*6. (a) In performing a titration, why is it better to use a solution of a concentration such that 30-45 mL is required, instead of a more concentrated solution that might only require about 5 mL to reach the end point? (b) To make a standardized NaOH solution, why is it better to prepare a NaOH solution of approxi- mate concentration and then standardize with KHP, rather than to weigh accurately some NaOH pellets, dissolve them, and dilute the solution in a volumetric flask? (c) În analVzing a 0.003 weak acid by titration with 0.00300 M NaOH, why would you be able to

*6. (a) In performing a titration, why is it better to use a solution of a concentration such that 30-45 mL is required, instead of a more concentrated solution that might only require about 5 mL to reach the end point? (b) To make a standardized NaOH solution, why is it better to prepare a NaOH solution of approxi- mate concentration and then standardize with KHP, rather than to weigh accurately some NaOH pellets, dissolve them, and dilute the solution in a volumetric flask? (c) În analVzing a 0.003 weak acid by titration with 0.00300 M NaOH, why would you be able to

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 7RQ: Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations...

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Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
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.
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.
What volume of 0.4 M Ba (OH)2 must be added to 50 mL of 0.3 M NaOH to give a solution 0.5 M in OH-.
Please Follow this Properly, I Like your answer Structure, Accuracy, Concept, Please No submit Handwriting.
1. A student failed to carry out all of the procedural steps when doing the experiment. Would the following procedural variations result in an experimentally determined molarity of NaOH that is too high or too low? Briefly Explain. (a) The student didnt clean the buret before the beginning the titration. After completeing the titration, the student noticed that droplets of the titrant were clinging to the inside surface of the barel. (b) The buret tip was not completely filled with NaOH solution when the titration was begun. (c) The student forgot to add phenolphthalein indicator solution to the KHP solution before doing the titration
A 92.0 mL sample of 0.0400 M HBr is titrated with 0.0800 M NaOH solution. Calculate the pH after the following volumes of base have been added. (a) 23.0 mLpH = (b) 45.5 mLpH = (c) 46.0 mLpH = (d) 47.8 mLpH = (e) 81.9 mL
What is impoantant about mass percent in chemistry? What does it do in the context of a acid-base titration?
Part (c) and (d) only
A 71.0 mL sample of 0.0100 M HClO4 is titrated with 0.0200 M NaOH solution. Calculate the pH after the following volumes of base have been added. (a) 13.8 mLpH = (b) 35.1 mLpH = (c) 35.5 mLpH = (d) 36.6 mLpH = (e) 61.4 mL