Be sure to answer all parts. Enter your answers in scientific notation. Calculate the hydronium ion concentrations of the following solutions at 25°C, given the pH. (a) pH=9.58 [H₂O+] = (b) pH = 3.58 [H₂0] = x 10 x 10 M M
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![**Title: Calculating Hydronium Ion Concentrations from pH Values**
**Instructions:**
Be sure to answer all parts. Enter your answers in scientific notation.
**Objective:**
Calculate the hydronium ion concentrations of the following solutions at 25°C, given the pH.
**Problem Statement:**
(a) **pH = 9.58**
\[
[\text{H}_3\text{O}^+] = \underline{\quad\quad} \times 10^{\underline{\quad\quad}} \, \text{M}
\]
(b) **pH = 3.58**
\[
[\text{H}_3\text{O}^+] = \underline{\quad\quad} \times 10^{\underline{\quad\quad}} \, \text{M}
\]
**Explanation:**
To find the concentration of hydronium ions \([\text{H}_3\text{O}^+]\), use the formula:
\[
[\text{H}_3\text{O}^+] = 10^{-\text{pH}}
\]
Please calculate the values and express them in the format of scientific notation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2ceb2d65-29b4-49d4-9830-4ba06589987b%2Fbc5de452-fe66-4e4f-8a37-be43397d1ef2%2Fav6vxi_processed.jpeg&w=3840&q=75)
The relation between pH and [H+] is ->
pH = -log[H+]
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