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. Group of answer choices 5.5 × 10-10 M, neutral 9.2 × 10-1 M, basic 9.2 × 10-1 M, acidic 1.8 × 10-10 M, basic

The correct option is option (D).

Therefore the concentration of is 1.8×10⁻¹⁰ M and it is basic in nature.

Explanation:

List of pH:

pH of a solution is = - log₁₀[H₃O⁺]

We know that,

[H₃O⁺][OH⁻] = =  (at 25°C)

Taking log both sides

log ([H₃O⁺][OH⁻]) =log =log

⇒log[H₃O⁺]+log[OH⁻] = log = -14 log 10

[since log(mn)= log m + log n, ]

⇒ - log[H₃O⁺] - log[OH⁻] = - (-14)  [ log 10 =1]

⇒pH+pOH =14.

Given that,

The concentration of OH⁻ is 5.5 × 10⁻⁵ M

[H₃O⁺][OH⁻] = =

⇒[H₃O⁺] 5.5 × 10⁻⁵ M=10⁻¹⁴

⇒[H₃O⁺] = 1.8×10⁻¹⁰ M

Now check the pH of the solution.

[H₃O⁺] = 1.8×10⁻¹⁰

Taking log both sides

log [H₃O⁺] =log( 1.8×10⁻¹⁰)

⇒ -log [H₃O⁺] = - log( 1.8×10⁻¹⁰)

⇒ pH = - log( 1.8×10⁻¹⁰)

⇒ pH =9.7.

So the nature of solution is basic.

Therefore the concentration of is 1.8×10⁻¹⁰ M and it is basic in nature.

sry but any answer choices

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i think? ?