Part B: Titration of Iron UnknownTrial ITrial IITrial IIIMass of unknown used1.2091.20 g1.20 gInitial buret reading0 mL32.1 mL13.0 mLFinal buret reading32.1mL13.0 mL43.5mLVolume of KMnO4 used32.1 mL30.9mL30.5 mL17.9+13.0 Determine the % Fe in each sample and the average % Fe.

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Answered: Part B: Titration of Iron Unknown Trial…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter11: Dynamic Electrochemistry

Section: Chapter Questions

Problem 9P

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Consider a 10.0% (by mass) solution of hypochlorous acid. Assume the density of the solution to be 1.00 g/mL. A 30.0-mL sample of the solution is titrated with 0.419 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.
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?
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.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink in the base form (pH 10.0). It is a weak acid with a pKa of 8.7. What fraction is in the acid form when the acid color is apparent? What fraction is in the base form when the base color is apparent?
BURETTE READING SAMPLE Pp Mo A 12.4 25.0 6.2 6.2 9.2 16.8 D. 0.0 5.3 Use the table below to identify the basic compound C: *Note that double indicator titration for each compound was done using a standard acid solution with 0.0 mL as initial reading. O NaHCO3 O NaOHANazCO3 O NaOHANaHCO3 O Nazco3
10. How many mililiters of 0.085 M NaOH are required to titrate the following solution to the equivalence point: 40.0 mL of 0.0900M HNO3 Group of answer choices A) 42.4 mL NaOH soln B) 23.6 mL C.) 37.8 mL D.) 40.0 mL
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Titration of the I2 produced from .1045g of primary standard KIO3 required 30.72ml of sodium thiosulfateCalculate the concentration of the Na2S2O3
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Part B: Titration of Iron Unknown Trial I Trial II Trial III Mass of unknown used 1.209 1.20 g 1.20 g Initial buret reading 0 mL 32.1 mL 13.0 mL Final buret reading 32.1mL 13.0 mL 43.5mL Volume of KMnO4 used 32.1 mL 30.9mL 30.5 mL 17.9+13.0 Determine the % Fe in each sample and the average % Fe.