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# Finding the Acid Dissociation Constant of an Unknown Acid

CHEM-LCAB1B

An weak, monoprotic acid is titrated to the equivalence point with $34.84\text{ mL}$ of $0.112\text{ M }NaOH$.

If the $pH$ of the solution is $4.88$ after $15.31\text{ mL}$ is added, what is the ${K}_{a}$ of the acid?

A

${K}_{a}=1.0\times{10}^{-5}$

B

${K}_{a}=1.3\times{10}^{-4}$

C

${K}_{a}=7.2\times{10}^{-6}$

D

${K}_{a}=4.6\times{10}^{-5}$