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This table involves calculating pH and hydronium ion concentration \([H_3O^+]\) for different solutions, based on the given values. The relationship between \([H_3O^+]\) and pH is expressed by the equation:

\[
\text{pH} = -\log[H_3O^+]
\]

Let's complete the table step by step:

1. **For Solution A:**
   - \([H_3O^+]\) is given as \(4.8 \times 10^{-7}\) mol/L.
   - Using the pH formula:
     \[
     \text{pH} = -\log(4.8 \times 10^{-7}) \approx 6.32
     \]
     So, the pH of Solution A is approximately **6.32**.

2. **For Solution B:**
   - pH is given as 3.25.
   - Rearranging the pH formula to find \([H_3O^+]\):
     \[
     [H_3O^+] = 10^{-\text{pH}} = 10^{-3.25} \approx 5.62 \times 10^{-4} \, \text{mol/L}
     \]
     So, \([H_3O^+]\) for Solution B is approximately **\(5.62 \times 10^{-4}\)** mol/L.

3. **For Solution C:**
   - \([H_3O^+]\) is given as \(1.8 \times 10^{-9}\) mol/L.
   - Using the pH formula:
     \[
     \text{pH} = -\log(1.8 \times 10^{-9}) \approx 8.74
     \]
     So, the pH of Solution C is approximately **8.74**.

### Completed Table:

| Solution | \([H_3O^+]\) (mol/L)     | pH     |
|----------|--------------------------|--------|
| A        | \(4.8 \times 10^{-7}\)    | 6.32   |
| B        | \(5.62 \times 10^{-4}\)   | 3.25   |
| C        | \(1.8 \times 10^{-9}\)    | 8.74   |

Would you like further details or clarifications?

### 5 Related Questions:
1. How is the pH scale defined, and what do its values represent?
2. What is the difference between a strong acid and a weak acid in terms of \([H_3O^+]\)?
3. How can temperature affect the pH of a solution?
4. Why is pH = 7 considered neutral at 25°C?
5. How does the logarithmic nature of pH impact small changes in \([H_3O^+]\)?

### Tip:
Always ensure the use of the correct number of significant digits when working with logarithms and pH calculations to maintain precision.

Complete the table by calculating pH or hydronium ion concentration for different solutions at 25°C.

Learn how to calculate the pH and hydronium ion concentration of different solutions using the formula pH = -log[H3O+]. Includes example solutions and step-by-step instructions for high school students.

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