   Chapter 7, Problem 9RQ

Chapter
Section
Textbook Problem

If a patient has a level of 70 mm Hg, what is the H 2 CO 3 concentration?A. 1.3 mEq/LB. 1.5 mEq/LC. 1.7 mEq/LD. 2.1 mEq/L

Summary Introduction

Introduction:

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

H-AH++A-acid            base

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

pH=pK+log[HCO3][PCO2×0.03]

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.

Explanation

Explanation for the correct answer:

Option (D) is given as 1.7 mEq/L. In the equation below:

[HCO3]= antilog(7.406.1)×(PCO2×0.03)= antilog(1.3)×(70×0.03)=19.5×2.1=40.95

HCO3H2CO3=201H2CO3=40

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 