Water Quality Instrumentation : Principles and Practice.

Water Quality Instrumentation provides both a theoretical explanation of how water sensors operate and a more practical discussion of how practitioners should deploy them to best effect. Readers will walk away with an enhanced understanding of the water instrumentation design, operation, and the che...

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Detalles Bibliográficos
Clasificación:Libro Electrónico
Autor principal: Federation, Water Environment
Autor Corporativo: Water Environment Federation (Autor)
Formato: Electrónico eBook
Idioma:Inglés
Publicado: Chicago : Water Environment Federation, 2022.
Temas:
Water quality > Measurement.
Eau > Qualité > Mesure.
Water quality > Measurement
Acceso en línea:Texto completo
Tabla de Contenidos:
  • Front Cover
  • Title Page
  • Copyright
  • About WEF
  • Contents
  • List of Figures
  • List of Tables
  • Preface
  • 1.0 References
  • Chapter 1: Introduction
  • 1.0 Definitions
  • 2.0 The Elemental Truth
  • 3.0 Molecules and Ions
  • 4.0 Chemistry Reactions
  • 5.0 Chemical Recipes
  • 6.0 What Makes Chemistry "Go?"
  • 7.0 References
  • Chapter 2: Oxidation-Reduction Potential
  • 1.0 Why Start with Oxidation-Reduction Potential?
  • 2.0 What ORP Means
  • 3.0 The Electrochemical Cell-Two Halves Make a Whole
  • 4.0 What Really Happens at the Electrode
  • 5.0 The Hydrogen Convention
  • 6.0 The Nernst Equation
  • 7.0 Construction of an ORP Sensor
  • 7.1 The ORP Sensor on Paper
  • 7.2 Constructing an Actual ORP Sensor
  • 7.3 The Combination ORP Probe
  • 7.4 The Differential Probe
  • 8.0 Calibration and Mechanics
  • 8.1 Why Calibration Is a One-Point Exercise
  • 8.2 A Question of Accuracy
  • 8.3 Why ORP Measurements Are Usually Very Slow
  • 8.4 Why pH Measurements Are Temperature Compensated but ORP Measurements Are Not
  • 9.0 The Connection Between pH and ORP?
  • 10.0 ORP Applications
  • 10.1 ORP to Monitor Disinfection
  • 10.2 Monitoring Nitrification and Denitrification
  • 10.3 Phosphorus Removal
  • 10.4 Sulfide Removal
  • 10.5 Methane Production
  • 10.6 Redox Titration for Precise Measurement
  • 10.7 Cyanide Destruction
  • 10.8 Protection Against Corrosion
  • 10.9 The Final Word
  • 11.0 References
  • Chapter 3: pH
  • 1.0 The King of Sensors that is Misunderstood
  • 2.0 Why a Proton Changes Everything
  • 3.0 How a pH Probe Works
  • 3.1 The Secret Ingredient of a pH Probe
  • 3.2 The Connection Between the Nernst Equation and the pH Probe
  • 3.3 Making the Nernst Equation Fit a Proton
  • 3.4 Channeling the Inner Potential
  • 3.5 Adapting to a Differential Probe
  • 4.0 Revisiting Sensor Types
  • 4.1 Separate Electrodes
  • 4.2 The pH Combination Probe.
