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Related Concept Videos

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...
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...
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,...
Buffers: Buffer Capacity01:09

Buffers: Buffer Capacity

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 acid...
Protein Buffers in Blood Plasma and Cells01:20

Protein Buffers in Blood Plasma and Cells

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...

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Common stock solutions, buffers, and media

    Current Protocols in Cytometry
    |September 5, 2008
    PubMed
    Summary
    This summary is machine-generated.

    This study details recipes for essential laboratory solutions, including cell lysis and buffer preparations. These detailed protocols support molecular biology and cell culture research, ensuring reproducible experimental results.

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    Area of Science:

    • Molecular Biology
    • Cell Biology
    • Biochemistry

    Background:

    • Standardized laboratory reagents are crucial for reproducible scientific experiments.
    • A comprehensive list of commonly used solutions facilitates research workflows.

    Purpose of the Study:

    • To provide detailed recipes for frequently used laboratory solutions.
    • To serve as a reference for preparing reagents in molecular biology and cell culture.

    Main Methods:

    • Preparation of solutions including Ammonium chloride lysing solution, Complete DMEM, Complete RPMI, DL-dithiothreitol (DTT), and Ethylenediamine tetraacetic acid (EDTA).
    • Formulation of Ethidium bromide staining solution, Fetal bovine serum (FBS), Formamide, Gel loading buffer, L-Glutamine, and Hanks' buffered salt solution (HBSS).
    • Detailed recipes for Phosphate-buffered saline (PBS), RNase A stock solution, Sodium chloride sodium citrate (SSC), Tris-acetate-EDTA (TAE) buffer, Tris-borate-EDTA (TBE) buffer, Tris-EDTA (TE) buffer, and Tris-HCl (TrisCl).

    Main Results:

    • Established protocols for preparing 20 essential laboratory solutions.
    • Solutions cover cell lysis, cell culture media, buffers, and staining reagents.
    • Recipes include concentrations and necessary components for accurate preparation.

    Conclusions:

    • The provided recipes ensure the accurate and reproducible preparation of critical laboratory reagents.
    • This resource supports researchers in molecular biology, cell culture, and biochemistry.
    • Standardized reagent preparation enhances the reliability of experimental outcomes.