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…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.21QAP

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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?
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
Calculate the pH during the titration of 20.00 mL of0.1 M NaOH with 0.100 M HCl after theaddition of the following volumes of reagent:a. 0.00 mLb. 10.00 mLc. 15.00 mLd. 20.00 mLe. 24.5 mLf. 25.00 mLg. 30 mLh. 35 mL
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Determination of K, TRIAL Volume NaOH at pH at Midpoint of Titration Midpoint of Titration 1. 3.22 3. Average K Identity of Unknown Acid
0.8 0.7 0.6 0.5- 0.4- 0.3- 0.2 0.1 0 5 6 C. (ii) only D. (i) and (ii) 7 8 pH 9 Free Bound 10 11 ii. The free indicator is a stronger acid than the bound indicator. A. (i) only B. Neither (i) nor (ii) 0.8 0.7 0.6 0.5 -0.4 -0.3 0.2 0.1 A scientist measured the absorbance of a pH indicator dye when it was free or bound to a small peptide at their respective maximum absorbance wavelengths. Which of the following options is CORRECT? i. The pka of the indicator increased upon peptide binding. 0
A 24.0 mL sample of 0.115 M sulfurous acid (H,S03) is titrated with 0.1019 M KOH At what added volume of base solution does the first equivalence point occur? Express your answer in mililiters to three significant figures. V. mL Submit Request Answer Vorue nertlel

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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.