   Chapter 7, Problem 10RQ

Chapter
Section
Textbook Problem

The value of the pK in the Henderson- Hasselbalch equation isA. 1.0B. 6.1C. 7.4D. 20.1

Summary Introduction

Introduction:

In biochemical reactions, the Henderson–Hasselbalch equation can be used to determine the pH (potential of hydrogen) of a buffer solution, when the concentration of the acid and that of its conjugate base are given.

H-AH++Aacid                 base

logKa=log[H+]+log([A]/[HA])pKa=pH=log([A]/[HA])therefore,pH=pKa+log[(ionized/unionized)]

Thus, the Henderson–Hasselbalch equation applied during normal conditions in the blood is,

pH=pK+log[HCO3][PCO2×0.03]

This equation helps to calculate bicarbonate ion concentration.

Explanation

Explanation/justification for the correct answer:

Option (B) is given as 6.1. In the equation below,

pH=pK+log[HCO3][PCO2×0.03]

Under normal conditions, pH= 7.4

pH=pK+log[HCO3][PCO2×0.03]7.4=pK+log2440×0

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