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Related Concept Videos

Buffers02:56

Buffers

173.4K
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...
173.4K
Buffers: Buffer Capacity01:09

Buffers: Buffer Capacity

2.5K
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...
2.5K
Buffer Effectiveness02:19

Buffer Effectiveness

55.6K
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...
55.6K
Phosphate Buffer01:22

Phosphate Buffer

5.4K
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...
5.4K
Buffers: Overview01:30

Buffers: Overview

10.2K
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).
10.2K
Calculating pH Changes in a Buffer Solution02:45

Calculating pH Changes in a Buffer Solution

59.0K
A buffer can prevent a sudden drop or increase in the pH of a solution after the addition of a strong acid or base up to its buffering capacity; however, such addition of a strong acid or base does result in the slight pH change of the solution. The small pH change can be calculated by determining the resulting change in the concentration of buffer components, i.e., a weak acid and its conjugate base or vice versa. The concentrations obtained using these stoichiometric calculations can be used...
59.0K

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Mycobacterial DNA Extraction using Bead Beating in Custom Buffer Followed by NGS Workflow
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Buffers.

Michael R Green, Joseph Sambrook

    Cold Spring Harbor Protocols
    |February 14, 2018
    PubMed
    Summary
    This summary is machine-generated.

    Biological reactions require stable pH levels, which can be disrupted by proton changes. Buffers maintain hydrogen ion concentration within acceptable limits for molecular cloning, using substances like Tris, Good, and phosphate buffers.

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    Area of Science:

    • Biochemistry
    • Molecular Biology
    • Biotechnology

    Background:

    • Biological reactions are sensitive to hydrogen ion concentration (pH).
    • Many biological reactions alter pH by generating or consuming protons.
    • Maintaining a stable pH is crucial for reaction efficiency.

    Purpose of the Study:

    • To introduce standard buffers used in molecular cloning.
    • To explain the function of buffers in maintaining pH.
    • To highlight common buffer types in biological research.

    Main Methods:

    • Description of buffer principles.
    • Overview of Tris buffers.
    • Overview of Good buffers.
    • Overview of phosphate buffers.

    Main Results:

    • Buffers maintain hydrogen ion concentration within a narrow, optimal range.
    • Standard buffers like Tris, Good, and phosphate are effective for molecular cloning.
    • Reversible protonation allows buffers to counteract pH changes.

    Conclusions:

    • Buffers are essential for controlling pH in biological systems.
    • Appropriate buffer selection ensures the success of molecular cloning experiments.
    • Understanding buffer mechanisms is key to optimizing biochemical reactions.