(a) Given that Kb for ammonia is 1.8 ×10^-5 and that for hydroxylamine is 1.1 ×10^-8, which is t

step 1 Chapter 16, Problem 78. Given that KB for ammonium is 1 .8 times 10 to negative 5th, and that fo

(a) Given that Kb for ammonia is 1.8 ×10^-5 and that for...

(a) Given that $K_{b}$ for ammonia is $1.8 \times 10^{-5}$ and that for hydroxylamine is $1.1 \times 10^{-8}$, which is the stronger base? (b) Which is the stronger acid, the ammonium ion or the hydroxylammonium ion? (c) Calculate $K_{a}$ values for $\mathrm{NH}_{4}^{+}$ and $\mathrm{H}_{3} \mathrm{NOH}^{+}$.

Key Concepts

Conjugate Acid-Base Pairs

A conjugate acid-base pair consists of two species that transform into each other by the gain or loss of a proton. Understanding these pairs is critical in acid-base chemistry since the strength of an acid is inversely related to the strength of its conjugate base, and vice versa. This relationship is key to comparing acid and base strengths in different chemical systems.

Relationship between Ka, Kb, and Kw

For a conjugate acid-base pair in water, the product of the acid dissociation constant (Ka) and the base dissociation constant (Kb) is equal to the ionization constant of water (Kw). This fundamental relationship, expressed as Ka × Kb = Kw, allows for the determination of one constant if the other is known, providing insight into the relative strengths of acids and bases.

Base Dissociation Constant (Kb)

The base dissociation constant is a quantitative measure of the strength of a base in solution. It represents the equilibrium constant for the reaction in which a base accepts a proton from water, forming its conjugate acid and hydroxide ion. A higher Kb value indicates a stronger base, as it shows that the base more readily accepts a proton.

Acid Dissociation Constant (Ka)

The acid dissociation constant quantifies the strength of an acid by measuring its tendency to donate a proton in solution. It is the equilibrium constant for the dissociation of an acid into its conjugate base and a proton. A higher Ka value signifies a stronger acid because it indicates that the acid more readily releases a proton.

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