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- https://chem.libretexts.org/Courses/South_Puget_Sound_Community_College/Chem_121%3A_Introduction_to_Chemistry/09%3A_Chapter_8A_-_Acids_bases_and_pH/9.01%3A_Strong_and_Weak_Acids_and_Bases_(Conceptual_Introduction)/9.1.01%3A_Ionization_of_Acids_in_Solution_(Ka_values_and_Comparative_strengths)We will address this fully in Chapter 10, but according to the Law of Mass Action, the equilibrium constant, K for this reaction, is simply given by the ratio of the activities of the products and rea...We will address this fully in Chapter 10, but according to the Law of Mass Action, the equilibrium constant, K for this reaction, is simply given by the ratio of the activities of the products and reactants. When you are dealing with acids, the equilibrium constant is generally called an acid dissociation constant, and is written as K a . The larger the value of K a , the greater the extent of ionization and the and the higher the resulting concentration of the hydronium ion.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_Online_(Young)/08%3A_Acids_Bases_and_pH/8.2%3A_Ionization_of_Acids_in_SolutionWe will address this fully in Chapter 10, but according to the Law of Mass Action, the equilibrium constant, K for this reaction, is simply given by the ratio of the activities of the products and rea...We will address this fully in Chapter 10, but according to the Law of Mass Action, the equilibrium constant, K for this reaction, is simply given by the ratio of the activities of the products and reactants. When you are dealing with acids, the equilibrium constant is generally called an acid dissociation constant, and is written as K a . The larger the value of K a , the greater the extent of ionization and the and the higher the resulting concentration of the hydronium ion.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Inorganic_Chemistry_(LibreTexts)/06%3A_Acid-Base_and_Donor-Acceptor_Chemistry/6.03%3A_Brnsted-Lowry_Concept/6.3.05%3A_Thermodynamics_of_Solution-Phase_Brnsted_Acidity_and_BasicityThe text discusses the influence of solvation on the behavior of Br??nsted-Lowry acids and bases in aqueous systems, with a focus on thermochemical parameters such as enthalpy and entropy changes for ...The text discusses the influence of solvation on the behavior of Br??nsted-Lowry acids and bases in aqueous systems, with a focus on thermochemical parameters such as enthalpy and entropy changes for acid dissociation. The major driving force for dissociation is the enthalpy, which is exothermic for most acids, except for certain weak acids where entropy plays a larger role.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.06%3A_Ladder_DiagramsThe page discusses the importance of considering chemical interactions, like pH and solubility, when developing or evaluating analytical methods. It critiques the inappropriate use of NH3 in precipita...The page discusses the importance of considering chemical interactions, like pH and solubility, when developing or evaluating analytical methods. It critiques the inappropriate use of NH3 in precipitating AgCl due to its solubility-increasing effect. Key analytical errors often stem from overlooking chemical interferences. Ladder diagrams are introduced as tools for visualizing equilibrium chemistry, aiding in understanding reaction dynamics and evaluating changes in solution conditions.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_Online_(Young)/08%3A_Acids_Bases_and_pH/8.S%3A_Acids_Bases_and_pH_(Summary)For the dissociation of the simple acid, HA, the equilibrium constant, K a , is simply given by the ratio of the concentrations of the products and the reactants, remembering that the molarity of the ...For the dissociation of the simple acid, HA, the equilibrium constant, K a , is simply given by the ratio of the concentrations of the products and the reactants, remembering that the molarity of the solutes have been used to approximate their activity, and that solvents, such as water, have an activity of 1.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.08%3A_Buffer_SolutionsThis page explains the different responses to adding HCl to pure water versus a solution with acetic acid and sodium acetate. It describes how buffers, like the acetic acid-sodium acetate mixture, res...This page explains the different responses to adding HCl to pure water versus a solution with acetic acid and sodium acetate. It describes how buffers, like the acetic acid-sodium acetate mixture, resist changes in pH due to their equilibrium shifting. The Henderson-Hasselbalch equation is central to understanding buffer preparation and effectiveness.
