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Questions and Answers
What is the Brønsted-Lowry definition of a base?
What is the Brønsted-Lowry definition of a base?
What does the Henderson-Hasselbalch equation help to calculate?
What does the Henderson-Hasselbalch equation help to calculate?
When is a buffer most effective?
When is a buffer most effective?
What does the pKa of an acid indicate?
What does the pKa of an acid indicate?
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What is the significance of the pKa value in the Henderson-Hasselbalch equation?
What is the significance of the pKa value in the Henderson-Hasselbalch equation?
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Why is it important for inorganic phosphate to have multiple pKa values?
Why is it important for inorganic phosphate to have multiple pKa values?
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How does the Henderson-Hasselbalch equation relate to the presence of a conjugate acid-base pair at a certain pH?
How does the Henderson-Hasselbalch equation relate to the presence of a conjugate acid-base pair at a certain pH?
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Study Notes
Brønsted-Lowry Definition of a Base
- A Brønsted-Lowry base is a substance that accepts a proton (H+)
Henderson-Hasselbalch Equation
- Calculates the pH of a buffer solution
- Equation: pH = pKa + log ([conjugate base]/[acid])
Buffer Effectiveness
- Buffers are most effective when the pH is close to the pKa of the acid
- The buffer is able to resist changes in pH when there is a roughly equal concentration of the acid and its conjugate base
pKa of an Acid
- Indicates the acid's strength in a solution
- Lower pKa: Stronger acid
- Higher pKa: Weaker acid
pKa Significance in the Henderson-Hasselbalch Equation
- The pKa value in the Henderson-Hasselbalch equation represents the pH at which the concentrations of the acid and its conjugate base are equal
Inorganic Phosphate pKa Values
- Inorganic phosphate (H3PO4) has multiple pKa values because it can donate multiple protons in a stepwise fashion.
- Important for buffering within biological systems since it can act as a buffer over a broad pH range
Conjugate Acid-Base Pair and pH
- The Henderson-Hasselbalch equation demonstrates the relationship between the pH and the relative amounts of a conjugate acid-base pair
- When the pH is equal to the pKa, the concentrations of the acid and its conjugate base are equal
- As the pH increases, the concentration of the conjugate base increases relative to the concentration of the acid
- As the pH decreases, the concentration of the acid increases relative to the concentration of the conjugate base
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Description
Test your understanding of acid-base reactions, the Brønsted-Lowry definition, strong and weak acids, and the Henderson-Hasselbalch equation in the context of pH and buffers. This quiz covers material from Lecture 2 of BCMB 401, Spring 24, focusing on Chapter 1.3 of the reading.
