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To solve this problem, let's go through each part step-by-step. We are given the hydroxide ion concentration, \([OH^-] = 2.3 \times 10^{-9}\) M, at a temperature of 25°C. 

### Step 1: Calculate \([H^+]\)
The product of \([H^+]\) and \([OH^-]\) concentrations in water at 25°C is given by the ion-product constant for water, \(K_w\), which is:

\[
K_w = [H^+][OH^-] = 1.0 \times 10^{-14}
\]

Using this relationship, we can find \([H^+]\) as follows:

\[
[H^+] = \frac{K_w}{[OH^-]} = \frac{1.0 \times 10^{-14}}{2.3 \times 10^{-9}}
\]

Calculating this gives:

\[
[H^+] \approx 4.35 \times 10^{-6} \, \text{M}
\]

### Step 2: Calculate pH
The pH is defined as:

\[
\text{pH} = -\log [H^+]
\]

Substituting \([H^+] = 4.35 \times 10^{-6}\):

\[
\text{pH} \approx -\log(4.35 \times 10^{-6}) \approx 5.36
\]

### Step 3: Calculate pOH
Similarly, the pOH is defined as:

\[
\text{pOH} = -\log [OH^-]
\]

Substituting \([OH^-] = 2.3 \times 10^{-9}\):

\[
\text{pOH} \approx -\log(2.3 \times 10^{-9}) \approx 8.64
\]

### Summary of Answers:
1. \([H^+] = 4.35 \times 10^{-6}\) M
2. \(\text{pH} = 5.36\)
3. \(\text{pOH} = 8.64\)

Would you like further details on these calculations, or do you have any questions?

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Here are five related questions to deepen your understanding:
1. How does temperature affect the value of \(K_w\) and consequently pH and pOH?
2. What is the relationship between pH and pOH at 25°C?
3. How can you determine whether a solution is acidic, neutral, or basic based on pH?
4. Why is water self-ionizing, and what are its effects on pH and pOH?
5. How would you calculate pH and pOH if given \([H^+]\) instead of \([OH^-]\)?

**Tip:** Remember, \(\text{pH} + \text{pOH} = 14\) at 25°C, which helps in quickly verifying calculations.

Determine the [H+], pH, and pOH of a solution with an [OH-] of 2.3 x 10^-9 M at 25 °C.

Learn how to determine the [H+], pH, and pOH of a solution with an [OH-] concentration of 2.3 x 10^-9 M at 25°C. This problem covers key concepts in acid-base chemistry, including the ion-product constant of water and the relationships between pH, pOH, and [H+]. Suitable for students in Grades 10-12.

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