g Calculate the concentration of hydronium in a solution that contains 5.5x10-5 M OH - at 25C. Indentify the solution as acidic, basic, or neutral. 1.8x10-10 M, basic 9.2x10-1 M, acidic 1.8x10-10 M, acidic 9.2x10-1 M, basic 5.5x10-10 M, neutral

First option is correct, and it's a basic solution

Explanation:

This is actually pretty easy, the solution contains 5.5x10⁻⁵ M of OH⁻, so all we need to do is calculate the hydronium with the following expression:

Kw = [H₃O⁺] [OH⁻]

Solving for hydronium:

[H₃O⁺] = Kw / [OH⁻]

The value of Kw is 1x10⁻¹⁴, so replacing the values we have:

[H₃O⁺] = 1x10⁻¹⁴ / 5.5x10⁻⁵

[H₃O⁺] = 1.818x10⁻¹⁰ M

This is the concentration of hydronium, so the first option is the correct answer.

To know if this solution is acidic, basic, or neutral, let's calculate the pH:

pH = - log[H₃O⁺]

Replacing:

pH = - log (1.818x10⁻¹⁰)

pH = 9.74

This pH is >7 so this solution is basic.