For 480.0 mL of a buffer solution that is 0.160 M in CH3CH2NH2 and 9.00×10−2 M in CH3CH2NH3Cl , calculate the initial pH and the final pH after adding 1.5×10−2 mol of HCl . ( Kb(CH3CH2NH2)=5.6×10−4 .)
For 480.0 mL of a buffer solution that is 0.160 M in CH3CH2NH2 and 9.00×10−2 M in CH3CH2NH3Cl , calculate the initial pH and the final pH after adding 1.5×10−2 mol of HCl . ( Kb(CH3CH2NH2)=5.6×10−4 .)
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section17.2: Controlling Ph: Buffer Solutions
Problem 1RC: 1. Which choice would be a good buffer solution?
0.20 M KCH3CO2 and 0.20 M CH3CO2H
0.20 M HCl and...
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For 480.0 mL of a buffer solution that is 0.160 M in CH3CH2NH2 and 9.00×10−2 M in CH3CH2NH3Cl , calculate the initial pH and the final pH after adding 1.5×10−2 mol of HCl . ( Kb(CH3CH2NH2)=5.6×10−4 .)
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