{"product_id":"handbook-of-aqueous-electrolyte-thermodynamics-9780816903504","title":"Handbook of Aqueous Electrolyte Thermodynamics","description":"\u003cb\u003eBook Synopsis\u003c\/b\u003e\u003cbr\u003eExpertise in electrolyte systems has become increasingly important in traditional CPI operations, as well as in oil\/gas exploration and production. This book is the source for predicting electrolyte systems behavior, an indispensable do-it-yourself guide, with a blueprint for formulating predictive mathematical electrolyte models, recommended tabular values to use in these models, and annotated bibliographies. The final chapter is a general recipe for formulating complete predictive models for electrolytes, along with a series of worked illustrative examples. It can serve as a useful research and application tool for the practicing process engineer, and as a textbook for the chemical engineering student.\u003cbr\u003e\u003cbr\u003e\u003cb\u003eTable of Contents\u003c\/b\u003e\u003cbr\u003e\u003cb\u003eI. INTRODUCTION.\u003c\/b\u003e  \u003cp\u003e\u003cb\u003eII. THERMODYNAMICS OF SOLUTIONS.\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003eBasic Thermodynamic Functions.\u003c\/p\u003e \u003cp\u003eSolutions – Basic Definitions and Concepts.\u003c\/p\u003e \u003cp\u003eEquilibrium – Necessary Conditions.\u003c\/p\u003e \u003cp\u003eActivities, Activity Coefficients and Standard States.\u003c\/p\u003e \u003cp\u003e\u003cb\u003eIII. EQUILIBRIUM CONSTANTS.\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003eIonic and\/or Reaction Equilibrium in Aqueous Solutions.\u003c\/p\u003e \u003cp\u003eSolubility Equilibria Between Crystals and Saturated Solutions.\u003c\/p\u003e \u003cp\u003eVapor-Liquid Equilibria in Aqueous Solutions.\u003c\/p\u003e \u003cp\u003eTemperature Effects on the Equilibrium Constant.\u003c\/p\u003e \u003cp\u003eEstimating Temperature Effects on Heat Capacity and Other Thermodynamic Properties.\u003c\/p\u003e \u003cp\u003eEquilibrium Constants from Tabulated Data.\u003c\/p\u003e \u003cp\u003ePressure Effects on the Equilibrium Constant.\u003c\/p\u003e \u003cp\u003eAppendix 3.1 – Criss and Cobble Parameters.\u003c\/p\u003e \u003cp\u003e\u003cb\u003eIV. ACTIVITY COEFFICIENTS OF SINGLE STRONG ELECTROLYTES.\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003eHistory.\u003c\/p\u003e \u003cp\u003eBromley’s Method.\u003c\/p\u003e \u003cp\u003eMeissner’s Method.\u003c\/p\u003e \u003cp\u003ePitzer’s Method.\u003c\/p\u003e \u003cp\u003eChen’s Method.\u003c\/p\u003e \u003cp\u003eTemperature Effects.\u003c\/p\u003e \u003cp\u003eApplication.\u003c\/p\u003e \u003cp\u003eBromley’s Extended Equation.\u003c\/p\u003e \u003cp\u003eComparison of Temperature Effect Methods.\u003c\/p\u003e \u003cp\u003eAppendix 4.1 – Values for Guggenheim’s β Parameter.\u003c\/p\u003e \u003cp\u003eTable 1: β Values for Uni-univalent Electrolytes.\u003c\/p\u003e \u003cp\u003eTable 2: β and B Values of Bi-univalent and Uni-bivalent Electrolytes from Freezing Points.