Respuesta :

maacastrobr

Answer:

[H⁺] = 3.23x10⁻³ M

Explanation:

For a weak monoprotic acid, such as acrylic acid, we can calculate [H⁺] using the following formula if the solution concentration is significantly higher than the Ka:

  • [H⁺] = √(C * Ka)

Where C is the weak acid concentration.

We input the data:

  • [H⁺] = [tex]\sqrt{0.330 M * 3.16x10^{-5}}[/tex]

And solve for [H⁺]:

  • [H⁺] = 3.23x10⁻³ M