Chapter 7, Problem 9RQ

Summary Introduction

Introduction:

The acid–base reaction equation can be given as follows:

$\begin{array}{l}\text{H-A}\rightleftarrows {\text{H}}^{\text{+}}{\text{+A}}^{\text{-}}\\ \text{acid base}\end{array}$

Furthermore, the Henderson–Hasselbalch equation applied during normal conditions in the blood is given as follows:

$\text{pH}=\text{pK}+\log \frac{[{\text{HCO}}_{\text{3}}^{-}]}{[{\text{P}}_{\text{CO2}}\times \text{0}\text{.03]}}$

This equation helps to calculate the bicarbonate ion concentration. pH is defined as the negative logarithm of base 10 of the hydrogen ion concentration. pK is a logarithmic value of the dissociation constant.