Inorganic Chemistry (14) Buffer = Definition, Types, Properties | Henderson -Hasselbalch Equation

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Contents for 2nd Unit of Inorganic Chemistry -

(01) Acids, Bases and Buffers: Buffer equations and buffer capacity in general, buffers in pharmaceutical systems, preparation, stability, buffered isotonic solutions, measurements of tonicity, calculations and methods of adjusting is tonicity.

(02) Major extra and intracellular electrolytes: Functions of major physiological ions, Electrolytes used in the replacement therapy: Sodium chloride*, Potassium chloride, Calcium gluconate* and Oral Rehydration Salt (ORS), Physiological acid-base balance.

(03) Dental products: Dentifrices, the role of fluoride in the treatment of dentalcare, Desensitizing agents, Calcium carbonate, Sodium fluoride, and Zinc eugenol cement.

Buffer Solution
A buffer solution refers to an aqueous solution. Furthermore, it consists of a mixture of a weak acid and its conjugate base or vice-versa. This solution is quite important in the field of chemistry. You can explore more about buffer solutions here.

Definition of Buffer Solution
Buffer solution or simply called buffer in analytical chemistry or biology is a solution whose pH remains virtually unchanged upon the addition of small amounts of strong acids or bases. A buffer solution may be made up of an acid and its conjugate base or a base and its conjugate acid.

The use of conjugate solutions is significantly important in buffer solutions. We used buffer solutions in order to keep pH at a somewhat constant value. This has a wide variety of chemistry applications.

Application of Buffer Solution
1. Buffer solutions certainly have a massive range of applications. The applications of buffer solutions are for both the real world and the lab.

2. A buffered pH is a necessity of most enzymes to function efficiently and correctly. Furthermore, buffering is important for ensuring proper colour concentration when using dyes.

3. A buffer solution is required for calibrating equipment. It is especially required for pH meters that may be in the miscalibrated in the absence of a buffer.

4. Buffer solutions whose preparation takes place from acetic acid, citric acid, ammonia, can have pH values as high as 10 or as low as 2. This allows buffer solutions to be worked with very strong bases or acids.

Properties of Buffer Solution
Buffer solutions are certainly resistant to changes in pH. However, the pH of a buffer solution can change if there is an addition of sufficient strong acid or strong base.

Buffer capacity refers to the amount of strong acid or base a buffer solution can take before significant pH changes take place. It is a measure of the resistance of a buffer solution to pH change on the addition of hydroxide ions.

Buffer capacity differs in accordance with the core components of the buffer solution and the amount of strong acid or base. If adding a strong acid to buffer solutions, the capacity is equal to the ba

Types of buffers
Buffer solutions consist of either a weak acid or weak base and its salts. Therefore, buffers are broadly divided into two types,
1. Acid buffer
2. Alkali buffer

1. Acid buffers
Acid buffers are the mixture of a weak acid and its salt. A mixture of acetic acid and sodium acetate in a certain proportion is an example of an acid buffer solution. If a few drops of strong base sodium hydroxide are added to this acid buffer, the dissociated OH− ions will be consumed by weak acetic acid. Therefore, the pH of the buffer system remains unchanged.

Alkali buffers
Alkali buffers are the mixture of a weak base and its salt. A mixture of ammonium hydroxide and ammonium chloride in a certain proportion is an example of an alkali buffer solution.

Buffer action
The buffer action maintains steady pH by adjusting the equilibrium between a weak acid or a weak base and its conjugate ions.


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