (or Nearly So)

    • 7.9 Polyprotic Acids and Their Salts

      • Buffer Calculations for Polyprotic Acids

      • Dissociation Calculations for Polyprotic Acids

    • 7.10 Ladder Diagrams

    • 7.11 Fractions of Dissociating Species at a Given pH: α Values-How Much of Each Species?

    • 7.12 Salts of Polyprotic Acids-Acid, Base, or Both?

    • 7.13 Physiological Buffers-They Keep You Alive

    • 7.14 Buffers for Biological and Clinical Measurements

      • Phosphate Buffers

      • Solving Example 7.24 Using Excel Solver

      • Tris Buffers

      • Good Buffers

    • 7.15 Diverse Ion Effect on Acids and Bases: cKa and cKb-Salts Change the pH

    • 7.16 log C- pH Diagrams

    • 7.17 Exact pH Calculators

  • Chapter 8 Acid-Base Titrations

    • 8.1 Strong Acid versus Strong Base-The Easy Titrations

      • Spreadsheet Exercise——Titrating a Strong Acid With a Strong Base

    • 8.2 The Charge Balance Method-An Excel Exercise for the Titration of a Strong Acid and a Strong Base

    • 8.3 Detection of the End Point: Indicators

    • 8.4 Standard Acid and Base Solutions

    • 8.5 Weak Acid versus Strong Base-A Bit Less Straightforward

      • Spreadsheet Exercise——Weak Acid—Strong Base Titration

    • 8.6 Weak Base versus Strong Acid

    • 8.7 Titration of Sodium Carbonate-A Diprotic Base

    • 8.8 Using a Spreadsheet to Perform the Sodium Carbonate-HCl Titration

    • 8.9 Titration of Polyprotic Acids

    • 8.10 Mixtures of Acids or Bases

    • 8.11 Equivalence Points from Derivatives of a Titration Curve

      • Buffer Intensity

      • Buffer Intensity Computations Depend on the pH Resolution: Buffer Capacity

      • The Second Derivative

    • 8.12 Titration of Amino Acids-They Are Acids and Bases

    • 8.13 Kjeldahl Analysis: Protein Determination

    • 8.14 Titrations Without Measuring Volumes

  • Chapter 9 Complexometric Reactions and Titrations

    • 9.1 Complexes and Formation Constants-How Stable Are Complexes?

    • 9.2 Chelates: EDTA-The Ultimate Titrating Agent for Metals

      • The Chelon Effect——The more Complexing Groups, the Better

      • Edta Equilibria

      • Formation Constant

      • Effect of pH On Edta Equilibria——How Much is Present as Y4−?

      • Conditional Formation Constant——Use for a Fixed pH

    • 9.3 Metal-EDTA Titration Curves

    • 9.4 Detection of the End Point: Indicators-They Are Also Chelating Agents

    • 9.5 Other Uses of Complexes

    • 9.6 Cumulative Formation Constants β and Concentrations of Specific Species in Stepwise Formed Complexes

    • Recommended References

  • Chapter 10 Gravimetric Analysis and Precipitation Equilibria

    • 10.1 How to Perform a Successful Gravimetric Analysis

      • What Steps are Needed?

      • First Prepare the Solution

      • Then do the Precipitation——But Under the Right Conditions

      • Digest the Precipitate to Make Larger and More Pure Crystals

      • Impurities in Precipitates

      • Washing and Filtering the Precipitates——Take Care or you may Lose Some

      • Drying or Igniting the Precipitate

    • 10.2 Gravimetric Calculations-How Much Analyte Is There?

