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To calculate the concentration of hydronium ions \([H_3O^+]\) from the given pH, we use the formula:

\[
[H_3O^+] = 10^{-\text{pH}}
\]

In this case, the pH is 4.35. Plugging this value into the formula:

\[
[H_3O^+] = 10^{-4.35}
\]

Now let's calculate it:

\[
[H_3O^+] \approx 4.47 \times 10^{-5} \, \text{M}
\]

Thus, the concentration of \([H_3O^+]\) is approximately \(4.47 \times 10^{-5}\) M.

Would you like more details on the calculation or any clarifications?

Here are 5 related questions you might find useful:
1. How does pH relate to the strength of an acid?
2. How is the pH scale defined and what does it represent?
3. What is the significance of hydronium ion concentration in a solution?
4. How can you calculate pOH from the pH of a solution?
5. What is the relationship between \( [OH^-] \) and \( [H_3O^+] \)?

**Tip:** The pH scale is logarithmic, meaning each whole number change represents a tenfold difference in \( [H_3O^+] \).

Calculate the [H3O+] of a solution with a pH of 4.35?

Learn how to find the concentration of hydronium ions [H3O+] in a solution with a pH of 4.35 using the formula [H3O+] = 10^(-pH). Understand the relationship between pH and hydronium ion concentration, and see step-by-step calculations for this logarithmic function. Suitable for high school students.

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