Calculate the [H3O+] of a 1.99 M HBrO solution at 25 ºC.
HBrO + H2O <=> H3O+ + BrO-
initial I 1.99 M------------------ 0 ------ 0
change C -x ------------------ +x ------ +x
equilibrium E 1.99-x ------------------ +x ------- +x Ka for HBrO at 25 oC = 2.8 x 10-9
Ka = [H3O+][BrO-]/ [HBrO] = ( x)(x )/ (1.99-x) = 2.8 x
10-9
Ka is very small hence (1.99-x) term becomes 1.99
( x)(x )/ (1.99) = 2.8 x 10-9 solving for x gives
x = 7.4645 X 10-5
Hence [H3O+] = 7.4645 X 10-5
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