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- https://chem.libretexts.org/Courses/University_of_Wisconsin_Oshkosh/Chem_370%3A_Physical_Chemistry_1_-_Thermodynamics_(Gutow)/02%3A_Extended_Explanations_-_Solutions_I_-_Volatile_Solutes/2.07%3A_Activities_of_Nonideal_SolutionsAs seen before activities are a way to account for deviation from ideal behavior while still keeping the formulism for the ideal case intact.
- https://chem.libretexts.org/Courses/DePaul_University/Physical_Chemistry_for_Biological_Sciences/14%3A_Solutions_I_-_Volatile_Solutes/14.07%3A_Activities_of_Nonideal_SolutionsAs seen before activities are a way to account for deviation from ideal behavior while still keeping the formulism for the ideal case intact.
- 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/16.03%3A_Expressing_the_Activity_Coefficient_as_a_Deviation_from_Raoult's_LawIf the components behave ideally in the gas phase and if pure liquid \(A\) at its equilibrium vapor pressure, \(P^{\textrm{⦁}}_A\), is the standard state for the activity of \(A\) in solution, we find...If the components behave ideally in the gas phase and if pure liquid \(A\) at its equilibrium vapor pressure, \(P^{\textrm{⦁}}_A\), is the standard state for the activity of \(A\) in solution, we find in Section 16.2 that the activity of component \(A\) is \({\tilde{a}}_A\left(P,y_A,y_B\right)={x_AP}/{P^{\textrm{⦁}}_A}\).
- 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/Courses/Grinnell_College/CHM_363%3A_Physical_Chemistry_1_(Grinnell_College)/11%3A_Solutions_Liquid_Liquid/11.07%3A_Activities_of_Nonideal_SolutionsAs seen before activities are a way to account for deviation from ideal behavior while still keeping the formulism for the ideal case intact.
- 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/Topics_in_Thermodynamics_of_Solutions_and_Liquid_Mixtures/01%3A_Modules/1.01%3A_Activity/1.1.09%3A_Activity_of_Water_-_Two_Solutes&\quad=\left(\mathrm{m}_{\mathrm{j}} / \mathrm{m}_{\mathrm{j}}\right) \, \mathrm{d}\left(\mathrm{m}_{\mathrm{j}} / \mathrm{m}^{0}\right)+\mathrm{m}_{\mathrm{j}} \, \mathrm{d} \ln \left(\gamma_{\mathrm...&\quad=\left(\mathrm{m}_{\mathrm{j}} / \mathrm{m}_{\mathrm{j}}\right) \, \mathrm{d}\left(\mathrm{m}_{\mathrm{j}} / \mathrm{m}^{0}\right)+\mathrm{m}_{\mathrm{j}} \, \mathrm{d} \ln \left(\gamma_{\mathrm{j}}\right)+\left(\mathrm{m}_{\mathrm{i}} / \mathrm{m}_{\mathrm{i}}\right) \, \mathrm{d}\left(\mathrm{m}_{\mathrm{i}} / \mathrm{m}^{0}\right)+\mathrm{m}_{\mathrm{j}} \, \mathrm{d} \ln \left(\gamma_{\mathrm{j}}\right)
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Thermodynamics_and_Chemical_Equilibrium_(Ellgen)/14%3A_Chemical_Potential_-_Extending_the_Scope_of_the_Fundamental_Equation/14.10%3A_Chemical_ActivityWe introduce the activity concept in the particular context of chemical equilibria, but its scope is broader. The activity of a component is a wholly new thermodynamic quantity. We view it as the prop...We introduce the activity concept in the particular context of chemical equilibria, but its scope is broader. The activity of a component is a wholly new thermodynamic quantity. We view it as the property that determines the chemical potential, μ , of a substance in a particular system at a given temperature. As such, the activity directly links the properties of the substance to the behavior of the system.
- https://chem.libretexts.org/Courses/University_of_Georgia/CHEM_3212%3A_Physical_Chemistry_II/09%3A_Phase_Equilibria/9.08%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/General_Chemistry/Chem1_(Lower)/13%3A_Acid-Base_Equilibria/13.02%3A_Strong_Monoprotic_Acids_and_BasesTo a good approximation, strong acids, in the forms we encounter in the laboratory and in much of the industrial world, have no real existence; they are all really solutions of H3O+. So if you think ...To a good approximation, strong acids, in the forms we encounter in the laboratory and in much of the industrial world, have no real existence; they are all really solutions of H3O+. So if you think about it, the labels on those reagent bottles you see in the lab are not strictly true! However, if the strong acid is highly diluted, the amount of H3O+ it contributes to the solution becomes comparable to that which derives from the autoprotolysis of water.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.14%3A_Chapter_Summary_and_Key_TermsThe chapter discusses analytical chemistry as the application of chemistry to analyze samples, focusing on using chemical reactivity to dissolve samples, separate analytes, transform analytes, or prov...The chapter discusses analytical chemistry as the application of chemistry to analyze samples, focusing on using chemical reactivity to dissolve samples, separate analytes, transform analytes, or provide a signal. Key reactions include precipitation, acid-base, metal-ligand complexation, and oxidation-reduction. It also covers equilibrium concepts, such as Le Ch??telier's principle, and solutions like buffers, using equilibrium constants, ladder diagrams, and activity coefficients.
