Consider the titration of 30.0 mL of 0.275 M weak base B (Kb = 1.3 x 10-10) with 0.150 M HI. What is the pH of the solution before any acid has been added?
Consider the titration of 30.0 mL of 0.275 M weak base B (Kb = 1.3 x 10-10) with 0.150 M HI. What is the pH of the solution before any acid has been added?
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 16.53QE
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It is given that concentration of weak base is equal to 0.275 M and base constant is equal to . For calculating pH of the solution, first pOH of solution has to be find out. As it is weak acid, it will not dissociates completely and dissociation constant, α comes into account.
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