Calculate the concentration of h3o in a solution that contains 5.5 × 10-5 m oh- at 25°c. identify the solution as acidic, basic, or neutral.

[H₃O⁺] = 1.81.10⁻¹⁰

pH of the solution = 9,742, is a basic solution

pH is the degree of acidity of a solution that depends on the concentration of H ions. The greater the value the more acidic the solution and the smaller the pH.

pH = - log [H⁺]

So that the two quantities between pH and [H⁺] are inversely proportional because they are associated with negative values.

A solution whose value is different by n has a difference in the concentration of H ions of 10ⁿ.

The concentration of hydronium ions determines a solution's pH.

H₂O ionization reaction

2 H₂O ⇌ OH− + H₃O⁺

The water equilibrium constant (Kw) is the product of concentration

the ions:

Kw = [H₃O +] [OH-]

Kw value at 25° C = 10⁻⁴

It is known [OH-] = 5.5 × 10⁻⁵

then the concentration of H₃O⁺:

10⁻¹⁴ = [H₃O⁺]. 5.5 × 10⁻⁵

 [H₃O⁺] = 10⁻¹⁴: 5.5 × 10⁻⁵

 [H₃O⁺]= 1.81.10⁻¹⁰

pH - -log [H₃O⁺]

pH = - log 1.81.10⁻¹⁰

pH = 9,742

Because the pH > 7, the solution is said to be a basic solution

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i think its 100

i hope this !