7 Questions
What is the Brønsted-Lowry definition of a base?
A proton acceptor
What does the Henderson-Hasselbalch equation help to calculate?
The pH of a solution containing a weak acid and its conjugate base
When is a buffer most effective?
At a pH equal to the pKa of the weak acid
What does the pKa of an acid indicate?
The tendency of the acid to donate a proton
What is the significance of the pKa value in the Henderson-Hasselbalch equation?
It represents the pH at which the buffering action of a weak acid is most effective.
Why is it important for inorganic phosphate to have multiple pKa values?
To enable it to act as a buffer over a wide range of pH values.
How does the Henderson-Hasselbalch equation relate to the presence of a conjugate acid-base pair at a certain pH?
It quantifies the ratio of the conjugate acid to base at a specific pH.
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.
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