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A 10.0 mL solution containing an unknown monoprotic acid, HA, ([HA]0 = 0.450 mol/L) was found...

A 10.0 mL solution containing an unknown monoprotic acid, HA, ([HA]0 = 0.450 mol/L) was found to have a percent ionization of 1.18 % at 25.0 ̊C. Determine the value of Ka for this unknown acid.

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Answer #1

- HT + А НА + и At t=0 .45M At equilibrium .45-48.45 xxoU5 XX:45 Rato 18 = .0118 Ka= [ht] [4] [HA] .450 X .45% .45(1-2) 0452²

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