Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter14: Acid-base Equilibria
Section: Chapter Questions
Problem 93E: What concentration of NH4NO3 is required to make [OH]=1.0105 in a 0.200-M solution of NH3?
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Question
There are 2 mL of buffer per well. Calculate the final pH of the undiluted buffer after 0.25 mL (5 drops) of 0.1 M NaOH is added. Ka of CH3COOH is 1.8 × 10-5. Use the CH3COOH buffer concentration calculated in Table 2, an ICE table, and a balanced dissociation equilibrium equation to determine the pH.
Please help me with the steps of this question, thanks!
![Concentration of
0.05 M
0.02 M
0.01 M
0.003 M
sodium acetate (M)
PH 4.7
bufter
znd
di lutionn
3rd
dilution
dilution](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F08ba6b13-0037-4514-a799-394b5d4dfa4e%2F4ced8980-0bab-47ed-a447-222da38666f8%2F4ayk4lh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Concentration of
0.05 M
0.02 M
0.01 M
0.003 M
sodium acetate (M)
PH 4.7
bufter
znd
di lutionn
3rd
dilution
dilution
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