    • 10.3 Examples of Gravimetric Analysis

    • 10.4 Organic Precipitates

    • 10.5 Precipitation Equilibria: The Solubility Product

      • The Saturated Solution

      • Decreasing the Solubility——The Common Ion Effect

      • Solubility Depends on the Stoichiometry

    • 10.6 Diverse Ion Effect on Solubility: Ksp and Activity Coefficients

      • Spreadsheet Examples

  • Chapter 11 Precipitation Reactions and Titrations

    • 11.1 Effect of Acidity on Solubility of Precipitates: Conditional Solubility Product

    • 11.2 Mass Balance Approach for Multiple Equilibria

      • Alternate Goal Seek—Based Solution

    • 11.3 Effect of Complexation on Solubility: Conditional Solubility Product

    • 11.4 Precipitation Titrations

      • Titration Curves——Calculating pX

      • Stepwise Precipitation Titrations

      • Detection of the end Point: Indicators

      • Titration of Sulfate with Barium

  • Chapter 12 Electrochemical Cells and Electrode Potentials

    • 12.1 What Are Redox Reactions?

    • 12.2 Electrochemical Cells-What Electroanalytical Chemists Use

      • Voltaic Cell and Spontaneous Reactions——What is the Cell Potential?

      • Half-Reactions——Giving and Accepting Electrons

      • Half-Reaction Potentials——They are Measured Relative to Each Other

      • What Substances React?

      • Which is the Anode? and Which is the Cathode?

    • 12.3 Nernst Equation-Effects of Concentrations on Potentials

      • Equilibrium Potential——After the Reaction has Occurred

      • Cell Voltage——Before Reaction

    • 12.4 Formal Potential-Use It for Defined Nonstandard Solution Conditions

      • Dependence of Potential on pH

      • Dependence of Potential on Complexation

    • 12.5 Limitations of Electrode Potentials

  • Chapter 13 Potentiometric Electrodes and Potentiometry

    • 13.1 Metal Electrodes for Measuring the Metal Cation

    • 13.2 Metal-Metal Salt Electrodes for Measuring the Salt Anion

    • 13.3 Redox Electrodes-Inert Metals

    • 13.4 Voltaic Cells without Liquid Junction-For Maximum Accuracy

    • 13.5 Voltaic Cells with Liquid Junction-The Practical Kind

      • Liquid-Junction Potential——We Can’t Ignore This

      • How do we Minimize the Liquid-Junction Potential?

    • 13.6 Reference Electrodes: The Saturated Calomel Electrode

    • 13.7 Measurement of Potential

      • The pH Meter

      • The Cell for Potential Measurements

    • 13.8 Determination of Concentrations from Potential Measurements

    • 13.9 Residual Liquid-Junction Potential-It Should Be Minimized

    • 13.10 Accuracy of Direct Potentiometric Measurements-Voltage Error versus Activity Error

    • 13.11 Glass pH Electrode-Workhorse of Chemists

      • Principle of the Glass Electrode

      • Combination pH Electrodes——A Complete cell

      • What Determines the Glass Membrane Potential?

      • Alkaline Error

      • Acid Error

    • 13.12 Standard Buffers-Reference for pH Measurements

    • 13.13 Accuracy of pH Measurements

    • 13.14 Using the pH Meter-How Does It Work?

    • 13.15 pH Measurement of Blood-Temperature Is Important

    • 13.16 pH Measurements in Nonaqueous Solvents

    • 13.17 Ion-Selective Electrodes

      • Glass Membrane Electrodes

      • Solid-State Electrodes

      • Liquid—Liquid Electrodes

      • Plastic Membrane—Ionophore Electrodes

      • Mechanism of Membrane Response

      • Selectivity Coefficient

      • Experimental Methods for Determining Selectivity Coefficients

      • Measurement with Ion-Selective Electrodes

    • 13.18 Chemical Analysis on Mars using Ion-Selective Electrodes

  • Chapter 14 Redox and Potentiometric Titrations

    • 14.1 First: Balance the Reduction-Oxidation Reaction

    • 14.2 Calculation of the Equilibrium Constant of a Reaction-Needed to Calculate Equivalence Point Potentials

    • 14.3 Calculating Redox Titration Curves

    • 14.4 Visual Detection of the End Point

      • Self-Indication

      • Starch Indicator

      • Redox Indicators

    • 14.5 Titrations Involving Iodine: Iodimetry and Iodometry

      • Iodimetry

      • Iodometry

    • 14.6 Titrations with Other Oxidizing Agents

    • 14.7 Titrations with Other Reducing Agents

    • 14.8 Preparing the Solution-Getting the Analyte in the Right Oxidation State before Titration

