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To solve this problem, let's go through the required steps.

Given dataTo solve this problem, let's go through the required steps.

Given 
- \( \text{pOH} = 12.91 \)
- Temperature = 25°C, so \( \text{pH} + \text{pOH} = 14 \) (since this is the ion-product constant of water at this temperature)

### Step 1: Calculate pH
Using the relationship:
\[
\text{pH} = 14 - \text{pOH}
\]
\[
\text{pH} = 14 - 12.91 = 1.09
\]

### Step 2: Calculate \([OH^-]\)
We know that:
\[
\text{pOH} = -\log [\text{OH}^-]
\]
Rearranging to solve for \([OH^-]\):
\[
[\text{OH}^-] = 10^{-\text{pOH}}
\]
\[
[\text{OH}^-] = 10^{-12.91} \approx 1.23 \times 10^{-13} \, \text{M}
\]

### Step 3: Calculate \([H^+]\)
Similarly, we can find \([H^+]\) using the relationship with pH:
\[
\text{pH} = -\log [\text{H}^+]
\]
\[
[\text{H}^+] = 10^{-\text{pH}}
\]
\[
[\text{H}^+] = 10^{-1.09} \approx 8.13 \times 10^{-2} \, \text{M}
\]

### Summary of Results
- \([H^+] = 8.13 \times 10^{-2} \, \text{M}\)
- \([OH^-] = 1.23 \times 10^{-13} \, \text{M}\)
- \(\text{pH} = 1.09\)

Would you like additional details or have any questions?

---

1. How do we calculate pOH if only pH is given?
2. What is the relationship between pH, pOH, and the temperature of water?
3. How does temperature affect the ion-product constant of water?
4. What is the significance of a high pOH value in a solution?
5. Can we determine the concentration of other ions in solution based on pH?

**Tip:** Remember that for pure water at 25°C, pH and pOH always add up to 14 due to the ion-product constant, \( K_w \).

Determine the [H+], [OH-], and pH of a solution with a pOH of 12.91 at 25 °C.

Find the hydrogen ion concentration [H+], hydroxide ion concentration [OH-], and pH for a solution with a pOH of 12.91 at 25 °C. Learn how to use the pH + pOH relationship and logarithmic functions to determine these values.

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