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Calculate the pH of a mixture that contains 0.12 M of HBr and 0.27 M of...

Calculate the pH of a mixture that contains 0.12 M of HBr and 0.27 M of HBrO.

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Answer #1

[H+] from HOBr = 2.65*10^-5 M

[H+] from HBr = 0.12 M (since HBr is strong acid so [HBr] = [H+]

total [H+] = 0.12 +  2.65*10^-5 = 0.1200 M

so pH = -log [H+] = - log [ 0.1200] = 0.921

pH = 0.92

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