1. 10.0 mL of 0.40 M weak acid is being neutralized with 0.10 M NaOH. The results of this titrationis shown below.1412Referring to a chart of indicators andtheir turning points, which indicatorwould you use for this titration?Explain.a.10 -6 -1040Volume of NaOH addod (ml)2030506070b. Using the symbol "HA" to represent the weak acid, use a dissociation equation to explainwhy this acid behaves as a weak acid.In the buffer zone between 20 and 30 ml. of titrant added the pH doesn't change veryC.much. How does Le Chatelier's Principle explain this phenomenon?

a. For the titration of a weak acid with a strong base, the pH at the equivalence point is greater…

1. 10.0 mL of 0.40 M weak acid is being neutralized with 0.10 M NAOH. The results of this titration is shown below. 14 12 a. Referring to a chart of indicators and their turning points, which indicator would you use for this titration? Explain. 10 6 - 4 10 20 40 Volumo of NaOH addod (ml) 30 50 60 70 80 b. Using the symbol "HA" to represent the weak acid, use a dissociation equation to explain why this acid behaves as a weak acid.

1. 10.0 mL of 0.40 M weak acid is being neutralized with 0.10 M NAOH. The results of this titration is shown below. 14 12 a. Referring to a chart of indicators and their turning points, which indicator would you use for this titration? Explain. 10 6 - 4 10 20 40 Volumo of NaOH addod (ml) 30 50 60 70 80 b. Using the symbol "HA" to represent the weak acid, use a dissociation equation to explain why this acid behaves as a weak acid.

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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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.
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