\u003c\/p\u003e \u003cp\u003eMethods for Calculating β.\u003c\/p\u003e \u003cp\u003eAppendix 4.2 – Bromley Interaction Parameters.\u003c\/p\u003e \u003cp\u003eTable 1: B Values at 25°C Determined by the Method of Least Squares on Log γ to I=6.0 (or less of limited data).\u003c\/p\u003e \u003cp\u003eTable 2: Individual Ion Values of B and δ in Aqueous Solutions at 25°C.\u003c\/p\u003e \u003cp\u003eTable 3: Bivalent Metal Sulfates at 25°C.\u003c\/p\u003e \u003cp\u003eAppendix 4.4 – Pitzer Parameters,\u003c\/p\u003e \u003cp\u003eTable 1: Inorganic Acids, Bases and Salts of 1-1 Type.\u003c\/p\u003e \u003cp\u003eTable 2: Salts of Carboxylic Acids (1-1 Type).\u003c\/p\u003e \u003cp\u003eTable 3: Tetraalkylammonium Halides.\u003c\/p\u003e \u003cp\u003eTable 4: Sulfonic Acids and Salts (1-1 Type).\u003c\/p\u003e \u003cp\u003eTable 5: Additional 1-1 Type Organic Salts.\u003c\/p\u003e \u003cp\u003eTable 6: Inorganic Compounds of 2-1 Type.\u003c\/p\u003e \u003cp\u003eTable 7: Organic Electrolytes of 2-1 Type.\u003c\/p\u003e \u003cp\u003eTable 8: 3-1 Electrolytes.\u003c\/p\u003e \u003cp\u003eTable 9: 4-1 Electrolytes.\u003c\/p\u003e \u003cp\u003eTable 10: 5-1 Electrolytes.\u003c\/p\u003e \u003cp\u003eTable 11: 2-2 Electrolytes.\u003c\/p\u003e \u003cp\u003eAppendix 4.5 – Pitzer Parameter Derivatives.\u003c\/p\u003e \u003cp\u003eTable 1: Temperature Derivatives of Parameters for 1-1 Electrolytes Evaluated from Calorimetric Data.\u003c\/p\u003e \u003cp\u003eTable 2: Temperature Derivatives of Parameters for 2-1 and 1-2 Electrolytes Evaluated from Calorimetric Data.\u003c\/p\u003e \u003cp\u003eTable 3: Temperature Derivatives of Parameters for 3-1 and 2-2 Electrolytes Evaluated from Calorimetric Parameters.\u003c\/p\u003e \u003cp\u003eAppendix 4-6 Chen Parameters.\u003c\/p\u003e \u003cp\u003eTable: τ Values Fit for Molality Mean Ionic Activity Coefficient Data of Aqueous Electrolytes at 298.15 K.\u003c\/p\u003e \u003cp\u003e\u003cb\u003eV. ACTIVITY COEFFICIENTS OF MULTICOMPONET STRONG ELECTROLYTES.\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003eGuggenheim’s Method for Multicomponent Solutions.\u003c\/p\u003e \u003cp\u003eBromley’s Method for Multicomponent Solutions.\u003c\/p\u003e \u003cp\u003eMeissner’s Method for Multicomponent Solutions.\u003c\/p\u003e \u003cp\u003ePitzer’s Method for Multicomponent Solutions.\u003c\/p\u003e \u003cp\u003eApplication.\u003c\/p\u003e \u003cp\u003ePhase Diagram Calculations.\u003c\/p\u003e \u003cp\u003eAppendix 5.1 – Values for Pitzer’s θ and ψ Parameters.\u003c\/p\u003e \u003cp\u003eTable 1: Parameters for mixed electrolytes with viral coefficient equations (at 25°C).\u003c\/p\u003e \u003cp\u003eTable 2: Parameters for the viral coefficient equations at 25°C,\u003c\/p\u003e \u003cp\u003eTable 3: Parameters for binary mixtures with a common ion at 25°C.\u003c\/p\u003e \u003cp\u003e\u003cb\u003eVI. ACTIVITY COEFFICIENT OF STRONGLY COMPLEXING COMPOUNDS.