  • 4.3 The Differential pH Probe
  • 5.0 Calibration
  • 5.1 Two Points (or More)
  • 5.2 Why Calibration Should Be Done at the Same Temperature as the Process
  • 6.0 Things that Affect pH Measurement
  • 6.1 It's the Activity, Not the Concentration
  • 6.2 Temperature Compensation
  • 6.3 A Temperature Effect That Is Real
  • 6.4 Buffer Solutions
  • 6.5 The Diffusion Potential at the Liquid Junction
  • 6.6 The Ever-Changing Reference Electrode
  • 6.7 The Process Electrode in Harm's Way
  • 6.8 Diagnosing a Probe
  • 7.0 The Curse of the Dreaded Ground Loop
  • 7.1 The Key Word Is Loop
  • 7.1.1 Induction
  • 7.1.2 Common Mode Impedance Coupling
  • 7.1.3 What to Do About Ground Loops
  • 7.2 Further Abuse by Static Charge
  • 7.3 Acid and Alkaline Error
  • 7.4 Hydrofluoric Acid
  • 7.5 The pH of Mixed Solvents
  • 7.6 Summary of Probe Issues
  • 8.0 Real World Applications for pH Measurement
  • 8.1 Water Treatment
  • 8.2 Municipal Wastewater Treatment
  • 8.3 Acid Mine Remediation
  • 8.4 Corrosion
  • 8.5 Metal Precipitation
  • 8.6 Industrial Wastewater Treatment
  • 8.7 Scaling-The Problem With High pH
  • 8.8 Water Softening
  • 8.9 Disinfection
  • 8.10 Food and Dairy Production
  • 8.11 Metal Plating
  • 9.0 References
  • Chapter 4: Conductivity
  • 1.0 What it is and Why it Matters
  • 2.0 Let'S Make a Model
  • 2.1 Ohm's Law for Aqueous Solutions
  • 2.2 From Resistance to Conductance to Conductivity
  • 2.3 Conductivity in the Real World of Electrolytes
  • 2.4 Relating Ion Properties to Conductivity Values
  • 2.5 From Conductivity to Ion Mobility
  • 2.6 Salinity-The Third Yardstick
  • 2.7 Conductivity Examples
  • 2.8 Temperature Dependence
  • 3.0 Construction of a Conductivity Sensor
  • 3.1 The Two Electrode Sensor
  • 3.2 Just What Does the Cell Constant Mean?
  • 3.2.1 The Wheatstone Bridge
  • 3.2.2 The Analyzer With a Resistance Readout
  • 3.2.3 The Reference Resistor.
  • 3.3 The Two-Electrode Analyzer
  • 3.4 Linearity and Calibration
  • 3.5 Why the Cable Matters
  • 3.6 The Four Electrode Sensor
  • 3.7 The Toroidal Conductivity Sensor
  • 4.0 Real World Applications
  • 4.1 Water Purity
  • 4.2 Pure Water
  • 4.3 Cooling Towers
  • 4.4 Boiler Feedwater
  • 4.5 Chemical Concentration
  • 4.6 Conductometric Titration
  • 4.7 Leak Detection
  • 5.0 References
  • Chapter 5: Dissolved Oxygen
  • 1.0 Three Parameters that Affect Dissolved Oxygen Concentrations
  • 1.1 From Oxygen in the Air to Oxygen in the Water
  • 1.2 Variation of Dissolved Oxygen Concentration With Air Pressure and Sea Level
  • 1.3 Variation of Dissolved Oxygen Concentration With Temperature
  • 1.4 Variation of Dissolved Oxygen With Dissolved Salts
  • 1.5 Variation of Dissolved Oxygen With Relative Humidity
  • 1.6 A Dissolved Oxygen Sensor Measures Partial Pressure, Not Concentration
  • 2.0 The Grand Unified Theory of Electrochemical Sensors
  • 3.0 The Dissolved Oxygen Amperometric Probe
  • 3.1 The Clark Cell
  • 3.2 Variations on the Clark Theme
  • 3.3 Galvanic Sensor
  • 3.4 The Key Role of Membranes
  • 3.5 Temperature and Membranes
  • 3.6 Clark or Galvanic?
  • 3.7 Interferences
  • 4.0 Optical Dissolved Oxygen Sensors
  • 4.1 The Weird World of Fluorescence
  • 4.2 Ruthenium-The Secret Ingredient
  • 4.3 Making a Difficult Measurement Easy
  • 4.4 Why Calibration of the Optical Dissolved Oxygen Sensor Is a One-Point Exercise
  • 4.5 Comparison Between Electrochemical and Optical Dissolved Oxygen Sensors
  • 5.0 Calibration
  • 6.0 Dissolved Oxygen Probes in the Real World
  • 6.1 Biological Nutrient Removal
  • 6.2 BOD Measurement
  • 6.3 Boiler Water Deaeration
  • 7.0 References
  • Chapter 6: Free Chlorine
  • 1.0 Hypochlorous Acid and Hypochlorite
  • 2.0 Breakpoint Chlorination
  • 3.0 The Dpd Analyzer
  • 3.1 The Wondrous Wurster Red Dye.
