EXERCISE 1: Calculate the pH of a 0.50 M HA at 25°C. At 25°C, the acid dissociation constant (K₂) of the monoprotic weak acid, HA, is 7.2 x 10-6. Complete the ICE Table below: + Dissociation Equation HA(aq) H+ (aq) A (aq) INITIAL 0.500 0 Concentration CHANGE -X +X EQUILIBRIUM Concentration (6 pts) [HA] = [H+] = [A-] = Write the equilibrium expression for the acid dissociation constant, K₂, and substitute the mathematical equation containing the variable x into the equilibrium expression. Then calculate the [H+] and pH of the solution. Show your complete solution. 0 +X

EXERCISE 1: Calculate the pH of a 0.50 M HA at 25°C. At 25°C, the acid dissociation constant (K₂) of the monoprotic weak acid, HA, is 7.2 x 10-6. Complete the ICE Table below: + Dissociation Equation HA(aq) H+ (aq) A (aq) INITIAL 0.500 0 Concentration CHANGE -X +X EQUILIBRIUM Concentration (6 pts) [HA] = [H+] = [A-] = Write the equilibrium expression for the acid dissociation constant, K₂, and substitute the mathematical equation containing the variable x into the equilibrium expression. Then calculate the [H+] and pH of the solution. Show your complete solution. 0 +X

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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Practice chemistry question
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