      • Reduction of the Sample Prior to Titration

      • Oxidation of the Sample Prior to Titration

    • 14.9 Potentiometric Titrations (Indirect Potentiometry)

      • pH Titrations——Using pH Electrodes

      • Precipitation Titrations——Using Silver Electrodes

      • Redox Titrations——Using Platinum Electrodes

      • Ion-Selective Electrodes in Titrations——Measuring pM

      • Derivative Titrations

      • Gran’s Plots for End-Point Detection

      • Automatic Titrators

  • Chapter 15 Voltammetry and Electrochemical Sensors

    • 15.1 Voltammetry

      • The Voltammetric Cell——An Electrolytic Cell

      • The Current—Voltage Curve——The Basis of Voltammetry

      • Stepwise Reduction or Oxidation

      • The Supporting Electrolyte——Needed for Voltammetric Measurements

      • Irreversible Reduction or Oxidation

      • The Working Potential Range——It Depends on the Electrode

    • 15.2 Amperometric Electrodes-Measurement of Oxygen

    • 15.3 Electrochemical Sensors: Chemically Modified Electrodes

      • Enzyme-Based Electrodes for Measuring Substrates

      • Catalytic Electrodes——Redox Mediators

    • 15.4 Ultramicroelectrodes

    • 15.5 Microfabricated Electrochemical Sensors

    • 15.6 Micro and Ultramicroelectrode Arrays

  • Chapter 16 Spectrochemical Methods

    • 16.1 Interaction of Electromagnetic Radiation with Matter

      • The Electromagnetic Spectrum

      • How Does Matter Absorb Radiation?

      • Rotational Transitions

      • Vibrational Transitions

      • Electronic Transitions

      • What Happens to the Absorbed Radiation?

    • 16.2 Electronic Spectra and Molecular Structure

      • Kinds of Transitions

      • Absorption by Isolated Chromophores

      • Absorption by Conjugated Chromophores

      • Absorption by Aromatic Compounds

      • What if a Molecule Does not Absorb Radiation?

      • Inorganic Chelates: How do they Absorb so Intensely?

    • 16.3 Infrared Absorption and Molecular Structure

      • Absorption of Infrared Radiation

      • Infrared Spectra

      • Infrared Spectrometry in Everyday Life

    • 16.4 Near-Infrared Spectrometry for Nondestructive Testing

      • Overtones and Bands——The Basis of Nir Absorption

      • Short- And Long-Wavelength Nir

      • Nir for Nondestructive Testing——How do we Calibrate?

      • Some Uses of Nir Spectrometry

    • 16.5 Spectral Databases-IdentifyingUnknowns

    • 16.6 Solvents for Spectrometry

    • 16.7 Quantitative Calculations

      • Beer’s Law——Relating the Amount of Radiation Absorbed to Concentration

      • Mixtures of Absorbing Species

      • General Solution to the Determination of two Components in a Mixture

      • Quantitative Measurements from Infrared Spectra

    • 16.8 Spectrometric Instrumentation

      • Sources

      • Monochromators

      • Sample Cells

      • Optical Fibers and Liquid Core Waveguide Cells

      • Detectors

      • Slit Width——Physical Vs. Spectral

      • Instrumental Wavelength and Absorbance Calibration

    • 16.9 Types of Instruments

      • Single-Beam Spectrometers

      • Double-Beam Spectrometers

    • 16.10 Array Spectrometers-Getting the Entire Spectrum at Once

    • 16.11 Fourier Transform Infrared Spectrometers

    • 16.12 Near-IR Instruments

    • 16.13 Spectrometric Error in Measurements

    • 16.14 Deviation from Beer's Law

      • Chemical Deviations

      • Instrumental Deviations

    • 16.15 Fluorometry

      • Principles of Fluorescence

      • Chemical Structure and Fluorescence

      • Fluorescence Quenching

      • Relationship Between Concentration and Fluorescence Intensity

      • Fluorescence Instrumentation

      • Fluorescence Lifetime and Gated Fluorescence/Phosphorescence Measurement

      • Fluorescence Vs. Absorbance

    • 16.16 Chemiluminescence

    • 16.17 Fiber-Optic Sensors

  • Chapter 17 Atomic Spectrometric Methods

    • 17.1 Principles: Distribution between Ground and Excited States-Most Atoms Are in the Ground State