  • 3.2 To Measure Total Chlorine Just Add Iodide (and Starch)
  • 3.3 Titration Goes Better With Current Than Color
  • 4.0 The Amperometric Chlorine Analyzer
  • 4.1 The Two-Electrode Sensor
  • 4.2 Total Chlorine
  • 4.3 The Potentiostatic (Three-Electrode) Sensor
  • 5.0 Interferences and Other Sources of Error
  • 6.0 How do ORP Measurements Stack Up Against Free Chlorine Measurements?
  • 7.0 Chlorine Alternatives
  • 7.1 Chlorine's Achilles Heel
  • 7.2 Monochloramine
  • 7.3 Chlorine Dioxide
  • 7.4 Peracetic Acid
  • 7.5 Ozone
  • 7.6 UV and Advanced Oxidation Processes
  • 8.0 References
  • Chapter 7: Turbidity
  • 1.0 Solids in the Water
  • 2.0 How Light Interacts With Suspended Solids
  • 2.1 Photons and Particles
  • 2.2 (Particle) Size Matters
  • 2.3 Light Scattering
  • 3.0 Why Turbidity is in the Eyes of the Beholder (or the Method)
  • 4.0 Different Strategies for Quantifying Turbidity
  • 4.1 The Secchi Disk
  • 4.2 The Jackson Turbidimeter
  • 4.3 A Better Way to Measure Scattering
  • 4.4 Turbidity Units and Standards
  • 5.0 Modern Turbidimeter Design
  • 5.1 The Standard Nephelometric Turbidimeter
  • 5.2 The Near Infrared Alternative
  • 5.3 Sources of Error
  • 5.4 The Ratio Turbidimeter
  • 5.5 The Four-Beam Turbidimeter
  • 5.6 Keeping the Units Straight
  • 5.7 The Submersible (or In Situ) Turbidimeter
  • 5.8 Other Turbidimeter Designs and Methods
  • 6.0 Turbidity in Practice
  • 6.1 Drinking Water
  • 6.2 Pathogen Detection
  • 6.3 Groundwater
  • 6.4 Surface Water
  • 7.0 TSS Measurements and Turbidity
  • 8.0 References
  • Chapter 8: Advanced Electrochemical Sensors-ISEs and Voltammetry
  • 1.0 Ion Selective Electrodes
  • 1.1 Back to the Nernst Equation
  • 1.2 Ionic Sites-The Neglected Costars of Potentiometry
  • 1.3 It's the Activity, Not the Concentration (Again)
  • 1.4 Selectivity-The Lower Limit
  • 1.5 Donnan Failure-The Upper Limit.
  • 1.6 Construction of an Ion Selective Electrode
  • 1.7 Glass ISEs
  • 1.8 Crystalline (Solid State) ISEs-The Fluoride Sensor
  • 1.9 Polymer Membrane ISEs-The Potassium and Ammonia Sensors
  • 1.10 Calibration
  • 1.11 Measurement-Direct or Incremental
  • 2.0 The pH ISFET
  • 2.1 Limitations
  • 3.0 Voltammetry
  • 3.1 Amperometry With a Third Dimension
  • 3.2 Linear Sweep Voltammetry
  • 3.3 Extracting the Standard Potential and Concentration From Voltammogram
  • 3.4 A Real Example
  • 3.5 The Voltametric Advantage
  • 3.6 Polarography
  • 3.7 Variations on a Pulse
  • 3.8 Cyclic Voltammetry
  • 3.9 Stripping Voltammetry
  • 3.10 Rotating Disc Electrode (Hydrodynamic Voltammetry)
  • 3.11 Ion Transfer Stripping Voltammetry
  • 3.12 Summary and Comparison
  • 4.0 References
  • Chapter 9: Organic Matter
  • 1.0 From Bod to Cod
  • 2.0 Toc-Burn and Measure
  • 2.1 Making Carbon Dioxide From Carbon Compounds
  • 2.1.1 UV Oxidation
  • 2.1.2 Supercritical Water Oxidation
  • 2.2 Detection of CO2
  • 2.3 Calibration
  • 2.4 Surrogate Measurements With UV Absorption
  • 3.0 From 254 NM to Beyond-Spectroscopy
  • 3.1 The Spectrometer
  • 3.2 Spectroscopy of Water
  • 3.3 The Spectral Analyzer
  • 3.4 Chemometrics to the Rescue
  • 4.0 References
  • Index.

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