What is the expression for the relationship between the acid dissociation constant (Ka) and the base ionization constant (Kb)?

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Multiple Choice

What is the expression for the relationship between the acid dissociation constant (Ka) and the base ionization constant (Kb)?

Explanation:
The relationship between the acid dissociation constant (Ka) and the base ionization constant (Kb) is captured by the expression that links them through the ion product of water, Kw. This relationship is derived from the equilibrium expressions for acids and bases. In simple terms, for a weak acid (HA) dissociating in water, we have: HA ⇌ H⁺ + A⁻ The acid dissociation constant, Ka, is given by the expression: Ka = [H⁺][A⁻] / [HA] Similarly, for a weak base (B) that reacts with water, the equation is: B + H₂O ⇌ BH⁺ + OH⁻ And the base ionization constant, Kb, is expressed as: Kb = [BH⁺][OH⁻] / [B] When one combines these two equilibria, the water autoionization reaction can be considered: H₂O ⇌ H⁺ + OH⁻ The equilibrium constant for this process is the ion product of water, which is represented as: Kw = [H⁺][OH⁻] By substituting the expressions for Ka and Kb into this relationship, we arrive at the

The relationship between the acid dissociation constant (Ka) and the base ionization constant (Kb) is captured by the expression that links them through the ion product of water, Kw. This relationship is derived from the equilibrium expressions for acids and bases.

In simple terms, for a weak acid (HA) dissociating in water, we have:

HA ⇌ H⁺ + A⁻

The acid dissociation constant, Ka, is given by the expression:

Ka = [H⁺][A⁻] / [HA]

Similarly, for a weak base (B) that reacts with water, the equation is:

B + H₂O ⇌ BH⁺ + OH⁻

And the base ionization constant, Kb, is expressed as:

Kb = [BH⁺][OH⁻] / [B]

When one combines these two equilibria, the water autoionization reaction can be considered:

H₂O ⇌ H⁺ + OH⁻

The equilibrium constant for this process is the ion product of water, which is represented as:

Kw = [H⁺][OH⁻]

By substituting the expressions for Ka and Kb into this relationship, we arrive at the

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