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- https://chem.libretexts.org/Courses/Mount_Aloysius_College/CHEM_100%3A_General_Chemistry_(O'Connor)/10%3A_Chemical_Equilibrium/10.05%3A_Some_Special_Types_of_EquilibriaThe conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematic...The conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematical relationship between K a and K b : The crystals precipitate in the wine or grow on the insides of the wine bottle and, if the bottle is stored on its side, on the bottom of the cork.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Beginning_Chemistry_(Ball)/13%3A_Chemical_Equilibrium/13.06%3A_Some_Special_Types_of_EquilibriaThe conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematic...The conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematical relationship between K a and K b : The crystals precipitate in the wine or grow on the insides of the wine bottle and, if the bottle is stored on its side, on the bottom of the cork.
- https://chem.libretexts.org/Courses/University_of_California_Davis/Chem_4B%3A_General_Chemistry_for_Majors_II_(Larsen)/Chem_4B_Textbook/Unit_III%3A_Chemical_Equilibria/VI%3A_AcidBase_Equilibria/6.04%3A_Equilibria_Involving_Weak_Acids_and_BasesThe strengths of Brønsted-Lowry acids and bases in aqueous solutions can be determined by their acid or base ionization constants. Stronger acids form weaker conjugate bases, and weaker acids form str...The strengths of Brønsted-Lowry acids and bases in aqueous solutions can be determined by their acid or base ionization constants. Stronger acids form weaker conjugate bases, and weaker acids form stronger conjugate bases. Thus strong acids are completely ionized in aqueous solution because their conjugate bases are weaker bases than water. Weak acids are only partially ionized because their conjugate bases are strong enough to compete successfully with water for possession of protons.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Analytical_Chemistry/2%3A_Analytical_Chemistry_2.0_(Harvey)/07%3A_Equilibrium_Chemistry/7.04%3A_Equilibrium_Constants_for_Chemical_ReactionsSeveral types of chemical reactions are important in analytical chemistry, either in preparing a sample for analysis or during the analysis. The most significant of these are: precipitation reactions,...Several types of chemical reactions are important in analytical chemistry, either in preparing a sample for analysis or during the analysis. The most significant of these are: precipitation reactions, acid–base reactions, complexation reactions, and oxidation–reduction (redox) reactions. In this section we review these reactions and their equilibrium constant expressions.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Acids_and_Bases/Ionization_Constants/Weak_Acids_and_Bases_1Weak acids and bases are only partially ionized in their solutions, whereas strong acids and bases are completely ionized when dissolved in water. The ionization of weak acids and bases is a chemical ...Weak acids and bases are only partially ionized in their solutions, whereas strong acids and bases are completely ionized when dissolved in water. The ionization of weak acids and bases is a chemical equilibrium phenomenon. The equilibrium principles are essential for the understanding of equilibria of weak acids and weak bases. In this connection, you probably realize that conjugate acids of weak bases are weak acids and conjugate bases of weak acids are weak bases.
- https://chem.libretexts.org/Courses/SUNY_Adirondack/CHM_103%3A_Principles_of_Chemistry/11%3A_Chemical_Equilibrium/11.6%3A_Some_Special_Types_of_EquilibriaIn one sense, all chemical equilibria are treated the same. However, there are several classes of reactions that are noteworthy because of either the identities of the reactants and products or the fo...In one sense, all chemical equilibria are treated the same. However, there are several classes of reactions that are noteworthy because of either the identities of the reactants and products or the form of the K expression.
- https://chem.libretexts.org/Courses/Fresno_City_College/Introductory_Chemistry_Atoms_First_for_FCC/13%3A_Chemical_Equilibrium/13.5%3A_Some_Special_Types_of_EquilibriaHC 2 H 3 O 2 is soluble in H 2 O (in fact, it is the acid in vinegar), so the reactant concentration will appear in the equilibrium constant expression. This is the same K w that was introduced in Cha...HC 2 H 3 O 2 is soluble in H 2 O (in fact, it is the acid in vinegar), so the reactant concentration will appear in the equilibrium constant expression. This is the same K w that was introduced in Chapter 12 and the same 1.0 × 10 −14 that appears in the relationship between the K a and the K b of a conjugate acid-base pair. The crystals precipitate in the wine or grow on the insides of the wine bottle and, if the bottle is stored on its side, on the bottom of the cork.
- https://chem.libretexts.org/Courses/Nassau_Community_College/Principles_of_Chemistry/13%3A_Chemical_Equilibrium/13.05%3A_Some_Special_Types_of_EquilibriaThe conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematic...The conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematical relationship between K a and K b : The crystals precipitate in the wine or grow on the insides of the wine bottle and, if the bottle is stored on its side, on the bottom of the cork.
- https://chem.libretexts.org/Courses/Lakehead_University/Analytical_I/6%3A_Equilibrium_Chemistry/6.04%3A_Equilibrium_Constants_for_Chemical_ReactionsSeveral types of chemical reactions are important in analytical chemistry, either in preparing a sample for analysis or during the analysis. The most significant of these are: precipitation reactions,...Several types of chemical reactions are important in analytical chemistry, either in preparing a sample for analysis or during the analysis. The most significant of these are: precipitation reactions, acid–base reactions, complexation reactions, and oxidation–reduction (redox) reactions. In this section we review these reactions and their equilibrium constant expressions.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Inorganic_Chemistry_(LibreTexts)/06%3A_Acid-Base_and_Donor-Acceptor_Chemistry/6.02%3A_Arrhenius_ConceptThe Arrhenius acid-base concept defines acids and bases in terms of how they affect the amount of hydronium ions (and by extension hydroxide ions in aqueous solutions. Simply, in the Arrhenius definit...The Arrhenius acid-base concept defines acids and bases in terms of how they affect the amount of hydronium ions (and by extension hydroxide ions in aqueous solutions. Simply, in the Arrhenius definition an acid is a substance that increases the concentration of hydronium ions when it is dissolved in water. This typically occurs when the acid dissociates by loss of a proton to water.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Acids_and_Bases/Ionization_Constants/Weak_Acids_and_BasesUnlike strong acids/bases, weak acids and weak bases do not completely dissociate (separate into ions) at equilibrium in water, so calculating the pH of these solutions requires consideration of a uni...Unlike strong acids/bases, weak acids and weak bases do not completely dissociate (separate into ions) at equilibrium in water, so calculating the pH of these solutions requires consideration of a unique ionization constant and equilibrium concentrations. Although this is more difficult than calculating the pH of a strong acid or base solution, most biochemically important acids and bases are considered weak, and so it is very useful to understand how to calculate the pH of these substances.
