EXERCISE 2: Calculate the pH of a 0.50 M NH 3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3) is 1.8 × 10-5. Step 1. Complete the ICE Table below: Hydrolysis Equation NH4+ (aq) NH3(aq) + H₂O(l) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM [NH3] [NH4*] = [OH-] = Step 2. Write the equilibrium expression for the base dissociation constant, K. Кь = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the value of [OH-]. Show the complete solution. SOLUTION Step 5. Calculate pH of the solution. Show the complete solution. Answer: + OH (aq) 0 +X

EXERCISE 2: Calculate the pH of a 0.50 M NH 3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3) is 1.8 × 10-5. Step 1. Complete the ICE Table below: Hydrolysis Equation NH4+ (aq) NH3(aq) + H₂O(l) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM [NH3] [NH4*] = [OH-] = Step 2. Write the equilibrium expression for the base dissociation constant, K. Кь = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the value of [OH-]. Show the complete solution. SOLUTION Step 5. Calculate pH of the solution. Show the complete solution. Answer: + OH (aq) 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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