    • 17.2 Flame Emission Spectrometry

      • Burners Used for Flame Spectrometry and Desirable Flame Characteristics

      • Flame Processes Occurring in Typical Flame Photometry

    • 17.3 Atomic Absorption Spectrometry

      • Principles of Flame AAS

      • Types Of AAS Instrumentation

      • Light Sources for AAS

      • Analyte Atom Sources

      • Continuum Source AAS Instrumentation

      • Interferences in AAS

    • 17.4 Sample Preparation-Sometimes Minimal

    • 17.5 Internal Standard and Standard Addition Calibration

    • 17.6 Atomic Emission Spectrometry: The Induction Coupled Plasma (ICP)

      • Polychromators and Detectors in ICP-OES

      • Ionization and ICP-MS

      • Laser Ablation ICP-OES/MS

    • 17.7 Atomic Fluorescence Spectrometry

  • Chapter 18 Sample Preparation: Solvent and Solid-Phase Extraction

    • 18.1 Distribution Coefficient

    • 18.2 Distribution Ratio

    • 18.3 Percent Extracted

    • 18.4 Solvent Extraction of Metals

      • Extraction of Ion-Association Complexes

      • Extraction of Metal Chelates

      • Extraction Process for Metal Chelates

    • 18.5 Accelerated and Microwave-Assisted Extraction

    • 18.6 Solid-Phase Extraction

      • SPE Cartridges

      • SPE Pipet Tips

      • SPE Disks

      • 96-Well SPE Plates

      • Other Sorbents for Solid-Phase Extraction

      • Polymeric Phases

      • Dual Phases

    • 18.7 Microextraction

      • Solid-Phase Microextraction (SPME)

      • Liquid-Phase Microextraction (LPME)

    • 18.8 Solid-Phase Nanoextraction (SPNE)

  • Chapter 19 Chromatography: Principles and Theory

    • 19.1 Countercurrent Extraction: The Predecessor to Modern Liquid Chromatography

      • Chromatography and Numerical Simulation

    • 19.2 Principles of Chromatographic Separations

    • 19.3 Classification of Chromatographic Techniques

      • Adsorption Chromatography

      • Partition Chromatography

      • Ion Exchange and Size Exclusion Chromatography

    • 19.4 Theory of Column Efficiency in Chromatography

      • Theoretical Plates

      • Rate Theory of Chromatography——The Van Deemter Equation

      • Reduced Plate Height

      • Open Tubular Columns

      • High-Performance Liquid Chromatography: The Huber and Knox Equations

      • Efficiency and Particle Size in HPLC

      • Retention Factor Efficiency and Resolution

      • Resolution in Chromatography

    • 19.5 Chromatography Simulation Software

  • Chapter 20 Gas Chromatography

    • 20.1 Performing GC Separations

    • 20.2 Gas Chromatography Columns

      • Packed Columns

      • Capillary Columns——The Most Widely Used

      • Stationary Phases——The key to Different Separations

      • Retention Indices for Liquid Stationary Phases

      • Analyte Volatility

    • 20.3 Gas Chromatography Detectors

      • GC-VUV

    • 20.4 Temperature Selection

    • 20.5 Quantitative Measurements

      • Spreadsheet Exercise: Internal Standard Calibration

    • 20.6 Headspace Analysis

    • 20.7 Thermal Desorption

    • 20.8 Purging and Trapping

    • 20.9 Small and Fast

    • 20.10 Separation of Chiral Compounds

    • 20.11 Two-Dimensional GC

  • Chapter 21 Liquid Chromatography and Electrophoresis

    • 21.1 High-Performance Liquid Chromatography

      • Principles

      • HPLC Subclasses

    • 21.2 Stationary Phases in HPLC

    • 21.3 Equipment for HPLC

      • An Important PCR Detection Application: Ion Exchange Separation of Amino Acids

    • 21.4 Ion Chromatography

    • 21.5 HPLC Method Development

    • 21.6 UHPLC and Fast LC

    • 21.7 Open Tubular Liquid Chromatography (OTLC)

