Given 0.1 M aqueous solutions of ammonium chloride (NH4Cl) and ammonia (NH3) to the solution of that of a weak base. Calculate the volumes of salt and ammonia to be mixed, in order to make 50mL of a buffer solution with pH=9.0. The ammonium ion (NH4+) has a dissociation constant of value, ka=5.62*10^-10.
Given 0.1 M aqueous solutions of ammonium chloride (NH4Cl) and ammonia (NH3) to the solution of that of a weak base. Calculate the volumes of salt and ammonia to be mixed, in order to make 50mL of a buffer solution with pH=9.0. The ammonium ion (NH4+) has a dissociation constant of value, ka=5.62*10^-10.
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
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.3QE:
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify...
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Given 0.1 M aqueous solutions of ammonium chloride (NH4Cl) and ammonia (NH3) to the solution of that of a weak base. Calculate the volumes of salt and ammonia to be mixed, in order to make 50mL of a buffer solution with pH=9.0. The ammonium ion (NH4+) has a dissociation constant of value, ka=5.62*10^-10.
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