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Related Concept Videos

Buffer Effectiveness02:19

Buffer Effectiveness

52.3K
Buffer solutions do not have an unlimited capacity to keep the pH relatively constant . Instead, the ability of a buffer solution to resist changes in pH relies on the presence of appreciable amounts of its conjugate weak acid-base pair. When enough strong acid or base is added to substantially lower the concentration of either member of the buffer pair, the buffering action within the solution is compromised.
The buffer capacity is the amount of acid or base that can be added to a given volume...
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Buffers: Buffer Capacity01:09

Buffers: Buffer Capacity

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Buffer capacity is the quantitative measure of a buffer to resist the change in pH. As shown in the following equation, the buffer capacity, denoted by 'beta', is expressed as the number of moles of acid or base needed to change the pH of a one-liter buffer solution by 1 unit. Here, Ca and Cb indicate the number of moles of acid and base, respectively. Note that dpH represents the change in pH.
In the graph, pH is plotted as a function of the number of moles of base (Cb) added to a weak...
1.8K
Buffers02:56

Buffers

169.0K
A solution containing appreciable amounts of a weak conjugate acid-base pair is called a buffer solution, or a buffer. Buffer solutions resist a change in pH when small amounts of a strong acid or a strong base are added. A solution of acetic acid and sodium acetate is an example of a buffer that consists of a weak acid and its salt: CH3COOH (aq) + CH3COONa (aq). An example of a buffer that consists of a weak base and its salt is a solution of ammonia and ammonium chloride: NH3 (aq) + NH4Cl...
169.0K
Buffers: Overview01:30

Buffers: Overview

6.9K
Buffers play a crucial role in stabilizing the pH of a solution by mitigating the effects of small amounts of added acid or base. They consist of a weak acid and its conjugate base or a weak base and its conjugate acid. A solution of acetic acid and sodium acetate is an example of a buffer that consists of a weak acid and its salt: CH3COOH (aq) + CH3COONa (aq). An example of a buffer that consists of a weak base and its salt is a solution of ammonia and ammonium chloride: NH3 (aq) + NH4Cl (aq).
6.9K
Protein Buffers in Blood Plasma and Cells01:20

Protein Buffers in Blood Plasma and Cells

2.8K
The human body utilizes protein buffer systems to maintain a stable pH. These systems capitalize on the dual role of amino acids, which can act as acids or bases by accepting or releasing hydrogen ions in response to pH changes. Protein buffer systems are particularly significant in the extracellular fluid (ECF) and intracellular fluid (ICF) of active cells, where structural and functional proteins provide substantial buffering capacity.
Certain amino acids can exist in a zwitterion state at a...
2.8K
Buffer Systems in the Body01:19

Buffer Systems in the Body

2.5K
Chemical buffers play a critical role in the body's regulation of pH levels. These systems contain one or more compounds that stabilize pH changes by neutralizing strong acids or bases. When pH levels drop, hydrogen ions bind to a weak base; when pH levels rise, hydrogen ions are released. This dynamic process helps maintain pH within a narrow and stable range essential for normal physiological function.
A typical buffer system in bodily fluids includes a weak acid and its corresponding...
2.5K

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Updated: Nov 7, 2025

Microfluidic Buffer Exchange for Interference-free Micro/Nanoparticle Cell Engineering
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Microfluidic Buffer Exchange for Interference-free Micro/Nanoparticle Cell Engineering

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Buffers, Especially the Good Kind.

Gary J Pielak1

  • 1Department of Chemistry, Department of Biochemistry and Biophysics, Lineberger Comprehensive Cancer Center, and Integrative Program for Biological and Genome Sciences, The University of North Carolina at Chapel Hill, Chapel Hill, North Carolina 27599, United States.

Biochemistry
|May 3, 2021
PubMed
Summary
This summary is machine-generated.

Norman Good

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Area of Science:

  • Biochemistry
  • Chemical Biology

Background:

  • Norman Good and colleagues developed essential hydrogen-ion buffers for biological research in 1966.
  • These buffers, known as
  • Good's buffers
  • became widely adopted in scientific research.
  • The original paper has over 2500 citations.

Observation:

  • The widespread use of Good's buffers means they are often used without critical re-evaluation.
  • The common buffer Tris is noted for its limitations in certain biochemical applications.

Findings:

  • The paper established criteria for effective hydrogen-ion buffers in biological systems.
  • Ten novel buffers were synthesized and validated, forming the basis of modern biochemical buffering.

Implications:

  • There is a need to develop new buffers by integrating Good's foundational principles with recent advancements in protein chemistry.
  • Synthesizing novel buffers could overcome limitations of existing ones, like Tris, and improve experimental outcomes.