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A monoprotic weak acid, HA (K, = 1.78 × 104), was titrated against NaOH. A 50.00-mL of 0.04870 M HA sample was titrated with 0.1000 M KOH. How much volume (mL) of titrant (NaOH) is needed to reach the equivalence point? а. Establish the stoichiometric ratio. Calculate the volume using the titration values and stoich ratio. b. What is the pH of the solution at the end/equivalence point? Create a hypothetical ICE table for the neutralization reaction. Use the Ka value to solve for the pOH/pH. Some conversion and equilibrium relationship may be necessary or needed. С. What indicator should be used for this titration analysis? And what color change may be observable? And why did you choose this indicator? You may use the table or chart from the modules or slide.

A monoprotic weak acid, HA (K, = 1.78 × 104), was titrated against NaOH. A 50.00-mL of 0.04870 M HA sample was titrated with 0.1000 M KOH. How much volume (mL) of titrant (NaOH) is needed to reach the equivalence point? а. Establish the stoichiometric ratio. Calculate the volume using the titration values and stoich ratio. b. What is the pH of the solution at the end/equivalence point? Create a hypothetical ICE table for the neutralization reaction. Use the Ka value to solve for the pOH/pH. Some conversion and equilibrium relationship may be necessary or needed. С. What indicator should be used for this titration analysis? And what color change may be observable? And why did you choose this indicator? You may use the table or chart from the modules or slide.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 47QAP: A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume...
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A monoprotic weak acid, HA (K, = 1.78 × 104), was titrated against NaOH. A 50.00-mL of 0.04870 M HA sample was titrated with 0.1000 M KOH. How much volume (mL) of titrant (NaOH) is needed to reach the equivalence point? а. Establish the stoichiometric ratio. Calculate the volume using the titration values and stoich ratio. b. What is the pH of the solution at the end/equivalence point? Create a hypothetical ICE table for the neutralization reaction. Use the Ka value to solve for the pOH/pH. Some conversion and equilibrium relationship may be necessary or needed. С. What indicator should be used for this titration analysis? And what color change may be observable? And why did you choose this indicator? You may use the table or chart from the modules or slide.
Transcribed Image Text:A monoprotic weak acid, HA (K, = 1.78 × 104), was titrated against NaOH. A 50.00-mL of 0.04870 M HA sample was titrated with 0.1000 M KOH. How much volume (mL) of titrant (NaOH) is needed to reach the equivalence point? а. Establish the stoichiometric ratio. Calculate the volume using the titration values and stoich ratio. b. What is the pH of the solution at the end/equivalence point? Create a hypothetical ICE table for the neutralization reaction. Use the Ka value to solve for the pOH/pH. Some conversion and equilibrium relationship may be necessary or needed. С. What indicator should be used for this titration analysis? And what color change may be observable? And why did you choose this indicator? You may use the table or chart from the modules or slide.
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