-14°C 5) Design: The iron(II) solution is titrated to iron (III) with a standard cerium (IV) ion solution which is reduced to cerium (III). The indicator shows, as the endpoint, a sharp colour change from red to pale blue. Evidence: Titration of 25.0 mL of Fe²+ (aq) with 0.125 mol/L Ce+ (aq). Trial Final burette reading (mL) Initial burette reading (mL) Volume of Ce4+ = 1 15.7 0.6 2 30.7 15.7 3 45.6 30.7 4 40.2 25.3 (Answer: 14.975) Problem: What is the amount concentration of iron (II) ionis in a solution obtained in an iron ore analysis? (Answer: 7.49 x 10¹² M) ENG £ 1 0 + O E 5:42 PM

-14°C 5) Design: The iron(II) solution is titrated to iron (III) with a standard cerium (IV) ion solution which is reduced to cerium (III). The indicator shows, as the endpoint, a sharp colour change from red to pale blue. Evidence: Titration of 25.0 mL of Fe²+ (aq) with 0.125 mol/L Ce+ (aq). Trial Final burette reading (mL) Initial burette reading (mL) Volume of Ce4+ = 1 15.7 0.6 2 30.7 15.7 3 45.6 30.7 4 40.2 25.3 (Answer: 14.975) Problem: What is the amount concentration of iron (II) ionis in a solution obtained in an iron ore analysis? (Answer: 7.49 x 10¹² M) ENG £ 1 0 + O E 5:42 PM

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Given this series of equilibrium reactions. See Image(a) Which way should the reaction to “tend” at high pH? Why?(b) Which way should the reaction to “tend” at low pH? Why? (c) What Fe(III) species would be least soluble?
Can cadmium (II), and mercury (II) be separated quantitatively by precipitation as sulfides from a solution that is 0.15 M cadmium nitrate and 0.10 M in mercuric ions? If possible, what range of sulfide concentration is permissible? Do you expect any interference from the formation of hydroxides of both heavy metals? CdS (144.46); Ksp = 1.0 x 10 ^ -27HgS (232.66); Ksp = 2.0 x 10 ^ -53 HINT: Determine the concentration at which each of the cations start to precipitate out of solution. >Quantitative precipitation means 1/1000 remains in solution.
QUSETION5 (a) You have a solution of 50.0 mL of 0.01 M AGNO , What is the AE after the addition of 50.0mL of 0.05M ligand which forms AgL complex? 3 Given log B = 16.3, and Ag* + e ++ Ag(s) E° = 0.799 V (b) Balance the foflowing reactions: KMNO4 with NaNO2 in acidic medium.
Consider the series of equilibrium reactions below. In which way would you expect the reaction to “tend” at high pH? What about low pH? Why? Circle the Fe(III) species that you’d expect to be least soluble. Fe3+ + OH- <---> FeOH2+ + OH- <---> Fe(OH)2+ + OH- <---->Fe(OH)3(ferrihydrite) + OH- <--->Fe(OH)4-
Hh.88.
1. A 0.7120 g of iron ore was brought into solution and passed through a Jones reductor. Titration of Fe(II) produced required 39.21mL of 0.02086M KMnO4. Express the results of analysis in terms of (a) percent Fe (MM 55.85) and (b) percent Fe₂O3 (MM 159.69). 5Fe +2 + MnO4 +8H+ → 5Fe+³+ Mn+² + 4H₂O
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Develop two methods to quantify Ag+, firstly using acid-base equilibria and then redox equilibria. Specify the reagents used in the method and the concentrations of each (Consider the analite concentration: 0.02M ).
16,17, & 18
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