Q4. A 5.00 mL aqueous sample containing hydrogen peroxide was diluted to 25 mL and analyzed by titration with permanganate in acidic pH: GER Mn04 + H202 → 02 + Mn2+ The sample required 84.2 mL of 0.0175 M permanganate to reach the endpoint. concentration of hydrogen peroxide in the original sample? NOT COPY NERSITY is the

Q4. A 5.00 mL aqueous sample containing hydrogen peroxide was diluted to 25 mL and analyzed by titration with permanganate in acidic pH: GER Mn04 + H202 → 02 + Mn2+ The sample required 84.2 mL of 0.0175 M permanganate to reach the endpoint. concentration of hydrogen peroxide in the original sample? NOT COPY NERSITY is the

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.39QAP

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Similar questions

Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M NH3 (Kb = 1.8 105) with 0.100 M HCl.
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
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.
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?
Consider die titration of 50.0 mL of 0.10 M H3A (Ka1 = 5.0 104, Ka2 = 1.0 108, Ka3 = 1.0 1012) titrated by 0.10 M KOH. a. Calculate the pH of the resulting solution at 125 mL of KOH added. b. At what volume of KOH added does pH = 3.30? c. At 75.0 mL of KOH added, is the solution acidic or basic?