Math  /  Algebra

Question1. The pH of a 6.81×102M6.81 \times 10^{-2} \mathrm{M} solution of a weak monoprotic acid is 5.28 . Calculate the percent dissociation of the acid to 3 significant figures. \% Submit Answer Tries 0/99

Studdy Solution
Calculate the percent dissociation of the acid.
Percent dissociation is given by the formula: Percent Dissociation=([H+][Acid]0)×100% \text{Percent Dissociation} = \left( \frac{[\mathrm{H}^+]}{[\text{Acid}]_0} \right) \times 100\%
Substitute the values: Percent Dissociation=(5.25×1066.81×102)×100% \text{Percent Dissociation} = \left( \frac{5.25 \times 10^{-6}}{6.81 \times 10^{-2}} \right) \times 100\%
Calculate the percent dissociation: Percent Dissociation0.00771% \text{Percent Dissociation} \approx 0.00771\%
Round to 3 significant figures: Percent Dissociation0.00771% \text{Percent Dissociation} \approx 0.00771\%

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