Question

What is the \(\text{P}^{OH}\) of solution having \([\text{H}_{3}\text{O}^{+}]1\times 10^{-4}\) at \(298\) K?

• A. \(4\)
• B. \(10\)
• C. \(1\)
• D. \(12\)

Hint:

Find pH from the hydronium concentration, then use pH plus pOH equal to 14.

Answer 1

The Correct Option is B

Step 1: Understanding the Concept
\(\text{pH}=-\log[\text{H}_3\text{O}^{+}]\), and at 298 K \(\text{pH}+\text{pOH}=14\).

Step 2: pH
\(\text{pH}=-\log(1\times10^{-4})=4\)

Step 3: Calculation
\(\text{pOH}=14-4=10\)

Step 4: Compare the options
The value 10 matches option (B).

Final Answer:
The pOH of the solution is 10. \[ \boxed{\text{(B) }\text{10}} \]