Calculate the pH of the solution that results from the mixture of 175.0 mL of 0.10 M C2H5NH2 and 275.0 mL of 0.20 M C2H5NH3Cl. (The Kb of C2H5NH2 = 5.6 x 10-4).
Calculate the pH of the solution that results from the mixture of 175.0 mL of 0.10 M C2H5NH2 and 275.0 mL of 0.20 M C2H5NH3Cl. (The Kb of C2H5NH2 = 5.6 x 10-4).
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter15: Solutions Of Acids And Bases
Section: Chapter Questions
Problem 15.121QE: A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to...
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Calculate the pH of the solution that results from the mixture of 175.0 mL of 0.10 M C2H5NH2 and
275.0 mL of 0.20 M C2H5NH3Cl. (The Kb of C2H5NH2 = 5.6 x 10-4).
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