The half-equivalence point of a titration occurs half way to the end point, wher

Question

The half-equivalence point of a titration occurs half way to the end point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted.
If 0.300 moles of a monoprotic weak acid (Ka = 1.5 × 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?

thanks

saping leaming Map The half-equivalence point of a titration occurs half way to the end point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted lf 0.300 moles af a monoprotic weak acid (K-1.5 x 10e)0trated with NaOH, what is the pH of the solution at the half-equivalence point? Number Ole

Explanation / Answer

by definition, the H in the half equivalence point is given by pKa

since

pH = pKa + log(conjugate/acid)

and

(conjugate/acid) = 1

so

log(1) = 0

pKa = -logKa = -log(1.5*10^-6) = 5.82390

pH = 5.82390

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