Acid dissociation constant - Relationship between acidity and basicity constants

In chemistry and biochemistry, acid dissociation constant, the acidity constant, or the acid-ionization constant (Ka) is a specific type of equilibrium constant that indicates the extent of dissociation of hydrogen ions from an acid. It is important to remember that the term [H2O] is omitted from the general equilibrium constant expression. While strong acids dissociate practically completely in solution and consequently have large acidity constants, weak acids do not fully dissociate and gen ...

Including:

• Acid dissociation constant - Basicity constant of the conjugate base
• Acid dissociation constant - Relationship between acidity and basicity constants
• Acid dissociation constant - The Relative Strengths of Acids and Bases
• Acid dissociation constant - pKa of some common substances

Read more here: » Acid dissociation constant: Encyclopedia - Acid dissociation constant

There exists a relationship between the value of Ka for an acid HA and the value of Kb for its conjugate base A–. Since adding the ionization reaction for HA and the ionization reaction of A– always gives the reaction for the self-ionization of water, the product of the acidity and basicity constants gives the dissociation constant of water (Kw), which is 1 ...

See also:

Acid dissociation constant, Acid dissociation constant - Basicity constant of the conjugate base, Acid dissociation constant - Relationship between acidity and basicity constants, Acid dissociation constant - The Relative Strengths of Acids and Bases, Acid dissociation constant - pKa of some common substances

Read more here: » Acid dissociation constant: Encyclopedia II - Acid dissociation constant - Relationship between acidity and basicity constants

The strengths of acids and bases in aqueous solutions are determined by the values of the dissociation constants Ka and Kb for acids and bases, respectively, and by their molar concentrations in solution. Outside of an aqueous solution, it is much more difficult to define the strengths of acids and bases (see Acid-base reaction theories for more information on Brønsted-Lowry, Arrhenius, and Lewis acids and bases.) For the purposes of this article, it is best to assume that a ...

See also:

Acid dissociation constant, Acid dissociation constant - Basicity constant of the conjugate base, Acid dissociation constant - Relationship between acidity and basicity constants, Acid dissociation constant - The Relative Strengths of Acids and Bases, Acid dissociation constant - pKa of some common substances

Read more here: » Acid dissociation constant: Encyclopedia II - Acid dissociation constant - The Relative Strengths of Acids and Bases

By analogy, one can define the basicity constant (Kb) and the pKb of the conjugate base A–: pKb = −log10Kb This is the dissociation constant for the equi ...

See also:

Acid dissociation constant, Acid dissociation constant - Basicity constant of the conjugate base, Acid dissociation constant - Relationship between acidity and basicity constants, Acid dissociation constant - The Relative Strengths of Acids and Bases, Acid dissociation constant - pKa of some common substances

Read more here: » Acid dissociation constant: Encyclopedia II - Acid dissociation constant - Basicity constant of the conjugate base