6.f. Consider the following coupled redox reaction.O₂ + 2NADH + 2H* = 2H₂O + 2NAD+Calculate AG" (at 310 K) if the standard reduction potentials for O2 andNAD+ are 0.815V and -0.315V respectively.g. If you wanted to shift the above reaction in f. to the left, how would youadjust the pH? Explain briefly.Lab-related questions.a. In lab, you made a 5 M NaCl stock solution. How would you make a 10-mL 0.5 M NaCl solution from your stock solution?i.9 mL 5 M NaCl and 1 mL waterii.5 mL 5 M NaCl and 5 mL wateriii.1 mL 5 M NaCl and 9 mL wateriv.0.1 mL 5 M NaCl and 9.9 mL waterb. In the first week of lab, you made a pH 7.4 phosphate buffer by mixingsome H₂PO4 with HPO4². The pK₂ of H₂PO4 is 7.2. Which of the followingis true?i.ii.iii.iv.7More H₂PO4* needs to be added because the pH > pKaMore HPO4²- needs to be added because the pH > pKaMore H₂PO4 needs to be added because more acid is needed tomaintain a pH of 7.4.More HPO4²- needs to be added because it is more stable.

Answered: Image /qna-images/answer/dd2f2f90-6ac6-45f6-9662-6c184e3e9b04.jpg

f. Consider the following coupled redox reaction. O2 + 2NADH + 2H* = 2H₂O + 2NAD+ Calculate AG" (at 310 K) if the standard reduction potentials for O2 and NAD+ are 0.815V and -0.315V respectively. g. If you wanted to shift the above reaction in f. to the left, how would you adjust the pH? Explain briefly.

f. Consider the following coupled redox reaction. O2 + 2NADH + 2H* = 2H₂O + 2NAD+ Calculate AG" (at 310 K) if the standard reduction potentials for O2 and NAD+ are 0.815V and -0.315V respectively. g. If you wanted to shift the above reaction in f. to the left, how would you adjust the pH? Explain briefly.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 147CP: The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a...

See similar textbooks

Similar questions

What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25 00C is given by the equation where contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that = 0.250 V and that a. What is the uncertainty in the values of pH and [H+] if the uncertainty in the measured potential is 1 m V ( 0.001 V)? b. To what precision must the potential be measured for the uncertainty in pH to be 0.02 pH unit?
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
In some old European churches, the stained-glass windowshave so darkened from corrosion and age that hardly anylight comes through. Microprobe analysis showed that tinycracks anddefects on the glass surface were enriched ininsoluble Mn(III) and Mn(IV) compounds. From AppendixE, suggest a reducing agent and conditions that might successfullyconvert thesecompounds to soluble Mn(II) withoutsimultaneously reducing Fe(III) (which gives the glassits colors) to Fe(II). Take MnO2 as representative of theinsoluble Mn(III) and Mn(IV) compounds.
In biological systems, acetate ion is converted to ethyl alcohol in a two-step process: CH3COO(aq)+3H+(aq)+2eCH3CHO(aq)+H2OE=0.581V CH3CHO(aq)+2H+(aq)+2eC2H5OH(aq)E=0.197V (E°' is the standard reduction voltage at 25°C and pH of 7.00.) (a) Calculate G°' for each step and for the overall conversion. (b) Calculate E°' for the overall conversion.
Calculate E° for the following cells: (a) Ag|Ag+Sn4+,Sn2+|Pt (b) Al|Al3+Cu2+|Cu (c) Pt|Fe2+,Fe3+MnO4,Mn2+|Pt
Consider a cell in which the reaction is 2Ag(s)+Cu2+(aq)2Ag+(aq)+Cu(s) (a) Calculate E° for this cell. (b) Chloride ions are added to the Ag|Ag+ half-cell to precipitate AgCl. The measured voltage is +0.060 V. Taking [Cu2+]=1.0M, calculate [Ag+]. (c) Taking [Cl-] in (b) to be 0.10 M, calculate Kspof AgCl.