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

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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
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.

NH,Br(aq) → NH (aq)+Br (aq)
NH; (aq) + H,0() ENH; (aq)+Н,О "aq)
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-.

Then the ICE table is:
NH,
НО
NH3
НО-
I (M)
C (M)
E (M)
0.3
0.3-x
+x
+x
0.3-x
х
х
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