    • 21.8 Thin-Layer Chromatography

      • Stationary Phases for TLC/HPTLC

      • Mobile Phases for TLC

      • Sample Application

      • Developing the Chromatogram

      • Visualization. Detection of the Spots

      • Quantitative Measurements

    • 21.9 Electrophoresis

      • Visualization and Quantitation

      • Related Techniques

    • 21.10 Capillary Electrophoresis

      • Operation

      • Detectors in CE

      • How CE can Provide Highly Efficient Separations

      • Electrophoretic Mobility and Separation

      • Plate Numbers and Resolution in CE

    • 21.11 Electrophoresis Related Techniques

      • Separation of Neutral Molecules: MEKC

      • Capillary Electrochromatography

      • Isotachophoresis and Capillary Isotachophoresis

  • Chapter 22 Mass Spectrometry

    • 22.1 Principles of Mass Spectrometry

      • Types of Masses in Mass Spectrometry

      • Resolution

      • Elemental Formula Determination

    • 22.2 Inlets and Ionization Sources

    • 22.3 Gas Chromatography-Mass Spectrometry

    • 22.4 Liquid Chromatography-Mass Spectrometry

    • 22.5 Laser Desorption/Ionization

    • 22.6 Secondary Ion Mass Spectrometry

    • 22.7 Inductively Coupled Plasma-Mass Spectrometry

    • 22.8 Mass Analyzers and Detectors

      • Quadrupole Mass Filter

      • Ion Trap

      • Time-of-Flight

      • Ion Cyclotron Resonance

      • Ion Detectors

    • 22.9 Hybrid Instruments and Tandem Mass Spectrometry

      • Tandem Mass Spectrometry

  • Chapter 23 Kinetic Methods of Analysis

    • 23.1 Kinetics-The Basics

      • First-Order Reactions

      • Second-Order Reactions

      • Reaction Time

    • 23.2 Catalysis

    • 23.3 Enzyme Catalysis

      • Enzyme Kinetics

      • Properties of Enzymes

      • Enzyme Inhibitors and Activators

      • The Michaelis Constant

      • Enzyme Specificity

      • Enzyme Nomenclature

      • Determination of Enzymes

      • Determination of Enzyme Substrates

      • Example Enzymatic Analyses

  • Chapter 24 Automation in Measurements

    • 24.1 Principles of Automation

    • 24.2 Automated Instruments: Process Control

      • Continuous Analyzers

      • Discrete Analyzers

      • Instruments Used in Automated Process Control

    • 24.3 Automatic Instruments

    • 24.4 Flow Injection Analysis

    • 24.5 Sequential Injection Analysis

    • 24.6 Laboratory Information Management Systems

  • Appendix A Literature of Analytical Chemistry

    • A.1 Journals

    • A.2 General References

    • A.3 Inorganic Substances

    • A.4 Organic Substances

    • A.5 Biological and Clinical Substances

    • A.6 Gases

    • A.7 Water and Air Pollutants

    • A.8 Occupational Health and Safety

  • Appendix B Review of Mathematical Operations: Exponents, Logarithms, and the Quadratic Formula

    • B.1 Exponents

    • B.2 Taking Logarithms of Numbers

    • B.3 Finding Numbers from Their Logarithms

    • B.4 Finding Roots with Logarithms

    • B.5 The Quadratic Formula

  • Appendix C Tables of Constants

  • Appendix F Answers to Problems

  • Index

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