Case 3: pH with known K: The dissociation of ammonia (NH3) in water is shown below: NH3 (aq) + H2O (m = NH4*(aq) + OH-(aq) At 25°C, Kb, is 1.8 × 10-5 (7) Calculate the pH of a mixture of 0.192 mol NH3 and 0.116 mol NH4C1 diluted to 400.0 mL with distilled water.

Chemistry & Chemical Reactivity
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Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
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Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases
Section: Chapter Questions
Problem 118IL: Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H)...
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Case 3: pH with known K:
The dissociation of ammonia (NH3) in water is shown below:
NH3 (aq) + H2O (m = NH4*(aq) + OH-(aq)
At 25°C, Kb, is 1.8 × 10-5
(7) Calculate the pH of a mixture of 0.192 mol NH3 and 0.116 mol NH4C1 diluted to 400.0 mL with
distilled water.
Transcribed Image Text:Case 3: pH with known K: The dissociation of ammonia (NH3) in water is shown below: NH3 (aq) + H2O (m = NH4*(aq) + OH-(aq) At 25°C, Kb, is 1.8 × 10-5 (7) Calculate the pH of a mixture of 0.192 mol NH3 and 0.116 mol NH4C1 diluted to 400.0 mL with distilled water.
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