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Uploaded bySheikhSujon
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presentation Buffer solution

Buffer solutions resist changes in pH upon the addition of acids or bases. There are two types: acidic buffers containing a weak acid and its salt with a strong base; and basic buffers containing a weak base and its salt with a strong acid. Buffer solutions work by neutralizing added H+ or OH- ions through acid-base reactions between the conjugate acid-base pairs. They have many applications where constant pH must be maintained, such as in biological systems, indicator dyes, and strong acid-base reactions.

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Submitted to: Shah Marzia Mahjabin Lina Assistant Professor Department of Pharmacy Stamford University Bangladesh Submitted by: Name: Sujon Mia ID: BPH-06707425 Batch No: 067 Stamford University Bangladsh Mid Assessment 2 : Presentation on Buffer solution Course: Pharmaceutical analysis Course Code: BPH 325 Batch:67
What is buffer solution? Buffer Solution resist a change in pH upon dilution or upon the addition of small amounts of acid or base. There are two types of buffer solution 1. Acidic Buffer 2. Basic Buffer
Acidic Buffer: A weak acid together with a salt of the same acid with a strong base. There are called Acidic Buffer. or Example. CH3COOH + CH3COONa Basic Buffers: A weak base and its salt with a strong acid. There are called Basic Buffers. Example: NH4OH +NH4Cl 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.
Mechanism of Buffer Action In solution, the salt is completely ionized and the weak acid is partly ionized. CH3COONa ⇌ Na+ + CH3COO– CH3COOH ⇌ H+ + CH3COO– On Addition of Acid and Base 1. On addition of acid, the released protons of acid will be removed by the acetate ions to form an acetic acid molecule. H+ + CH3COO– (from added acid) ⇌ CH3COOH (from buffer solution) 2. On addition of the base, the hydroxide released by the base will be removed by the hydrogen ions to form water. HO– + H+ (from added base) ⇌ H2O (from buffer solution)
Preparation of Buffer Solution  If the dissociation constant of the acid (pKa) and of the base (pKb) are known, a buffer solution can be prepared by controlling the salt-acid or the salt-base ratio.  As discussed earlier, these solutions are prepared by mixing the weak bases with their corresponding conjugate acids, or by mixing weak acids with their corresponding conjugate bases.
Application of Buffer Solution Buffer solutions certainly have a massive range of applications. The applications of buffer solutions are for both the real world and the lab.  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. 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.
There exists a few alternate names that are used to refer buffer solutions, such as pH buffers or hydrogen ion buffers. An example of the use of buffers in pH regulation is the use of bicarbonate and carbonic acid buffer system in order to regulate the pH of animal blood.  Buffer solutions are also used to maintain an optimum pH for enzyme activity in many organisms. Uses of Buffer Solutions
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