A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 MNaOH solution. The titration curve above was obtained. Which of the followingindicators would be best for this titration?pH ofsolutionin flask12.0110.08.06.04.02.05 10 15 20 25 30 35 40 45mL of 0.115 M NaOH added to flaskmethyl red.O bromthymol blueOthymol blueEquivalencePointOphenolpthaleinO bromocresol purpleIndicatormethyl orangemethyl redbromocresol purplebromthymol bluethymol bluephenolpthaleinpKa3.465.006.127.108.909.10

Given , A sample of monoprotic acid is titrated with NaOH solution .

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. Which of the following indicators would be best for this titration? pH of solution in flask 12.01 10.0 8.0 6.0 4.0 2.0 Equivalence Point 5 10 15 20 25 30 35 40 45 mL of 0.115 M NaOH added to flask methyl red Obromthymol blue Othymol blue Ophenolpthalein Indicator methyl orange methyl red bromocresol purple bromthymol blue thymol blue phenolpthalein pka 3.46 5.00 6.12 7.10 8.90 9.10

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. Which of the following indicators would be best for this titration? pH of solution in flask 12.01 10.0 8.0 6.0 4.0 2.0 Equivalence Point 5 10 15 20 25 30 35 40 45 mL of 0.115 M NaOH added to flask methyl red Obromthymol blue Othymol blue Ophenolpthalein Indicator methyl orange methyl red bromocresol purple bromthymol blue thymol blue phenolpthalein pka 3.46 5.00 6.12 7.10 8.90 9.10

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 34QRT

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Similar questions

When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
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