Consider the titration of 30.0 mL of0.275 M weak base B (Kb = 1.3 x10-10) with 0.150 M HI.What is the pH of the solutionbefore any acid has been added? Consider the titration of 30.0 mL of0.275 M weak base B (Kb = 1.3 x10-10) with 0.150 M HI.What would be the pH of thesolution after the addition of 20.0mL of HI?

Answered: Consider the titration of 30.0 mL of…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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 would be the pH of the
solution after the addition of 20.0
mL of HI?

Expert Solution

Step 1

It is given that concentration of weak base is equal to 0.275 M and base constant is equal to $1.3 \times 10^{- 10}$ . 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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