one chem question, need help :) thank you

Chemistry
Tutor: None Selected Time limit: 1 Day

Apr 29th, 2015

This is a buffer problem. 

ICE table should be used 

Ka = 2.0 x 10^-9 = [H+][OBr-] / [HOBr] 

0.50 mol in 1.00 L = 0.50 M HOBr 
0.30 mol in 1.00 L = 0.30 M KOBr (or OBr-) 

HOBr + H2O <-> H3O+ + OBr- 
0.50                       0           0.30 
-x +x +x 
(0.50-x)   x   (0.30+x) 

Assume x is small comparing to 0.30 and 0.50 

2.0 x 10^-9 = x (0.30) / 0.50) 

[H3O+] = x = 3.33 x 10^-9 

So : 
pH = 8.48


Good Luck 

Apr 29th, 2015

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