?A 0.100 M solution of bromoacetic acid \(\left(\mathrm{BrCH}_{2} \mathrm{COOH}\right)\)
Chapter 16, Problem 16.54(choose chapter or problem)
A 0.100 M solution of bromoacetic acid \(\left(\mathrm{BrCH}_{2} \mathrm{COOH}\right)\) is 13.2 % ionized. Calculate \(\left[\mathrm{H}^{+}\right],\left[\mathrm{BrCH}_{2} \mathrm{COO}^{-}\right],\left[\mathrm{BrCH}_{2} \mathrm{COOH}\right]\) and \(K_{a}\) for bromoacetic acid.
Text Transcription:
(BrCH2COOH)
[H+], [BrCH2COO-], [BrCH2COOH]
K_a
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