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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m=9

step-by-step explanation:

acid rain does not usually kill trees directly. instead, it is more likely to weaken the trees by damaging their leaves, limiting the nutrients available to them, or poisoning them with toxic substances slowly released from the soil. the main atmospheric pollutants that affect trees are nitrates and sulphates.