Respuesta :

maacastrobr

Answer:

Ka = 3.45x10⁻⁶

Explanation:

First we calculate [H⁺], using the given pH:

  • pH = -log[H⁺]
  • [H⁺] = [tex]10^{-pH}=10^{-5.6}[/tex]
  • [H⁺] = 2.51x10⁻⁶ M

To solve this problem we can use the following formula describing a monoprotic weak acid:

  • [H⁺] = [tex]\sqrt{C*Ka}[/tex]

We input the data that we already know:

  • 2.51x10⁻⁶ = [tex]\sqrt{0.530*Ka}[/tex]

And solve for Ka:

  • Ka = 3.45x10⁻⁶

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