\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003eIdentification of Complexing Electrolytes.\u003c\/p\u003e \u003cp\u003ePhosphoric Acid.\u003c\/p\u003e \u003cp\u003eSulfuric Acid.\u003c\/p\u003e \u003cp\u003eZinc Chloride.\u003c\/p\u003e \u003cp\u003eFerric Chloride.\u003c\/p\u003e \u003cp\u003eCuprous Chloride.\u003c\/p\u003e \u003cp\u003eCalcium Sulfate.\u003c\/p\u003e \u003cp\u003eSodium Sulfate.\u003c\/p\u003e \u003cp\u003eOther Chloride Complexes.\u003c\/p\u003e \u003cp\u003eActivity Coefficient Methods.\u003c\/p\u003e \u003cp\u003eSummary.\u003c\/p\u003e \u003cp\u003eAppendix 6.1 Cuprous Chloride.\u003c\/p\u003e \u003cp\u003eTable 1a: Interaction Parameters.\u003c\/p\u003e \u003cp\u003eTable 1b: Three Parameter Set.\u003c\/p\u003e \u003cp\u003eTable 2: Equilibrium Constants and Heats of Reaction.\u003c\/p\u003e \u003cp\u003eTable 3a: Equilibrium Constants and Changes in Thermodynamic Properties for Formation of CuC1¯ and CuC1²¯ from CuC1(s) + nC1¯ = CuC1\u003c\/p\u003e \u003cp\u003eTable 3b: Equilibrium Constants and Changes in Thermodynamic Properties for Formation of CuC1¯ and CuC1²¯ from Cu\u003csup\u003e+\u003c\/sup\u003e + nC1¯ = CuC1\u003csub\u003en\u003c\/sub\u003e\u003csub\u003e(n-1\u003c\/sub\u003e.\u003c\/p\u003e \u003cp\u003e\u003cb\u003eVII. ACTIVITY COEFFICIENTS OF WEAK ELECTROLYTES AND MOLECULAR SPECIES.\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003eSetschénow Equation.\u003c\/p\u003e \u003cp\u003ePitzer Based Equations.\u003c\/p\u003e \u003cp\u003ePredictions Based Upon Theoretical Equations.\u003c\/p\u003e \u003cp\u003eAppendix 7.1 – Salting Out Parameters for Phenol in Aqueous Salt Solutions at 25°C Celsius.\u003c\/p\u003e \u003cp\u003eAppendix 7.2 – Salting Out Parameters from Pawlikowski and Prausnitz for Nonpolar Gases in Common Salt Solutions at Moderate Temperatures.\u003c\/p\u003e \u003cp\u003eTable 1: Lennard – Jones Parameters for Nonpolar Gases as Reported by Liabastre (S14).\u003c\/p\u003e \u003cp\u003eTable 2: Salting Out Parameters for Strong Electrolytes in Equation (7.18) at 25°C.\u003c\/p\u003e \u003cp\u003eTable 3: Temperature Dependence of the Salting Out Parameters for Equation (7.19).\u003c\/p\u003e \u003cp\u003eTable 4: Salting Out Parameters for Individual Ions for Equation (7.20).\u003c\/p\u003e \u003cp\u003eTable 5: Temperature Dependence of the Salting Out Constants for Individual Loss.\u003c\/p\u003e \u003cp\u003e\u003cb\u003eVIII. THERMODYNAMIC FUNCTIONS DERIVED FROM ACTIVITY COEFFICIENTS.\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003eDensity.\u003c\/p\u003e \u003cp\u003eEnthalpy.\u003c\/p\u003e \u003cp\u003eExcess Enthalpy.\u003c\/p\u003e \u003cp\u003eExample.\u003c\/p\u003e \u003cp\u003e\u003cb\u003eIX. WORKED EXAMPLES.\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003eModel Formulation.\u003c\/p\u003e \u003cp\u003eObtaining Coefficients.\u003c\/p\u003e \u003cp\u003eModel Solution.\u003c\/p\u003e \u003cp\u003eSpecific Examples.\u003c\/p\u003e \u003cp\u003eAppendix 9.1 – Parameters for Beutier and Renon’s Method.