To solve for the pH and pOH of a blood sample with a given concentration of hydrogen ions \(\([H^+]\)\) equal to \(\(7.2 \times 10^8\)\)M, we need to follow these steps:
1. Calculate the pH: The pH of a solution is determined using the formula:
\(\[
\text{pH} = -\log_{10}[H^+]
\]\)
Given the concentration \(\([H^+] = 7.2 \times 10^8\)\) M, we plug this value into the formula to find the pH.
After performing the calculation, we find that:
\(\[
\text{pH} = -\log_{10}(7.2 \times 10^8) = -8.8573 \text{ (approximately)}
\]\)
2. Calculate the pOH: The pOH of a solution is related to the pH by the equation:
\(\[
\text{pH} + \text{pOH} = 14
\]\)
We can rearrange this equation to solve for pOH:
\(\[
\text{pOH} = 14 - \text{pH}
\]\)
Substituting the calculated pH value, we get:
\(\[
\text{pOH} = 14 - (-8.8573) = 22.8573 \text{ (approximately)}
\]\)
Therefore, the pH and pOH of the blood sample are approximately:
- pH = -8.8573
- pOH = 22.8573
