Lecture On Acid-Base Balance Masterclass: Henderson-Hasselbalch Equation & Body Buffers | MBBS

Описание: In this comprehensive biochemistry lecture for the MBBS 2025-2026 batch at Santiniketan Medical College & Hospital, we explore the vital physiological mechanisms of Acid-Base Balance. This session provides a step-by-step derivation of the Henderson-Hasselbalch Equation, an analysis of physiological buffer systems, and an introduction to clinical disorders like metabolic and respiratory acidosis/alkalosis.

What You Will Learn:

Fundamentals of Acids & Bases: Defining proton donors and acceptors and their role in maintaining blood pH within a narrow range (7.35–7.45) [04:53].

Understanding pH & Hydrogen Concentration: Exploring the inverse relationship between [H+] and pH, and why every 10-fold change in concentration shifts pH by 1 unit [14:06].

Henderson-Hasselbalch Equation Derivation: A detailed guide on how to calculate pH for weak acids and buffers using the dissociation constant (pKa​) [25:42].

Physiological Buffer Systems:

Bicarbonate Buffer: The major extracellular buffer (HCO3−​/H2​CO3​) and the significance of the 20:1 ratio in maintaining a pH of 7.4 [43:42].

Phosphate Buffer: Understanding its role as a primary intracellular buffer with a pKa​ of 6.8 [54:11].

Hemoglobin & Protein Buffers: Their specific roles in RBCs and cellular compartments [43:12].

Clinical Intro to Acid-Base Disorders: How shifts in the bicarbonate-to-pCO2​ ratio lead to Metabolic and Respiratory Acidosis/Alkalosis [51:47].

Mathematics of Blood pH: Converting 40 nmol/L of hydrogen ions into the physiological pH of 7.4 [57:09].

Key Timestamps:

[01:26] The four major acid-base disorders introduced.

[08:02] Defining Molar Concentration and Gram Molecular Weight.

[17:36] Neutral pH of water vs. Physiological pH of blood.

[20:03] Survival ranges: Why pH below 6.8 or above 7.8 is fatal.

[30:50] High Yield: The 20:1 Bicarbonate/Carbonic Acid ratio.

[35:01] How buffers minimize pH shifts when acids/alkalis are added.

[48:36] Converting pCO2​ to Carbonic Acid using the 0.03 solubility coefficient.

[55:33] Phosphate Buffer: Calculating the 4:1 ratio for intracellular balance.

[57:35] Solving the pH equation for 40 nmol/L hydrogen concentration.


SANTINIKETAN MEDICAL COLLEGE & HOSPITAL
Real Classroom Demonstration/Lecture
On: BIOCHEMISTRY by Prof. (Dr.) Tridibeswar Mondal
(MBBS Batch: 2025-26)
Conducted on: 21-01-26