What is Henderson-Hasselbalch equation with example?

We can determine the moles of acetic acid by using M = mol/L, which gives us mol = ML = (2M) * (0.5L) = 1mol acetic acid. If we use the Hendersen Hasselbach equation we can see that the pH equals the pKa when the concentration of conjugate base (acetate) equals the concentration of acid.

What is the Henderson-Hasselbalch equation and why is it important?

Henderson Hasselbalch Equation Definition The Henderson-Hasselbalch equation is the equation commonly used in chemistry and biology to determine the pH of a solution. This equation shows a relationship between the pH or pOH of the solution, the pKa or pKb, and the concentration of the chemical species involved.

What is the importance of Henderson-Hasselbalch equation?

Significance of Henderson – Hassel Balch equation: It is used to calculate the concentration of acid and salt when information of pH and total concentration of buffer solution is given. It is used to calculate the pH of buffer solution.

What is Henderson Hasselbalch used for?

The Henderson–Hasselbalch equation can be used to calculate the amount of acid and conjugate base to be combined for the preparation of a buffer solution having a particular pH, as demonstrated in the following problem.

What are buffers with examples?

In general, a buffer solution may be made from known quantities of a weak acid and a salt of the weak acid. Some examples of buffers are phosphate buffer (H2PO- and HPO2) ; acetate buffer (CH3COOH and CH3COO-). The pH of a buffer solution varies directly with the ratio of concentrations of its base and acid members.

How are buffers used in drugs?

In the pharmaceutical field, biological buffers are usually used to maintain the specific pH value. Ensure the stability of drug components: Maintain the pH value of essential components of the drug from being changed or degraded by the gastrointestinal environment, such as aspirin.

What are the examples of pharmaceutical buffers?

Commonly used buffers

• Sodium phosphate. Sodium phosphate (pKa 2.1, 7.2, and 12.3) is the most commonly used buffer found in parenteral formulations (Table 1).
• Citric acid.
• Acetic acid.
• Tromethamine.
• Histidine.
• Gluconic, lactic and tartaric acid.
• Aspartic and glutamic acid.
• Citric acid cycle intermediates.

What is the importance of buffer in pharmacy?

The primary purpose and importance of buffers in pharmacy is to protect pharmaceutical preparations from any sudden change in pH even when limited concentrations of acid or base are added.

Why buffers are used in pharmaceutical formulation?

What is the role of buffer in pharmaceutical preparation?