Question

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.

Answer 1

we have been given the OH⁻ ion concentration, we can calculate the pOH concentration. 
pOH = -log [OH⁻]
pOH = - log (5.5 x 10⁻⁵ M)
pOH = 4.26
we can then calculate the pH value 
pH + pOH = 14
pH = 14 - 4.26 
pH = 9.74
since pH > 7 the solution is basic.

by knowing the pH value, we can calculate the H₃O⁺ concentration
pH = - log[H₃O⁺]
[H₃O⁺] = antilog (-pH) = antilog (-9.74)
[H₃O⁺] = 1.82 x 10⁻¹⁰ M

Answer 2

[H₃O⁺] = 1.81.10⁻¹⁰

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

Further explanation

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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