Question

A patient with severe metabolic acidosis has a blood plasma $\mathrm{pH}$of $6.92$. What is the localid="1653994519831" $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$of the blood plasma?

Short answer

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

Step-by-step solution

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

Explanation 

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

localid="1653994543487" $$\begin{gathered} \left[H_3{O}^{+}\right]\left[O{H}^{-}\right]=1.0\times {10}^{-14} \\ pH=-\log H_3{O}^{+}] \\ pOH=-\log (O{H}^{-}) \end{gathered}$$

localid="1653994558542" $$\begin{gathered} \left[H_3{O}^{+}\right]={10}^{-pH} \\ ={10}^{-6.92} \\ =1.20\times {10}^{-7}M \end{gathered}$$

As a result, the concentration of the component is determined