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. Step 1. Complete the ICE Table below: Dissociation Equation H+ (aq) A-(aq) INITIAL 0 Concentration CHANGE +X EQUILIBRIUM Concentration [HA] = [H+] = [A-] = Step 2. Write the equilibrium expression for the acid dissociation constant, Ka. K₂ = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the [H+]. Show the complete solution. Answer: Step 5. Calculate pH of the solution. Show the complete solution. Answer: HA(aq) 0.500 -X 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. Step 1. Complete the ICE Table below: Dissociation Equation H+ (aq) A-(aq) INITIAL 0 Concentration CHANGE +X EQUILIBRIUM Concentration [HA] = [H+] = [A-] = Step 2. Write the equilibrium expression for the acid dissociation constant, Ka. K₂ = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the [H+]. Show the complete solution. Answer: Step 5. Calculate pH of the solution. Show the complete solution. Answer: HA(aq) 0.500 -X 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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