40.0 mL of 0.12 M weak monoprotic acid with a Ka value of 1.0*10^-5 is titrated with 0.12 M NaOH(aq). At which point during the titration will the equilibrium concentrations of H^+ and OH^- be equal? after the addition of exactly 20.0 mL of NaOH(aq) after the addition of slightly less than 40.0 mL of NaOH(aq) after the addition of exactly 40.0 mL of NaOH(aq) after the addition of more than 40.0 mL of NaOH(aq) The equilibrium concentrations of H+ and OH- are always equal. The equilibrium concentrations of H+ and OH- are never equal.
40.0 mL of 0.12 M weak monoprotic acid with a Ka value of 1.0*10^-5 is titrated with 0.12 M NaOH(aq). At which point during the titration will the equilibrium concentrations of H^+ and OH^- be equal? after the addition of exactly 20.0 mL of NaOH(aq) after the addition of slightly less than 40.0 mL of NaOH(aq) after the addition of exactly 40.0 mL of NaOH(aq) after the addition of more than 40.0 mL of NaOH(aq) The equilibrium concentrations of H+ and OH- are always equal. The equilibrium concentrations of H+ and OH- are never equal.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...
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Transcribed Image Text:40.0 mL of 0.12 M weak monoprotic acid with a Ka value of 1.0*10^-5 is
titrated with 0.12 M NaOH(aq). At which point during the titration will the
equilibrium concentrations of H^+ and OH^- be equal?
after the addition of exactly 20.0 mL of NaOH(aq)
after the addition of slightly less than 40.0 mL of NaOH(aq)
after the addition of exactly 40.0 mL of NaOH(aq)
after the addition of more than 40.0 mL of NaOH(aq)
The equilibrium concentrations of H+ and OH- are always equal.
The equilibrium concentrations of H+ and OH- are never equal.
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