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- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Topics_in_Thermodynamics_of_Solutions_and_Liquid_Mixtures/01%3A_Modules/1.01%3A_Activity/1.1.11%3A_Activity_CoefficientsThe properties of solutes in solutions are described using activity coefficients which are linked to the descriptions of the composition of solutions: molality scale, \(\gamma_{j}\); concentration sca...The properties of solutes in solutions are described using activity coefficients which are linked to the descriptions of the composition of solutions: molality scale, \(\gamma_{j}\); concentration scale \(\gamma_{j}\); mole fraction scale \(\mathrm{f}_{\mathrm{j}}^{*}\).
- 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)/06%3A_Multiple_Component_Phase_Equilibrium/6.13%3A_ActivityFor non-ideal gases, we introduced in chapter 11 the concept of fugacity as an effective pressure that accounts for non-ideal behavior.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Analytical_Chemistry/2%3A_Analytical_Chemistry_2.0_(Harvey)/07%3A_Equilibrium_Chemistry/7.09%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/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/The_Live_Textbook_of_Physical_Chemistry_(Peverati)/14%3A_Properties_of_Solutions/14.01%3A_ActivityFor non-ideal gases, we introduced in chapter 11 the concept of fugacity as an effective pressure that accounts for non-ideal behavior.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Topics_in_Thermodynamics_of_Solutions_and_Liquid_Mixtures/01%3A_Modules/1.01%3A_Activity/1.1.12%3A_Activity_Coefficients-_Salt_Solutions-_Ion-Ion_InteractionsIn fact for almost the whole of the 20th Century, scientists offered theoretical bases for expressing \(\ln \left(\gamma_{\pm}\right)\) as a function of the composition of a salt solution, temperature...In fact for almost the whole of the 20th Century, scientists offered theoretical bases for expressing \(\ln \left(\gamma_{\pm}\right)\) as a function of the composition of a salt solution, temperature, pressure and electric permittivity of the solvent. In order to calculate the electric potential at the j-ion arising from all other ions in solution, we need to know the distribution of these ions about the j-ion.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Instrumental_Analysis_(LibreTexts)/35%3A_Appendicies/35.07%3A_Activity_CoefficientsFailing to account for the effect of ionic strength can lead to a significant error in the reported concentration of H 3 O + . For example, if the pH of a solution is 7.00 and the activity coefficient...Failing to account for the effect of ionic strength can lead to a significant error in the reported concentration of H 3 O + . For example, if the pH of a solution is 7.00 and the activity coefficient for H 3 O + is 0.90, then the concentration of H 3 O + is \(1.11 \times 10^{-7}\) M, not \(1.00 \times 10^{-7}\) M, an error of +11%. Fortunately, when we develop and carry out an analytical method, we are more interested in controlling pH than in calculating [H 3 O + ].
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.11%3A_Some_Final_Thoughts_on_Equilibrium_CalculationsThe chapter discusses tools for evaluating system composition at equilibrium, highlighting the importance of selecting the appropriate tool based on the precision required. It emphasizes the need to i...The chapter discusses tools for evaluating system composition at equilibrium, highlighting the importance of selecting the appropriate tool based on the precision required. It emphasizes the need to include all relevant equilibrium reactions to prevent errors. It introduces computational programs like Visual Minteq and CurTiPot for modeling equilibria and the R package CHNOSZ for thermodynamic calculations in aqueous geochemistry.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Physical_Properties_of_Matter/Solutions_and_Mixtures/Nonideal_Solutions/Introduction_to_Non-ideal_SolutionsA non-ideal solution is a solution that does not abide to the rules of an ideal solution where the interactions between the molecules are identical (or very close) to the interactions between molecule...A non-ideal solution is a solution that does not abide to the rules of an ideal solution where the interactions between the molecules are identical (or very close) to the interactions between molecules of different components. That is, there is no forces acting between the components: no Van-der-Waals nor any Coulomb forces. We assume ideal properties for dilute solutions.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/25%3A_Solutions_II_-_Nonvolatile_Solutes/25.05%3A_Electrolytes_Solutions_are_Nonideal_at_Low_ConcentrationsThis page explores the challenges of studying strong electrolytes like NaCl in solution, focusing on the dissociation into charged ions and non-ideal behavior due to electrostatic interactions. It emp...This page explores the challenges of studying strong electrolytes like NaCl in solution, focusing on the dissociation into charged ions and non-ideal behavior due to electrostatic interactions. It emphasizes the significance of stoichiometric coefficients in thermodynamic descriptions and introduces mean ionic activity in relation to salt concentration.
