Respuesta :
Answer:
The correct option is option (D).
Therefore the concentration of [tex]H_3O[/tex] is 1.8×10⁻¹⁰ M and it is basic in nature.
Explanation:
List of pH:
- If pH of a solution is 7, then solution is neutral.
- If pH of a solution is grater than 7, then solution is basic.
- If pH of a solution is less than 7, then solution is acidic.
pH of a solution is = - log₁₀[H₃O⁺]
We know that,
[H₃O⁺][OH⁻] = [tex]K_w[/tex] = [tex]10^{-14}[/tex] (at 25°C)
Taking log both sides
log ([H₃O⁺][OH⁻]) =log [tex]K_w[/tex] =log [tex]10^{-14}[/tex]
⇒log[H₃O⁺]+log[OH⁻] = log[tex]K_w[/tex] = -14 log 10
[since log(mn)= log m + log n, [tex]log( a^b)=b\ log (a)[/tex] ]
⇒ - 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⁻] = [tex]K_w[/tex] = [tex]10^{-14}[/tex]
⇒[H₃O⁺] 5.5 × 10⁻⁵ M=10⁻¹⁴
[tex]\Rightarrow [H_3O^+]=\frac{10^{-14}}{5.5\times 10^{-5}}[/tex]
⇒[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 [tex]H_3O[/tex] is 1.8×10⁻¹⁰ M and it is basic in nature.
