Multiple Choice
If a solution of HF (Ka = 6.8 × 10⁻⁴) has a pH of 2.50, what is the initial concentration of hydrofluoric acid in the solution?
17. Acid and Base Equilibrium
pH of Weak Acids
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What is the equilibrium constant for the dissociation of a weak base in water?
A
Kw
B
Ka
C
Kb
D
Kc
Verified step by step guidance1
Understand that the equilibrium constant for the dissociation of a weak base in water is represented by Kb, which stands for the base dissociation constant.
Recall that the base dissociation constant, Kb, is used to describe the equilibrium between a weak base and its ions in solution.
Recognize that the equilibrium expression for a weak base B dissociating in water can be written as: B + H2O ⇌ BH+ + OH−.
The equilibrium constant expression for this reaction is: Kb = [BH+][OH−] / [B], where the square brackets denote the concentration of each species at equilibrium.
Note that Kw is the ion product of water, Ka is the acid dissociation constant, and Kc is the general equilibrium constant for reactions, but Kb specifically refers to the dissociation of a base.
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