Determine the pH during the titration of 71.2 mL of 0.422 M formic acid (Ka = 1.8×10-4) by 0.422 M KOH at the following points. (Assume the titration is done at 25 °C.)(a) Before the addition of any KOH(b) After the addition of 17.0 mL of KOH(c) At the half-equivalence point (the titration midpoint)(d) At the equivalence point(e) After the addition of 107 mL of KOH

Step 1:a) Before addition of any KOH the pH of the solution is due to ionization of weak acid…

Answered: Determine the pH during the titration…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.51QE

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Similar questions

Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
Determine the pH during the titration of 66.5 mL of 0.376 M acetic acid (K, 1.8x105) by 0.376 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 15.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 99.8 mL of KOH
Determine the pH during the titration of 26.8 mL of 0.447 M hypochlorous acid (K, = 3.5x103) by 0.467 M NAOH at the following points. (a) Before the addition of any NaOH 3.90 (b) After the addition of 6.20 mL of NaOH 6.95 (c) At the half-equivalence point (the titration midpoint) 6.90| (d) At the equivalence point (e) After the addition of 38.5 mL of NaOH
Determine the pH during the titration of 26.8 mL of 0.447 M hypochlorous acid (K, = 3.5x108) by 0.467 M NAOH at the following points. (a) Before the addition of any NaOH 3.90 (b) After the addition of 6.20 mL of NaOH 6.95 (c) At the half-equivalence point (the titration midpoint) 6.90 (d) At the equivalence point 10.41 (e) After the addition of 38.5 mL of NaOH 12.96 An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.

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