Textbook Question
For each of the following compounds, indicate the pH at which
b. more than 99% of the compound is in a form that possesses a charge.
1. CH3CH2COOH (pKa = 4.9)
2. CH3N+H3 (pKa = 10.7)
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3. Acids and Bases
Acid Base Equilibrium
Multiple Choice
Which of the following conditions is required for maintaining acid-base equilibrium in a solution?
A
The concentration of acid and base must be equal.
B
The solution must have a constant .
C
The rate of the forward and reverse reactions must be equal.
D
The solution must be at a high temperature.
Verified step by step guidance1
Understand the concept of acid-base equilibrium: In a chemical equilibrium, the rate of the forward reaction (acid dissociating into ions) and the rate of the reverse reaction (ions recombining to form the acid) must be equal.
Recognize that equilibrium does not require equal concentrations of acid and base. Instead, it requires that the rates of the forward and reverse reactions are equal, allowing the concentrations to remain constant over time.
Consider the role of pH: While a constant pH might indicate equilibrium, it is not a requirement for equilibrium itself. Equilibrium is about the balance of reaction rates, not necessarily the pH value.
Evaluate the effect of temperature: High temperature can affect the rates of reactions, but equilibrium is defined by the equality of the forward and reverse reaction rates, not by temperature conditions.
Conclude that the key condition for maintaining acid-base equilibrium is the equality of the forward and reverse reaction rates, ensuring that the system remains stable over time.
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