(a) Si la Ka del ácido acético es de 1.8 ×10^-5 y la del ácido hipocloroso es de 3.0 ×10^-8, ¿cu

step 1 Problem 79. Part A. Acetic acid is stronger because it has the larger KB value. This is explanat

(a) Si la Ka del ácido acético es de 1.8 ×10^-5 y la del...

(a) Si la $K_a$ del ácido acético es de $1.8 \times 10^{-5} \mathrm{y}$ la del ácido hipocloroso es de $3.0 \times 10^{-8}$, ¿cuál es el ácido más fuerte? (b) ¿Cuál es la base más fuerte: el ion aceta to o el ion hipoclorito? (c) Calcule los valores de $\mathrm{K}_b \mathrm{de}_2 \mathrm{H}_3 \mathrm{O}_2^{-} \mathrm{y} \mathrm{ClO}^{-}$.

Key Concepts

Relationship between Ka and Kb

The equilibrium constants for conjugate acid-base pairs are connected through the ionization constant of water (Kw), where Ka × Kb = Kw (typically 1.0 × 10?¹? at room temperature). This relationship allows one to calculate the strength of a conjugate base if the acid’s Ka is known, and vice versa.

Conjugate Acid-Base Pairs

Every acid has a corresponding conjugate base, and every base has a conjugate acid. The strengths of conjugate pairs are inversely related—a strong acid will have a weak conjugate base, while a strong base will have a weak conjugate acid. This interplay is important in understanding overall acid-base behavior.

Base Dissociation Constant (Kb)

The base dissociation constant (Kb) quantifies the ability of a base to accept a proton from water, forming hydroxide ions. A higher Kb signifies a stronger base, meaning it more readily engages in proton acceptance in aqueous environments.

Acid Strength Comparison

Comparing acid strengths involves evaluating their Ka values. In a scenario where one acid has a larger Ka than another, it is considered to be the stronger acid since it dissociates to a greater extent and thereby produces more hydrogen ions in solution.

Acid Dissociation Constant (Ka)

The acid dissociation constant (Ka) measures the extent to which an acid donates a proton in aqueous solution. It reflects the strength of an acid; higher Ka values indicate stronger acids because they are more efficient at releasing hydrogen ions during dissociation.

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