\u003c\/p\u003e \u003cp\u003eTable 1: Temperature fit parameters for equilibrium constants.\u003c\/p\u003e \u003cp\u003eTable 2: Temperature fit parameters for Henry’s constants.\u003c\/p\u003e \u003cp\u003eTable 3: Pitzer ion-ion interaction parameters.\u003c\/p\u003e \u003cp\u003eTable 4: Temperature fit molecule self interaction parameters.\u003c\/p\u003e \u003cp\u003eTable 5: Dielectric effect parameters.\u003c\/p\u003e \u003cp\u003eAppendix 9.2- Parameters for Edwards, Maurer, Newman and Prausnitz Method.\u003c\/p\u003e \u003cp\u003eTable 1: Temperature fit parameters for equilibrium constants.\u003c\/p\u003e \u003cp\u003eTable 2: Temperature fit parameters for Henry’s constants.\u003c\/p\u003e \u003cp\u003eTable 3: Ion-ion interaction parameters.\u003c\/p\u003e \u003cp\u003eTable 4: Temperature fit molecule self interaction parameters.\u003c\/p\u003e \u003cp\u003eTable 5: Molecule-ion interaction parameters.\u003c\/p\u003e \u003cp\u003eAppendix 9.3 - Fugacity Coefficient Calculation.\u003c\/p\u003e \u003cp\u003eTable 1: Pure component parameters.\u003c\/p\u003e \u003cp\u003eTable 2: Nonpolar and polar contribution to parameters α and β for four polar gases.\u003c\/p\u003e \u003cp\u003eTable 3: Interaction parameter \u003csup\u003eα\u003c\/sup\u003e\u003csub\u003e12\u003c\/sub\u003e for polar-nonpolar mixtures.\u003c\/p\u003e \u003cp\u003eTable 4: Parameter\u003csup\u003eα\u003c\/sup\u003e\u003csub\u003e12\u003c\/sub\u003e for binary mixtures of nonpolar gases.\u003c\/p\u003e \u003cp\u003eTable 5: Interaction parameter \u003csup\u003eα\u003c\/sup\u003e\u003csub\u003e12\u003c\/sub\u003e for polar-polar mixtures.\u003c\/p\u003e \u003cp\u003eAppendix 9.4 - Brelvi and O’Connell Correlation for Partial Molar Volumes.\u003c\/p\u003e \u003cp\u003eTable 1: Characteristic Volumes.\u003c\/p\u003e \u003cp\u003eAppendix 9.5 – Gypsum Solubility Study Parameters at 25°C.\u003c\/p\u003e \u003cp\u003eTable 1: Binary solution parameters for the Pitzer equations.\u003c\/p\u003e \u003cp\u003eTable 2: Mixed electrolyte solution parameters for the Pitzer equations.\u003c\/p\u003e \u003cp\u003eTable 3: Gypsum solubility product at 25°C.\u003c\/p\u003e \u003cp\u003eAppendix A. Computer Programs for Solving Equilibria Problems.\u003c\/p\u003e \u003cp\u003eAppendix B. Selected Thermodynamic Data.\u003c\/p\u003e \u003cp\u003eAppendix C. Compiled Thermodynamic Data Sources for Aqueous and Biochemical Systems: An Annotated Bibliography (1930-1983).\u003c\/p\u003e \u003cp\u003eIndex.\u003c\/p\u003e","brand":"John Wiley \u0026 Sons Inc","offers":[{"title":"Default Title","offer_id":49405981196631,"sku":"9780816903504","price":86.36,"currency_code":"GBP","in_stock":true}],"thumbnail_url":"\/\/cdn.shopify.com\/s\/files\/1\/0817\/1739\/5799\/files\/9780816903504.jpg?v=1730494129","url":"https:\/\/bookcurl.com\/products\/handbook-of-aqueous-electrolyte-thermodynamics-9780816903504","provider":"Book Curl","version":"1.0","type":"link"}