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  2. Conjugate (acid-base theory) - Wikipedia

    en.wikipedia.org/wiki/Conjugate_(acid-base_theory)

    One use of conjugate acids and bases lies in buffering systems, which include a buffer solution. In a buffer, a weak acid and its conjugate base (in the form of a salt), or a weak base and its conjugate acid, are used in order to limit the pH change during a titration process. Buffers have both organic and non-organic chemical applications.

  3. Lewis acids and bases - Wikipedia

    en.wikipedia.org/wiki/Lewis_acids_and_bases

    As usual, a weaker acid has a stronger conjugate base. Examples of Lewis bases based on the general definition of electron pair donor include: simple anions, such as H − and F −; other lone-pair-containing species, such as H 2 O, NH 3, HO −, and CH 3 −; complex anions, such as sulfate; electron-rich π-system Lewis bases, such as ethyne ...

  4. Acid strength - Wikipedia

    en.wikipedia.org/wiki/Acid_strength

    For example, acetic acid is a weak acid which has a = 1.75 x 10 −5. Its conjugate base is the acetate ion with K b = 10 −14 /K a = 5.7 x 10 −10 (from the relationship K a × K b = 10 −14), which certainly does not correspond to a strong base. The conjugate of a weak acid is often a weak base and vice versa.

  5. Acid–base reaction - Wikipedia

    en.wikipedia.org/wiki/Acidbase_reaction

    In chemistry, an acidbase reaction is a chemical reaction that occurs between an acid and a base.It can be used to determine pH via titration.Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acidbase theories, for example, Brønsted–Lowry acidbase theory.

  6. Buffer solution - Wikipedia

    en.wikipedia.org/wiki/Buffer_solution

    When some strong acid is added to an equilibrium mixture of the weak acid and its conjugate base, hydrogen ions (H +) are added, and the equilibrium is shifted to the left, in accordance with Le Chatelier's principle. Because of this, the hydrogen ion concentration increases by less than the amount expected for the quantity of strong acid added.

  7. Deprotonation - Wikipedia

    en.wikipedia.org/wiki/Deprotonation

    For example, deprotonation of an alcohol forms the negatively charged alkoxide, which is a much stronger nucleophile. To determine whether or not a given base will be sufficient to deprotonate a specific acid, compare the conjugate base with the original base. A conjugate base is formed when the acid is deprotonated by the base.

  8. Brønsted–Lowry acid–base theory - Wikipedia

    en.wikipedia.org/wiki/Brønsted–Lowry_acid...

    H 2 O is a base because it accepts a proton from CH 3 COOH and becomes its conjugate acid, the hydronium ion, (H 3 O +). [9] The reverse of an acidbase reaction is also an acidbase reaction, between the conjugate acid of the base in the first reaction and the conjugate base of the acid.

  9. Protonation - Wikipedia

    en.wikipedia.org/wiki/Protonation

    In chemistry, protonation (or hydronation) is the adding of a proton (or hydron, or hydrogen cation), usually denoted by H +, to an atom, molecule, or ion, forming a conjugate acid. [1] (The complementary process, when a proton is removed from a Brønsted–Lowry acid, is deprotonation.) Some examples include The protonation of water by ...