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18 January, 12:23

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?

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  1. 18 January, 12:29
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    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.
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