Buffer
Buffer
A buffer is a solution that resists changes in pH when small quantities of an acid or an alkali are added to it. Buffers are essential in many areas of chemistry and biology because they help maintain a stable pH environment, which is crucial for various biochemical processes.
Types of Buffers[edit | edit source]
Buffers can be broadly classified into two types:
- Acidic Buffers: These are solutions that have a pH less than 7 and are typically made from a weak acid and one of its salts. An example of an acidic buffer is a solution of acetic acid (Acetic acid) and sodium acetate.
- Basic Buffers: These are solutions that have a pH greater than 7 and are typically made from a weak base and one of its salts. An example of a basic buffer is a solution of ammonia (Ammonia) and ammonium chloride.
Buffer Capacity[edit | edit source]
The buffer capacity is a measure of the efficiency of a buffer in resisting changes in pH. It depends on the concentration of the acid and its conjugate base (or the base and its conjugate acid) in the buffer solution. The higher the concentration of these components, the greater the buffer capacity.
Applications of Buffers[edit | edit source]
Buffers have a wide range of applications in various fields:
- In biochemistry, buffers are used to maintain the pH of biological systems, such as blood, which has a natural buffer system to maintain a pH around 7.4.
- In chemical analysis, buffers are used to maintain the pH of solutions during titrations and other analytical procedures.
- In industrial processes, buffers are used in the manufacture of pharmaceuticals, food products, and other chemicals to ensure the correct pH is maintained.
Common Buffer Systems[edit | edit source]
Some common buffer systems include:
- Phosphate buffer: Used in biological research.
- Tris buffer: Commonly used in molecular biology.
- Citrate buffer: Used in various biochemical applications.
Related Pages[edit | edit source]
See Also[edit | edit source]
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