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Let's walk through the solution to this problem step-by-step. 

### Given:
- \([H^+] = 4.8 \times 10^{-12} \, M\)
- Temperature \(T = 25^\circ C\)

We need to find:
1. **[OH⁻] concentration**  
2. **pH**  
3. **pOH**  

---

### 1. Calculating the pH
The formula for pH is:
\[
\text{pH} = -\log [H^+]
\]
\[
\text{pH} = -\log (4.8 \times 10^{-12})
\]

Using logarithmic calculations:
\[
\text{pH} = -( \log(4.8) + \log(10^{-12}) )
\]
\[
\text{pH} = -(0.681 + (-12)) = 11.319
\]

So:
\[
\text{pH} \approx 11.32
\]

---

### 2. Calculating pOH
Since:
\[
\text{pH} + \text{pOH} = 14 \quad \text{(at 25°C)}
\]
\[
\text{pOH} = 14 - \text{pH} = 14 - 11.32 = 2.68
\]

---

### 3. Calculating [OH⁻] concentration
The relationship between \([H^+]\) and \([OH^-]\) is given by the water ionization constant:
\[
[H^+][OH^-] = 1.0 \times 10^{-14} \quad \text{(at 25°C)}
\]
\[
[OH^-] = \frac{1.0 \times 10^{-14}}{4.8 \times 10^{-12}}
\]
\[
[OH^-] = 2.08 \times 10^{-3} \, M
\]

---

### Final Answers:
1. \([OH^-] = 2.08 \times 10^{-3} \, M\)  
2. \(pH \approx 11.32\)  
3. \(pOH \approx 2.68\)

---

Do you need any further details or clarifications?

Here are five related questions:
1. How does temperature affect the pH and pOH relationship?
2. What happens to the concentration of \([OH^-]\) if the \([H^+]\) increases?
3. How can we determine if the solution is acidic, neutral, or basic based on pH?
4. What is the significance of the water ionization constant \(K_w\)?
5. How do strong acids and bases affect pH and pOH?

**Tip:** Remember that a solution is considered basic if the pH is greater than 7, neutral at pH 7, and acidic if the pH is less than 7.

Determine the [OH⁻], pH, and pOH of a solution with a [H⁺] of 4.8 x 10⁻¹² M at 25 °C.

Learn how to calculate the hydroxide ion concentration [OH⁻], pH, and pOH of a solution with a hydrogen ion concentration [H⁺] of 4.8 x 10⁻¹² M at 25°C. This solution involves key concepts in acid-base equilibria, including logarithmic calculations and the water ionization constant. Suitable for high school chemistry students.

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