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Calculate the ph of a 0.10 m solution of hypochlorous acid, hocl. ka of hocl is 3.5×10−8 at 25 ∘c. express your answer numerically using two decimal places.

Respuesta :

superman1987

Answer:

4.23.

Explanation:

∵ pH = - log[H⁺].

For weak acids:

∵ [H⁺] = √(ka)(c).

∴ [H⁺] = √(3.5 × 10⁻⁸)(0.10 M) = 5.92 x 10⁻⁵.

∴ pH = - log[H⁺] = - log(5.92 x 10⁻⁵) = 4.2279 ≅ 4.23.

batolisis

The pH of the 0.10 m solution of hypochlorous acid is :  4.23.

Given data :

Ka of HOCl = 3.5 * 10⁻⁸

Temperature = 25⁰C

Concentration ( c ) = 0.10 m

Determine the pH of the solution

pH = -log [ H⁺ ]   --- ( 1 )

For a weak acids

[ H⁺ ] = [tex]\sqrt{Ka*C}[/tex]

        = [tex]\sqrt{3.5 * 10^{-8} * 0.10}[/tex]  =  5.92 * 10⁻⁵

back to equation ( 1 )

pH of the solution = - log [ 5.92 * 10 ]

                              =  4.2279 ≈ 4.23

Hence we conclude that The pH of the 0.10 m solution of hypochlorous acid is :   4.23.

Learn more about pH of a solution : https://brainly.com/question/22390063

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