Welcome to Westonci.ca, where your questions are met with accurate answers from a community of experts and enthusiasts. Explore thousands of questions and answers from a knowledgeable community of experts ready to help you find solutions. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently.
Sagot :
1.4406 × 10⁻⁶ is the Ka(dissociation constant) for the acid.
The equilibrium constant for the reaction of an acid with water is the acid dissociation constant, where the acid, HA separates into H⁺ and A⁻ ions.
The acid dissociation constant is represented by (Ka).
So let's first imagine that the given monoprotic acid is HA.
HA will dissociate into H⁺ and A⁻ ions.
HA ⇒ H⁺ and A⁻
The formula used for Ka is
Ka = [H⁺] [A⁻] / [HA]
Given
pH = 2.83
[HA] = 1.50 M
From the given pH, we can calculate [H⁺] and [A⁻]
[H⁺] = [A⁻] = 1 × [tex]10^{-2.83}[/tex] = 1.47 × 10⁻³ M
Ka = 1.47 × 10⁻³ × 1.47 × 10⁻³ / 1.50
Ka = 1.4406 × 10⁻⁶
Hence, 1.4406 × 10⁻⁶ is the Ka for the acid.
Learn more about dissociation constant here https://brainly.com/question/3006391
#SPJ4
Your visit means a lot to us. Don't hesitate to return for more reliable answers to any questions you may have. We hope you found what you were looking for. Feel free to revisit us for more answers and updated information. Find reliable answers at Westonci.ca. Visit us again for the latest updates and expert advice.