Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter8: Acids And Bases
Section: Chapter Questions
Problem 8.117P
Related questions
Question

Transcribed Image Text:c. H20 = Lewis Base (donate
10. Calculate the pH of 0.3M solution of NH,Br if Ka of NH4* = 5.6x10-10
%3D
/PH= 11.4l
Expert Solution

Step 1
The pH of a 0.3 M solution of NH4Br is to be calculated if Ka of NH4+ = 5.6×10-10
Step 2
In aqueous solution of NH4Br, it exists as NH4+ and Br- .
NH4+ is the conjugate acid of NH3 (a weak base), thus it will partially ionize in solution to give H3O+ and NH3.

Step 3
Let x M be the amount of NH4+ consumed.
0.3 M of NH4Br gives 0.3 M NH4+ and 0.3 M Br-.

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