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- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.13%3A_Additional_ResourcesThe page provides a comprehensive list of references addressing various aspects of equilibrium chemistry. Topics covered include experimental determination of equilibrium constants, the impact of ioni...The page provides a comprehensive list of references addressing various aspects of equilibrium chemistry. Topics covered include experimental determination of equilibrium constants, the impact of ionic strength, solubility products, and buffer capacity. Historical perspectives on the field are also offered. Additionally, the list encompasses instructional strategies, simulations for teaching, and critiques of conventional approaches to equilibrium concepts.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.12%3A_ProblemsThis page contains a comprehensive set of chemistry problems related to equilibrium constants, redox reactions, solubility, acid-base equilibrium, buffer solutions, and complexation reactions. It star...This page contains a comprehensive set of chemistry problems related to equilibrium constants, redox reactions, solubility, acid-base equilibrium, buffer solutions, and complexation reactions. It starts with deriving equilibrium constant expressions for given chemical reactions, analyzing the favorability of reactions using ladder diagrams, and calculating potentials for redox systems.
- https://chem.libretexts.org/Courses/DePaul_University/Physical_Chemistry_for_Biological_Sciences/15%3A_Solutions_II_-_Nonvolatile_Solutes/15.06%3A_The_Debye-Huckel_TheoryDebye and Hückel came up with a theoretical expression that makes is possible to predict mean ionic activity coefficients as sufficiently dilute concentrations. The theory considers the vicinity of ea...Debye and Hückel came up with a theoretical expression that makes is possible to predict mean ionic activity coefficients as sufficiently dilute concentrations. The theory considers the vicinity of each ion as an atmosphere-like cloud of charges of opposite sign that cancels out the charge of the central ion.
- https://chem.libretexts.org/Courses/University_of_Wisconsin_Oshkosh/Chem_370%3A_Physical_Chemistry_1_-_Thermodynamics_(Gutow)/05%3A_Ions_and_Electrochemistry/5.02%3A_The_Debye-Huckel_TheoryDebye and Hückel came up with a theoretical expression that makes is possible to predict mean ionic activity coefficients as sufficiently dilute concentrations. The theory considers the vicinity of ea...Debye and Hückel came up with a theoretical expression that makes is possible to predict mean ionic activity coefficients as sufficiently dilute concentrations. The theory considers the vicinity of each ion as an atmosphere-like cloud of charges of opposite sign that cancels out the charge of the central ion.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/25%3A_Solutions_II_-_Nonvolatile_Solutes/25.06%3A_The_Debye-Huckel_TheoryThis page discusses the challenges of measuring activity coefficients in ionic solutions and presents the Debye-Hückel theory as a solution for predicting these coefficients in dilute concentrations. ...This page discusses the challenges of measuring activity coefficients in ionic solutions and presents the Debye-Hückel theory as a solution for predicting these coefficients in dilute concentrations. It highlights the importance of ionic strength in determining mean activity coefficients and the effects on Debye length.
- https://chem.libretexts.org/Courses/Lakehead_University/Analytical_I/6%3A_Equilibrium_Chemistry/6.09%3A_Activity_EffectsThe activity coefficient for a species corrects for any deviation between its physical and ideal concentration. For a gas, a pure solid, a pure liquid, or a non-ionic solute, the activity coefficient ...The activity coefficient for a species corrects for any deviation between its physical and ideal concentration. For a gas, a pure solid, a pure liquid, or a non-ionic solute, the activity coefficient is approximately one under reasonable experimental conditions. For reactions involving only these species, the difference between activity and concentration is negligible. The activity coefficient for an ion, however, depends on the solution’s ionic strength, the ion’s charge, and the ion’s size.
- https://chem.libretexts.org/Courses/Lebanon_Valley_College/CHM_312%3A_Physical_Chemistry_II_(Lebanon_Valley_College)/08%3A_Electrochemistry/8.02%3A_The_Debye-Huckel_TheoryDebye and Hückel came up with a theoretical expression that makes is possible to predict mean ionic activity coefficients as sufficiently dilute concentrations. The theory considers the vicinity of ea...Debye and Hückel came up with a theoretical expression that makes is possible to predict mean ionic activity coefficients as sufficiently dilute concentrations. The theory considers the vicinity of each ion as an atmosphere-like cloud of charges of opposite sign that cancels out the charge of the central ion.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/26%3A_Chemical_Equilibrium/26.12%3A_Activities_are_Important_for_Ionic_SpeciesThis page discusses the differences between weak and strong electrolytes, highlighting that strong electrolytes can be analyzed with Debye-Hückel theory at low concentrations, while weak electrolytes ...This page discusses the differences between weak and strong electrolytes, highlighting that strong electrolytes can be analyzed with Debye-Hückel theory at low concentrations, while weak electrolytes like acetic acid involve equilibrium, complicating analysis. It covers the calculation of equilibrium constants with activity coefficients and iterative methods for estimating ionic activity.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Map%3A_Physical_Chemistry_for_the_Biosciences_(Chang)/05%3A_Solutions/5.08%3A_Ionic_ActivityThe behavior of an electrolyte solution deviates considerably from that an ideal solution. Indeed, this is why we utilize the activity of the individual components and not the concentration to calcula...The behavior of an electrolyte solution deviates considerably from that an ideal solution. Indeed, this is why we utilize the activity of the individual components and not the concentration to calculate deviations from ideal behavior. In 1923, Peter Debye and Erich Hückel developed a theory that would allow us to calculate the mean ionic activity coefficient of the solution and could explain how the behavior of ions in solution contribute to this constant.
- https://chem.libretexts.org/Courses/Millersville_University/CHEM_341-_Physical_Chemistry_I/07%3A_Mixtures_and_Solutions/7.08%3A_Non-ideality_in_Solutions_-_ActivityThe bulk of the discussion in this chapter dealt with ideal solutions. However, real solutions will deviate from this kind of behavior. So much as in the case of gases, where fugacity was introduced t...The bulk of the discussion in this chapter dealt with ideal solutions. However, real solutions will deviate from this kind of behavior. So much as in the case of gases, where fugacity was introduced to allow us to use the ideal models, activity is used to allow for the deviation of real solutes from limiting ideal behavior.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Thermodynamics_and_Chemical_Equilibrium_(Ellgen)/16%3A_The_Chemical_Activity_of_the_Components_of_a_Solution/16.18%3A_Activities_of_Electrolytes_-_The_Debye-Huckel_TheoryThe Debye-Hückel theory leads to an equation for the activity coefficient of an ion in solution. The theory gives accurate values for the activity of an ion in very dilute solutions. As salt concentra...The Debye-Hückel theory leads to an equation for the activity coefficient of an ion in solution. The theory gives accurate values for the activity of an ion in very dilute solutions. As salt concentrations become greater, the accuracy of the Debye-Hückel model decreases. As a rough rule of thumb, the theory gives useful values for the activity coefficients of dissolved ions in solutions whose total salt concentrations are less than about 0.01 molal. The theory is based on an electrostatic model.
