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Related Concept Videos

Bicarbonate-Carbonic Acid Buffer01:22

Bicarbonate-Carbonic Acid Buffer

The carbonic acid-bicarbonate buffer system is critical for maintaining the body's pH balance. It operates on the equilibrium:
Buffer Systems in the Body01:19

Buffer Systems in the Body

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 anion,...
Buffer Effectiveness02:19

Buffer Effectiveness

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...
Buffers: Overview01:30

Buffers: Overview

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).
Buffers02:56

Buffers

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...
Phosphate Buffer01:22

Phosphate Buffer

The phosphate buffer system is a critical biological mechanism for maintaining pH stability in the body. This system operates primarily through two components: sodium dihydrogen phosphate (NaH2PO4), which acts as a weak acid, and sodium hydrogen phosphate (Na2HPO4), which serves as a weak base.
Sodium dihydrogen phosphate does not fully dissociate in neutral or acidic solutions. When a strong base, such as sodium hydroxide (NaOH), is introduced into the solution, sodium dihydrogen phosphate...

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Related Experiment Video

Updated: Jun 21, 2026

Anionic Polymerization of an Amphiphilic Copolymer for Preparation of Block Copolymer Micelles Stabilized by π-π Stacking Interactions
10:53

Anionic Polymerization of an Amphiphilic Copolymer for Preparation of Block Copolymer Micelles Stabilized by π-π Stacking Interactions

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Physiological bicarbonate buffers: stabilisation and use as dissolution media for modified release systems.

Hala M Fadda1, Hamid A Merchant, Basel T Arafat

  • 1Department of Pharmaceutics, The School of Pharmacy, University of London, 29-39 Brunswick Square, London, WC1N 1AX, United Kingdom.

International Journal of Pharmaceutics
|August 12, 2009
PubMed
Summary

Bicarbonate buffers better predict in vivo mesalazine release than phosphate buffers. Stabilized bicarbonate media revealed similar drug release patterns for Mezavant and Asacol, aligning with human pharmacokinetics.

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Area of Science:

  • Pharmaceutical Sciences
  • Drug Delivery
  • Gastrointestinal Physiology

Background:

  • Bicarbonate media mimic small intestinal fluid composition and buffering.
  • In vitro dissolution testing requires stable bicarbonate buffers for accurate drug release studies.

Purpose of the Study:

  • To investigate methods for stabilizing bicarbonate buffers for USP-II dissolution apparatus.
  • To compare the in vitro drug release of enteric-coated mesalazine products in bicarbonate versus phosphate buffers.

Main Methods:

  • Three mesalazine products (Asacol 400 mg, Asacol 800 mg HD, Mezavant 1200 mg) were tested.
  • Dissolution studies were conducted in pH 7.4 Krebs bicarbonate and phosphate buffers.
  • Bicarbonate stabilization techniques included CO(2) sparging, liquid paraffin overlay, and a custom seal device.

Main Results:

  • All products showed delayed drug release in bicarbonate media compared to phosphate buffer.
  • Mezavant exhibited zero-order, sustained release in phosphate buffer but a different profile in bicarbonate.
  • Mesalazine release patterns in bicarbonate media correlated with human pharmacokinetic data.

Conclusions:

  • Stabilized bicarbonate media offer a more predictive in vitro model for mesalazine enteric-coated formulations.
  • The in vitro release profiles in bicarbonate media align with in vivo performance, aiding formulation development.