Henderson-Hasselbalch Equation
Emily Wilson
8 min read
Listen to this study note
Study Guide Overview
This guide covers the Henderson-Hasselbalch equation for understanding and working with buffers. It explains the equation's components (pH, pKa, [A-], [HA]), its application in calculating buffer pH, and its use in titration problems. The guide also includes practice questions and exam tips.
#Mastering Buffers: Your Ultimate Guide to the Henderson-Hasselbalch Equation
Hey AP Chem student! Let's dive into the Henderson-Hasselbalch equation, your secret weapon for tackling buffer problems. This guide will break it down, step-by-step, so you feel confident and ready for anything the exam throws at you. Let's get started!
#Introduction to Buffers and the Henderson-Hasselbalch Equation
Buffers are crucial in chemistry and biology, and the Henderson-Hasselbalch equation is your go-to tool for understanding them. Remember, buffers resist changes in pH and consist of a weak acid and its conjugate base (or a weak base and its conjugate acid). Let's get cozy with this equation:
#Breaking Down the Equation
- pH: The measure of acidity, calculated as -log[H+]. Often, this is what you're solving for.
- pKa: -log(Ka), which tells us about the acid's strength. Remember, a lower pKa means a stronger acid.
- log([A-]/[HA]): This is the log of the ratio of the conjugate base [A-] to the weak acid [HA]. This ratio is key to understanding buffer behavior. 💡
Remember, the strongest buffer action occurs when [A-] = [HA], making the log term zero, and pH = pKa.
#Applying the Henderson-Hasselbalch Equation: Example Problems
Let's see how to use this equation in action. We'll ta...
How are we doing?
Give us your feedback and let us know how we can improve