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what is the acid dissociation constant of an monoprotic acid if a concentration of 0.3M solution has a pH of 3?

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The acid dissociation constant of a weak monoprotic acid if the concentration of the acid is 0.3M and it has a pH of 3 is 3 × 10⁻⁶.

What is the acid dissociation constant?

The acid dissociation constant (Ka) is the equilibrium constant for an acid dissociation reaction.

Let's consider the acid dissociation of a generic weak acid.

HA(aq) = H⁺(aq) + A⁻(aq)

  • Step 1. Calculate [H⁺].

The pH of the solution is 3.

pH = -log [H⁺]

[H⁺] = antilog -pH = antilog -3 = 1 × 10⁻³ M

  • Step 2. Calculate the acid dissociation constant (Ka).

The concentration of the acid (Ca) is 0.3 M. For a weak monoprotic acid, we can calculate the acid dissociation constant using the following expression.

[H⁺] = √(Ca × Ka)

Ka = [H⁺]² / Ca

Ka = (1 × 10⁻³)² / 0.3 = 3 × 10⁻⁶

The acid dissociation constant of a weak monoprotic acid if the concentration of the acid is 0.3M and it has a pH of 3 is 3 × 10⁻⁶.

Learn more about weak acids here: https://brainly.com/question/15192126

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