ibiscms/modnoisvew.piduu Jump to... Map Sapling Learning The half-equivalence po

Question

ibiscms/modnoisvew.piduu Jump to... Map Sapling Learning 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. 2.1 x10) is titrated with NaOH, what is the pH of the If 0.500 moles of a monoprotic weak acid (K solution at the half-equivalence point? Number Previous Give Up& View SolutionCheck Answer Next Ex Hint about us careers privacy policy terms of use contact us help 9

Explanation / Answer

Ka = 2.1*10^-5

pKa = - log (Ka)
= - log(2.1*10^-5)
= 4.678

At half equivalence point, half of acid has converted to form conjugate base and half of the acid remains

So, at half equivalence point,
[acid] = [conjugate base]

they form buffer

use:
pH = pKa + log ([Conjugate base]/[acid])
= 4.678+ log {1}
= 4.678

Answer: 4.68

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