Search
- https://chem.libretexts.org/Courses/Stanford_Online_High_School/TEN2A-Acids/02%3A_Acidic_Mixtures/2.02%3A_Solutions_of_Strong_Acids_and_BasesAcid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ b...Acid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ by only a proton constitute a conjugate acid–base pair. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases.
- https://chem.libretexts.org/Courses/Tennessee_State_University/Inorganic_Chemistry_(CHEM_5000_4200)/01%3A_Map-_Inorganic_Chemistry-I_(LibreTexts)/04%3A_Acid-Base_and_Donor-Acceptor_Chemistry/4.03%3A_Brnsted-Lowry_Concept/4.3.10%3A_Acid-Base_Chemistry_in_Amphoteric_Solvents_and_the_Solvent_Leveling_EffectThe strongest Brønsted base, B, that can exist in a solvent is determined by the relative acidity of the solvent and the base's conjugate acid, BH+, determines whether the base wi...The strongest Brønsted base, B, that can exist in a solvent is determined by the relative acidity of the solvent and the base's conjugate acid, BH+, determines whether the base will remain unprotonated and able to act as a base in that solvent.
- https://chem.libretexts.org/Courses/Saint_Marys_College_Notre_Dame_IN/CHEM_122-02_(Under_Construction)/3%3A_Acids_and_Bases/3.1%3A_AcidBase_Equilibria/Strong_Acids_and_BasesAcid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ b...Acid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ by only a proton constitute a conjugate acid–base pair. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases.
- https://chem.libretexts.org/Courses/Lansing_Community_College/LCC%3A_Chem_151_-_General_Chemistry_I/Text/15%3A_AcidBase_Equilibria/15.05%3A_Strong_Acids_and_BasesAcid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ b...Acid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ by only a proton constitute a conjugate acid–base pair. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases.
- https://chem.libretexts.org/Courses/Williams_School/Chemistry_IIA/05%3A_AcidBase_Equilibria/5.05%3A_Strong_Acids_and_BasesAcid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ b...Acid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ by only a proton constitute a conjugate acid–base pair. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases.
- https://chem.libretexts.org/Courses/Purdue/Chem_26505%3A_Organic_Chemistry_I_(Lipton)/Chapter_8._Acid-Base_Reactions/8.4_Solvent_EffectsSimilarly, when ammonia is the solvent, the strongest acid is ammonium (NH 4 + ), thus HCl and a super acid exert the same acidifying effect. As a result a strong acid such as perchloric acid exhibits...Similarly, when ammonia is the solvent, the strongest acid is ammonium (NH 4 + ), thus HCl and a super acid exert the same acidifying effect. As a result a strong acid such as perchloric acid exhibits more strongly acidic properties than a weak acid such as acetic acid when dissolved in a weakly basic solvent. HCl acts as an acid in H 2 O, a stronger acid in NH 3 , a weak acid in CH 3 COOH, neutral in C 6 H 6 and a weak base in HF.
- https://chem.libretexts.org/Sandboxes/khaas/Inorganic_Chemistry_II_(CHEM4210)/01%3A_Basic_Inorganic_Concepts/1.06%3A_Acid-Base_and_Donor-Acceptor_Chemistry/1.6.03%3A_Brnsted-Lowry_Concept/1.6.3.10%3A_Acid-Base_Chemistry_in_Amphoteric_Solvents_and_the_Solvent_Leveling_EffectThe Brønsted-Lowry concept allows for an understanding of hydrogen ion transfer chemistry in amphoteric protic solvents. Amphoteric protic solvents are those which can both accept and receive hydrogen...The Brønsted-Lowry concept allows for an understanding of hydrogen ion transfer chemistry in amphoteric protic solvents. Amphoteric protic solvents are those which can both accept and receive hydrogen ions. From the viewpoint of the Brønsted-Lowry concept the acid-base chemistry in these solvents is governed by autoionization equilibria analogous to water autoionization.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Acids_and_Bases/Acid_Base_Reactions/The_Fall_of_the_Proton_-_Viewing_Acid_Base_Chemistry_from_a_Thermodynamic_PerspectiveAn acid, being a proton donor, can only act as an acid if there is a suitable base present to accept the proton. What do we mean by "suitable'' in this context? Simply that a base, in order to accept ...An acid, being a proton donor, can only act as an acid if there is a suitable base present to accept the proton. What do we mean by "suitable'' in this context? Simply that a base, in order to accept a proton, must provide a lower-energy resting place for the proton. Thus you can view an acid-base reaction as the "fall" of the proton from a higher potential energy to a lower potential energy-- the same as a book will fall only downward, to a position of lower (gravitational) potential energy.
- https://chem.libretexts.org/Courses/Northern_Michigan_University/CH_215%3A_Chemistry_of_the_Elements_Fall_2023/02%3A_Acid-Base_and_Donor-Acceptor_Chemistry/2.05%3A_Brnsted-Lowry_Acid-Base_Concept/2.5.07%3A_Acid-Base_Chemistry_in_Amphoteric_Solvents_and_the_Solvent_Leveling_EffectThe Brønsted-Lowry concept allows for an understanding of hydrogen ion transfer chemistry in amphoteric protic solvents. Amphoteric protic solvents are those which can both accept and receive hydrogen...The Brønsted-Lowry concept allows for an understanding of hydrogen ion transfer chemistry in amphoteric protic solvents. Amphoteric protic solvents are those which can both accept and receive hydrogen ions. From the viewpoint of the Brønsted-Lowry concept the acid-base chemistry in these solvents is governed by autoionization equilibria analogous to water autoionization.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Inorganic_Chemistry_(LibreTexts)/06%3A_Acid-Base_and_Donor-Acceptor_Chemistry/6.03%3A_Brnsted-Lowry_Concept/6.3.10%3A_Acid-Base_Chemistry_in_Amphoteric_Solvents_and_the_Solvent_Leveling_EffectThe Brønsted-Lowry concept allows for an understanding of hydrogen ion transfer chemistry in amphoteric protic solvents. Amphoteric protic solvents are those which can both accept and receive hydrogen...The Brønsted-Lowry concept allows for an understanding of hydrogen ion transfer chemistry in amphoteric protic solvents. Amphoteric protic solvents are those which can both accept and receive hydrogen ions. From the viewpoint of the Brønsted-Lowry concept the acid-base chemistry in these solvents is governed by autoionization equilibria analogous to water autoionization.
- https://chem.libretexts.org/Courses/University_of_Alberta_Augustana_Campus/AUCHE_112_-_General_Chemistry_II_(Elizabeth_McGinitie)/05%3A_Acids_and_Bases/5.06%3A_Strong_Acids_and_BasesAcid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ b...Acid–base reactions always contain two conjugate acid–base pairs. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Two species that differ by only a proton constitute a conjugate acid–base pair. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases.
