Answer:
1.41 × 10⁻¹⁰ M
Explanation:
We have a solution with a pH of 9.85 at 25 °C. We can calculate the concentration of H⁺ using the following expression.
pH = -log [H⁺]
[H⁺] = antilog -pH
[H⁺] = antilog -9.85
[H⁺] = 1.41 × 10⁻¹⁰ M
H⁺ is usually associated with water molecules forming hydronium ions.
H⁺ + H₂O → H₃O⁺
Then, the concentration of H₃O⁺ ions is 1.41 × 10⁻¹⁰ M.
Answer:
The hydronium ion concentration for a solution with pH 9.85 = 1.41 *10^-10M
Explanation:
Step 1: data given
pH = 9.85
Temperature = 25.0 °C
the hydronium ion concentration = [H3O+] = [H+]
Step 2: Calculate the hydronium ion concentration
[H3O+] = [H+]
pH = -log[H+]
9.85 = -log[H+]
[H+] = 10^-9.85
[H+] = 1.41 *10^-10M = [H3O+]
The hydronium ion concentration for a solution with pH 9.85 = 1.41 *10^-10M
