EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 x 10-5. Step 1. Complete the ICE Table below: Hydrolysis Equation NH3(aq) + H₂O(l) NH, (aq) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM (6 pts) [NH3] = [NH] = [OH] = Step 2. Write the equilibrium expression for the base dissociation constant, Kt Kb = 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 NH3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 x 10-5. Step 1. Complete the ICE Table below: Hydrolysis Equation NH3(aq) + H₂O(l) NH, (aq) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM (6 pts) [NH3] = [NH] = [OH] = Step 2. Write the equilibrium expression for the base dissociation constant, Kt Kb = 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

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter16: Acid-base Equilibria

Section16.6: Buffers

Problem 16.6CC: The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate base,...

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The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate base, A. (Water molecules and spectator ions have been omitted for clarity.) a Which beaker on the right, X or Y, depicts the solution after the addition of two formula units of NaOH? b How many HCl molecules can be added to the original buffer solution before the buffer capacity is exceeded? c Draw a picture of the solution where the buffer capacity has been exceeded by the addition of HCl.
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