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Calculate the concentration of H3O⁺ in a solution that contains 6.25 × 10-9 M OH⁻ at 25°C. Identify the solution as acidic, basic, or neutral. A) 6.38 × 10-9 M, basic B) 1.60 × 10-6 M, acidic C) 7.94 × 10-11 M, acidic D) 7.38 × 10-3 M, basic E) 4.92× 10-5 M, acidic

Respuesta :

Answer: B) [tex]1.60\times 10^{-6}[/tex] M, acidic

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration and pOH is calculated by taking negative logarithm of hydroxide ion concentration.

Acids have pH ranging from 1 to 6.9, bases have pH ranging from 7.1 to 14 and neutral solutions have pH equal to 7.

[tex]pH=-\log [H_3O^+][/tex]

[tex]pOH=-log{OH^-}[/tex]

[tex]pH+pOH=14[/tex]

Given : [tex][OH^-]=6.25\times 10^{-9}M[/tex]

[tex]pOH=-log[6.25\times 10^{-9}M][/tex]

[tex]pOH=8.20[/tex]

[tex]pH=14-8.20=5.8[/tex]

As pH is less than 7, the solution is acidic.

[tex]5.8=-log[H_3O^+][/tex]

[tex][H_3O^+]=1.60\times [10^{-6}M[/tex]

Thus solution is acidic and concentration of [tex]H_3O^+[/tex] is [tex]1.60\times [10^{-6}M[/tex]

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