Science, Tech, Math › Science What Are Buffers and What Do They Do? Chemistry of Buffers Share Flipboard Email Print Cl4ss1cr0ck3R / Creative Commons Science Chemistry Basics Chemical Laws Molecules Periodic Table Projects & Experiments Scientific Method Biochemistry Physical Chemistry Medical Chemistry Chemistry In Everyday Life Famous Chemists Activities for Kids Abbreviations & Acronyms Biology Physics Geology Astronomy Weather & Climate By Anne Marie Helmenstine, Ph.D. Chemistry Expert Ph.D., Biomedical Sciences, University of Tennessee at Knoxville B.A., Physics and Mathematics, Hastings College Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. She has taught science courses at the high school, college, and graduate levels. our editorial process Facebook Facebook Twitter Twitter Anne Marie Helmenstine, Ph.D. Updated October 07, 2019 The use of buffers is an important concept in acid-base chemistry. Here's a look at what buffers are and how they function. What Is a Buffer? There are two key terms associated with buffers. A buffer is an aqueous solution that has a highly stable pH. A buffering agent is a weak acid or weak base that helps maintain the pH of an aqueous solution after adding another acid or base. If you add an acid or a base to a buffered solution, its pH will not change significantly. Similarly, adding water to a buffer or allowing water to evaporate will not change the pH of a buffer. How Do You Make a Buffer? A buffer is made by mixing a large volume of a weak acid or weak base together with its conjugate. A weak acid and its conjugate base can remain in solution without neutralizing each other. The same is true for a weak base and its conjugate acid. How Do Buffers Work? When hydrogen ions are added to a buffer, they will be neutralized by the base in the buffer. Hydroxide ions will be neutralized by the acid. These neutralization reactions will not have much effect on the overall pH of the buffer solution. When you select an acid for a buffer solution, choose an acid that has a pKa close to your desired pH. This will give your buffer nearly equivalent amounts of acid and conjugate base so it will be able to neutralize as much H+ and OH- as possible. Sources Atkins, Peter; Jones, Loretta (2005). Chemical Principles: The Quest for Insight (3rd ed.). New York: Freeman. ISBN 0-7167-5701-X.Harris, Daniel C. (2003). Quantitative Chemical Analysis (6th ed.). New York: Freeman. ISBN 0-7167-4464-3.