For a solution of 0.020 M lactic acid, HC₃H₅O₂ (Kₐ = 8.4 × 10⁻⁴), calculate:(a) [H⁺] [Information box] ___________ M(b) pH [Information box] ___________(c) percent ionization [Information box] ___________ %

Answered: For a solution of 0.020 M lactic acid,…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

For a solution of 0.020 M lactic acid, HC₃H₅O₂ (Kₐ = 8.4 × 10⁻⁴), calculate:

(a) [H⁺]

[Information box] ___________ M

(b) pH

[Information box] ___________

(c) percent ionization

[Information box] ___________ %

Expert Solution

Step 1

Given that: Concentration of lactic acid = 0.020 M and K_a = 8.4×10^-4

To find:

Concentration of H⁺ ions
pH of the solution
Percent ionization

Step 2

Lactic acid is a weak acid. The dissociation of this weak acid in water is as given by the reaction shown below.

${HC}_{3} H_{5} O_{3} (aq) \to C_{3} H_{5} O_{3}^{-} (aq) + H^{+} (aq)$

Step 3

Let x amount of lactic acid dissociate at equilibrium, the ICE table for the reaction is given by,

$\begin{matrix} {HC}_{3} H_{5} O_{3} & \to & C_{3} H_{5} O_{3}^{-} & + & H^{+} \\ I & 0.020 & 0 & 0 \\ C & - x & + x & + x \\ E & 0.020 - x & x & x \end{matrix}$

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