The ph of a 0.55 m aqueous solution of hypobromous acid, hbro, at 25.0°c is 4.48. what is the value of ka for hbro?

The solution would be like this for this specific problem:

Given:

pH of a 0.55 M hypobromous acid (HBrO) at 25.0 °C = 4.48

[H+] = 10^-4.48 = 3.31 x 10^-5 M = [BrO-]

Ka = (3.31 x 10^-5) ^2 / 0.55 = 2 x 10^-9

To add, Hypobromous Acid does not require acid adjustment, which is necessary for chlorine-based product and is stable and effective in pH ranges of 5-9.

Hypobromous Acid combines with organic compounds to form a bromamine. Chlorine also combines with the same organic compounds to form a chloramine. It is also one of the least expensive intervention antimicrobial compounds available.