Jason and his friends wish to determine iron content in an industrial sludge sample. They havedecided to carry out redox titration experiment. Given half reactions involved in this case asfollow.Fe+ + e- Fe2+E° = 0.77 VCet + e→ Ce+E° = 1.70 Va) Construct a balanced chemical reaction for this case.b) Assess the E° for this reaction.c) Indicate whether there is a pH indicator that could be used to determine the endpoint of thistitration. If yes, name the indicator that they would use.

Answered: Image /qna-images/answer/34f1852c-d811-4816-83d5-131b66047980.jpg

Jason and his friends wish to determine iron content in an industrial sludge sample. They have decided to carry out redox titration experiment. Given half reactions involved in this case as follow. Fe+ + e- Fe2+ E° = 0.77 V Ce* + e→ Ce+ E° = 1.70 V a) Construct a balanced chemical reaction for this case. b) Assess the E° for this reaction. c) Indicate whether there is a pH indicator that could be used to determine the endpoint of this titration. If yes, name the indicator that they would use.

Jason and his friends wish to determine iron content in an industrial sludge sample. They have decided to carry out redox titration experiment. Given half reactions involved in this case as follow. Fe+ + e- Fe2+ E° = 0.77 V Ce* + e→ Ce+ E° = 1.70 V a) Construct a balanced chemical reaction for this case. b) Assess the E° for this reaction. c) Indicate whether there is a pH indicator that could be used to determine the endpoint of this titration. If yes, name the indicator that they would use.

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...

See similar textbooks

Similar questions

[References] a. Will dichromate ions oxidize chloride ions to free chlorine in acidic solution? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E (V) Cr 0,2 + 14H+ +6e 2Cr* + 7H2O +1.33 Cl2+2e 2C1 +1.36 O yes Ono b. Will Fe+ oxidize'Sn+ to Sn**? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction € (V) Fe* +e+ Fe²* +0.77 Sn +2e Sn²* +0.15 O yes Ono
2. You are given an electrochemical cell where the chemical reaction involves a silver complex, and a silver metal bar is provided as the positive electrode. The electrochemical potential for this cell is given by a. b. E=Eº 1 [Ag] -0.0592 (volts).log- Ag /Ag For a test solution with a silver concentration of 0.001 M, the electrochemical cell potential is 0.20 volts. Find the silver electrode potential EºAg-Ag. The same cell from (a) will be used to measure the electrochemical potential for a new silver complex in equilibrium. If the measured cell potential is 0.324 volts, what is the silver concentration for this new silver complex at a chemical equilibrium state?
Calculate the EMF. Note: Answer in 2 decimal places.
+ Complete and balance the following half-reaction in basic solution. Be sure to include the proper phases for all species within the reaction. Reset 2 Question 3 of 37 03 02 0 3 02 03 04 05 H₂O* OH™ - SO3² (aq) → SO4² (aq) 4 ( ) 1 O 5 02 03+04+ 6 7 8 06 07 0 H* H 9 Do t (s) (1) (g) (aq) S H₂O • H₂O Delete Submit
Can someone please help with question 11
Topics: Cells and equilibrium; Competing equilibrium in cells Use general chemistry rules for significant figures. 2. Ecell for the cell below is 0.150 V. [H+] in the anode is unknown but kept constant by a buffer consisting of 0.10 F HA and 0.10 F A– . (These components are not shown in the cell notation but are present in the anode nonetheless.) Pt(s) | H+ (? M) | H2(g) (1.00 atm) || H+ (1.00 M) | H2(g) (1.00 atm) | Pt(s) Find the pH of the buffer and Ka for the monoprotic weak acid HA.
Which redox reaction is the correct reaction for the electrolysis of potassium iodide solution with phenolphthalein pink and starch indicators? 21+ H₂ + 2 OH-→ O₂ + 4H+ + 2 Zn 2 Zn²+ + 2 H₂O → O₂ + 4 H+ + 2 Zn OH- + H₂ + 12 → 21- + 2H₂O 21+ 2 H₂O → 12 + 2 OH- + H₂
9.)
Balance the following reaction in acidic solution. Fill in the coefficients for the balanced overall equation. H+ + Hg + 2+ PbO₂ + Hg →→→ Hg₂+ + Pb²+ -- V PbO₂ 2 2+ H8₂ + Pb²+ + H₂O
4. Name EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Electrodes Use the table of standard reduction potentials from your textbook to complete the following table. The zinc-copper Daniell cell is given as an example. Cu Cu Zn Zn Zn Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ 0.1 M Cu²+ Date 1.0 M Zn²+ Zn²+ + 2e-Zn (ag) Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) 1.0 M Cu²+ Cu²+ +2e-Cu Cathode B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ Anode + 2e → Zn Instructor Cu²+2e-Cu Zn²+ + 2e → Zn (aq) Report Sheet Cathode or Anode? Anode E E (table) (calcd) -0.76 V +0.34 V -0.76V Cathode 0.34 v anode 0.76v Cathode 0.34 v Cu²+ + 2e - Cul C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Zn(aq) +2e Zn (s) cathode -0.76 1.0 M Mg²+Mga+2e Mg(s) anode -2.38 +1.10 V 1.10 V 1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v 2+ +2e 1.0 M Mg²+ M Mg(s) anode -2.38v "You must use the Nernst equation to calculate this…
Considered the unbalanced equation of bromate reacting with iron ions. BrO3 + Fe+ Br +Fe+ Identify the true statements necessary in the process of balancing the equation in acidic solution. Select one or more: O 6H+ need to be added to the reduction half-reaction. The oxidation half-reaction needs to be multiplied by 3. 3H,0 need to be added to the reduction half-reaction. 3H,O need to be added to the oxidation half-reaction. The oxidation half-reaction needs to be multiplied by 6. 6OH need to be added to the oxidation half-reaction. K BACK Question 5 of 9
In which of the following processes would the entropy of the system increase? A liquid forming from a gas. A solid forming from a gas. The number of gas molecules increasing during a chemical reaction. A solid precipitating from a solution.