Ionization constants conjugate acid-base relationship

Equilibrium constants of weak bases can be measured in the laboratory by procedures very much like those used for weak acids. In practice, though, it is simpler to take advantage of a simple mathematical relationship between Kb for a weak base and Ka for its conjugate acid. This relationship can be derived by adding together the equations for the ionization of the weak acid HB and the reaction of the weak base B- with water ... [Pg.370]

THE RELATIONSHIP BETWEEN THE IONIZATION CONSTANTS OF ACIDS AND THEIR CONJUGATE BASES... [Pg.597]

Relationship between the acid and base ionization constants of a conjugate acid-base pair. [Pg.635]

The Relationship Between the Ionization Constants of Acids and Their Conjugate Bases... [Pg.659]

The Relationship Between Conjugate Acid-Base Ionization Constants 553... [Pg.529]

This relationship is general and shows that the product of acid- and base-ionization constants in aqueous solution for conjugate acid—base pairs equals the ion-product constant for water, K, . [Pg.708]

State the relationship between the ionization constant for an acid and that for its conjugate base (Section 15.3, Problems 21-22). [Pg.669]

An important relationship between the acid ionization constant and the ionization constant of its conjugate base can be derived as follows, using acetic acid as an example ... [Pg.615]

What is the relationship between the acid ionization constant for a weak acid (K, ) and the base ionization constant for its conjugate base (AT],) ... [Pg.745]

Perhaps you recognize this equation from the beginning of the chapter. If you don t, it is the equation for the self-ionization of water, from which Kw was derived. What you ve now seen are three equations. The first is an equation that would be used to calculate the Ka of acetic acid. The second is the equation used to calculate Kh for the conjugate base. The third, which is derived from these two, is the formula for calculating Kw. There is a very clear relationship between Ka, Ku, and Kw. The three constants are all related in Equation 14.9, shown below ... [Pg.329]

An acid constant of 10 ° for N2H4 N2H3in aqueous solutions was predicted from a linear relationship between the acidities of a series of nitrogen acids and (ab initio) calculated average local ionization energies of the conjugate bases [9]. A free enthalpy of 181.2 kJ/mol was derived for this process [8]. [Pg.86]

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