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To calculate the pH of a solution, we use the formula:

\[
\text{pH} = -\log[\text{H}_3\text{O}^+]
\]

Given that \([ \text{H}_3\text{O}^+ ] = 4.5 \times 10^{-7}\), we can substitute this value into the equation:

\[
\text{pH} = -\log(4.5 \times 10^{-7})
\]

Using logarithms:

\[
\text{pH} \approx -(\log(4.5) + \log(10^{-7})) = -(0.6532 - 7)
\]

\[
\text{pH} \approx 7 - 0.6532 = 6.35
\]

So, the pH of the solution is approximately **6.35**.

Would you like further details on the calculation or have any questions?

Here are five related questions:
1. What is the pH of a solution with \([ \text{H}_3\text{O}^+ ] = 1 \times 10^{-4}\)?
2. How do you convert pH to \([ \text{H}_3\text{O}^+ ]\)?
3. What is the relationship between pH and pOH?
4. How does temperature affect the pH of water?
5. What is the pH of a neutral solution at 25°C?

**Tip:** The pH scale ranges from 0 to 14. A pH less than 7 indicates acidity, while a pH greater than 7 indicates basicity.

Calculate the pH of a solution with [H3O+] = 4.5 × 10⁻⁷.

Calculate the pH of a solution with a hydronium ion concentration of 4.5 × 10⁻⁷ using the formula pH = -log[H3O+]. This step-by-step guide shows the use of logarithms to determine that the pH is approximately 6.35. Ideal for high school chemistry students.

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