Answer
See explanation below.
Work Step by Step
1
(A) Given :
1. pH of the buffer = 7.95
2. Ka of Acid (HBrO) = 2.3 x 10^-9
2
(B) Formulae :
1. Henderson - Hasselbalch equation of a buffer : pH = pKa + log [base] / [acid]
2. pKa = -log(Ka)
3
(C) Solution :
1. pKa = -log (Ka)
= -log (2.3 x 10^-9)
= 8.64 .... (1)
2. pH = pKa + log [base] / [acid]
7.95 = 8.64 + log ([BrO-] / [HBrO])
-0.69 = log ([BrO-] / [HBrO])
[BrO-] / [HBrO] = 10^(-0.69) = 0.20
Hence, the component concentration ratio [BrO-] / [HBrO] is equal to 0.20