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Related Concept Videos

Buffer Systems in the Body01:19

Buffer Systems in the Body

2.7K
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...
2.7K
Buffer Effectiveness02:19

Buffer Effectiveness

52.5K
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...
52.5K
Buffers: Overview01:30

Buffers: Overview

7.6K
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).
7.6K
Bicarbonate-Carbonic Acid Buffer01:22

Bicarbonate-Carbonic Acid Buffer

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The carbonic acid-bicarbonate buffer system is critical for maintaining the body's pH balance. It operates on the equilibrium:
4.2K
Buffers02:56

Buffers

169.3K
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...
169.3K
pH Homeostasis01:31

pH Homeostasis

17.5K
Acid-base homeostasis is essential for maintaining normal physiological activities in humans. The pH of various body fluids is strictly regulated because it is critical for the optimal activity of enzymes involved in metabolic reactions. Enzymes are basically proteins, so, any significant change in pH can affect their structure and activity. In humans, pH is regulated using three primary mechanisms— chemical buffer systems, respiratory regulation, and renal regulation.
Respiratory...
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Related Experiment Video

Updated: Nov 13, 2025

In vitro Monitoring of Extracellular pH in Real-Time
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In vitro Monitoring of Extracellular pH in Real-Time

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Extracellular buffer choice influences acid-base responses and gastrointestinal symptoms.

J Peacock1, S A Sparks1, I Middlebrook1

  • 1Sports Nutrition and Performance Research Group, Department of Sport and Physical Activity, Edge Hill University, Ormskirk, UK.

Research in Sports Medicine (Print)
|March 15, 2021
PubMed
Summary

Sodium bicarbonate and sodium citrate both elevate blood bicarbonate levels, but sodium bicarbonate leads to higher concentrations and pH. However, sodium citrate results in fewer gastrointestinal symptoms.

Keywords:
Alkalosisdelayed-release capsulessodium bicarbonatesodium citrate

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Area of Science:

  • Exercise Physiology
  • Nutritional Biochemistry
  • Sports Science

Background:

  • Sodium bicarbonate and sodium citrate are commonly used as ergogenic aids.
  • Understanding their comparative efficacy and tolerance is crucial for athletes.
  • Delayed-release formulations aim to mitigate gastrointestinal distress.

Purpose of the Study:

  • To compare the bicarbonate kinetics and gastrointestinal (GI) symptom responses between an equal dose of sodium bicarbonate and sodium citrate.
  • To evaluate the impact of delayed-release capsules on these parameters.

Main Methods:

  • A double-blind, randomized crossover study involving thirteen active males.
  • Participants consumed 0.3 g/kg body mass of sodium bicarbonate, sodium citrate, or a placebo.
  • Blood bicarbonate concentration, pH, and GI symptoms were measured for 180 minutes post-consumption.

Main Results:

  • Both sodium bicarbonate and sodium citrate significantly increased blood bicarbonate levels and pH.
  • Sodium bicarbonate resulted in significantly higher peak and sustained blood bicarbonate concentrations and pH compared to sodium citrate.
  • Mean GI symptom scores were lower with sodium citrate than with sodium bicarbonate, despite considerable inter-individual variability.

Conclusions:

  • Sodium bicarbonate is more effective at increasing blood bicarbonate levels and pH than an equivalent dose of sodium citrate.
  • Sodium citrate may offer a more tolerable alternative due to reduced gastrointestinal symptoms.
  • Further research is needed to optimize dosing and formulation for ergogenic benefits while minimizing side effects.