Consider the titration of 25.00mL of 0.200M Methylene (CH3NH2). The titrant is 0.120M HCL. Calculate each of the following. (a) the initial pH of base? (b) the pH of 5.00mL added? (c) the pH at 1/2 the HCl needed to reach equivalence point? (d) the volume of added acid required to reach equilibrium? (e) the pH at equivalence point?
Consider the titration of 25.00mL of 0.200M Methylene (CH3NH2). The titrant is 0.120M HCL. Calculate each of the following. (a) the initial pH of base? (b) the pH of 5.00mL added? (c) the pH at 1/2 the HCl needed to reach equivalence point? (d) the volume of added acid required to reach equilibrium? (e) the pH at equivalence point?
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.123QP: A 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl....
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Consider the titration of 25.00mL of 0.200M Methylene (CH3NH2). The titrant is 0.120M HCL. Calculate each of the following.
(a) the initial pH of base?
(b) the pH of 5.00mL added?
(c) the pH at 1/2 the HCl needed to reach equivalence point?
(d) the volume of added acid required to reach equilibrium?
(e) the pH at equivalence point?
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