NH3 + H3O+ →>> NH; + H2O 25.0 mL of the 0.0220 M NH3 was titrated with 0.010 M HBr. It took 55.0 mL of HBr to reach the equivalence point. Determine the pH of the solution when 75.0 mL of 0.010 M HBr are added. Assume the temperature is constant and the volumes are additive. KbNH3 = 1.85 x 10-5 pH = [?]
NH3 + H3O+ →>> NH; + H2O 25.0 mL of the 0.0220 M NH3 was titrated with 0.010 M HBr. It took 55.0 mL of HBr to reach the equivalence point. Determine the pH of the solution when 75.0 mL of 0.010 M HBr are added. Assume the temperature is constant and the volumes are additive. KbNH3 = 1.85 x 10-5 pH = [?]
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter13: Acids And Bases
Section: Chapter Questions
Problem 29QAP: How many grams of HI should be added to 265 mL of 0.215 M HCI so that the resulting solution has a...
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![NH3 + H3O+ → NH; + H2O
25.0 mL of the 0.0220 M NH3 was titrated
with 0.010 M HBr. It took 55.0 mL of HBr to
reach the equivalence point.
Determine the pH of the solution when
75.0 mL of 0.010 M HBr are added.
Assume the temperature is constant and
the volumes are additive.
K₂NH₂ = 1.85 x 10-5
pH = [?]
pH
Enter](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F545f6ba6-055a-4a28-8022-7d417ad2ec4b%2F08cbcd7b-c589-4891-9b24-871a50165a42%2Fosh3g9p_processed.jpeg&w=3840&q=75)
Transcribed Image Text:NH3 + H3O+ → NH; + H2O
25.0 mL of the 0.0220 M NH3 was titrated
with 0.010 M HBr. It took 55.0 mL of HBr to
reach the equivalence point.
Determine the pH of the solution when
75.0 mL of 0.010 M HBr are added.
Assume the temperature is constant and
the volumes are additive.
K₂NH₂ = 1.85 x 10-5
pH = [?]
pH
Enter
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