Question:
Determine the \([\text{OH}^{-}]\) of a solution of weak base BOH having its pH \(9.75\) at \(298\) K.
Determine the \([\text{OH}^{-}]\) of a solution of weak base BOH having its pH \(9.75\) at \(298\) K.
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Find pOH as 14 minus pH, then convert pOH to the hydroxide concentration.
Updated On: Nov 12, 2026
- \(6.512\times 10^{-5}\) M
- \(5.623\times 10^{-5}\) M
- \(4.647\times 10^{-5}\) M
- \(3.540\times 10^{-5}\) M
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The Correct Option is B
Solution and Explanation
Step 1: Understanding the Concept
At 298 K, \(\text{pH}+\text{pOH}=14\), and \([\text{OH}^-]=10^{-\text{pOH}}\).
Step 2: Find pOH
\(\text{pOH}=14-9.75=4.25\).
Step 3: Concentration
\([\text{OH}^-]=10^{-4.25}=10^{-5}\times10^{0.75}=5.623\times10^{-5}\) M.
Final Answer:
The hydroxide ion concentration is \(5.623\times10^{-5}\) M. \[ \boxed{\text{(B) }5.623\times10^{-5}\text{ M}} \]
At 298 K, \(\text{pH}+\text{pOH}=14\), and \([\text{OH}^-]=10^{-\text{pOH}}\).
Step 2: Find pOH
\(\text{pOH}=14-9.75=4.25\).
Step 3: Concentration
\([\text{OH}^-]=10^{-4.25}=10^{-5}\times10^{0.75}=5.623\times10^{-5}\) M.
Final Answer:
The hydroxide ion concentration is \(5.623\times10^{-5}\) M. \[ \boxed{\text{(B) }5.623\times10^{-5}\text{ M}} \]
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