Q. 10.43 - An Introduction to General, Organic, and Biological Chemistry

Question

A patient with severe metabolic acidosis has a blood plasma $\mathrm{pH}$ of $6.92$. What is the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$of the blood plasma?

Step-by-Step Solution

Answer

The$\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$of the blood plasma is determined as $1.20\times {10}^{-7} M$

Step 1 : Introduction

The given is the condition of the patient with severe metabolic acidosis

The objective is to determine what is the $H_3{O}^{+}$of the blood plasma

Step 2 : Explanation

The negative logarithmic (base 10) representation of pH is used in mathematics $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$.

$$\begin{gathered} \left[H_3{O}^{+}\right]\left[O{H}^{-}\right]=1.0 \times {10}^{-14} \\ pH=-\log H_3{O}^{+}] \\ pOH=-\log (O{H}^{-}) \end{gathered}$$

$$\begin{gathered} \left[H_3{O}^{+}\right]={10}^{-pH} \\ ={10}^{-6.92} \\ =1.20 \times {10}^{-7}M \end{gathered}$$

As a result, the concentration of the component is determined