e) Using the half reaction below sHE Pou3- HPO,2 + 2H* + 2e HPO+H;O E--0,234 V and acid dissociation constants for H3PO4 (K=7.11 × 10°; K2 = 6.32 × 10*, K7.1 x 1014), calculate standard reduction potential for the half reaction he Oy H2POª + H* + 2e HPO + H;O

e) Using the half reaction below sHE Pou3- HPO,2 + 2H* + 2e HPO+H;O E--0,234 V and acid dissociation constants for H3PO4 (K=7.11 × 10°; K2 = 6.32 × 10, K7.1 x 1014), calculate standard reduction potential for the half reaction he Oy H2POª + H + 2e HPO + H;O

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 88E: For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1,...

See similar textbooks

Related questions

Q: Which pairs of species will spontaneously react? Standard Reduction E° (V) Potentials A) Cd and Sn2-…

Q: Q5: Answer with True or False for the following statements (only 7 statements) 1. If the reduction…

A: Following are the appropriate answers (True/Fulse) of the given questions. According to…

Q: C(s) | K2SO4(aq) | Au(s) the following (Note: For this question it is ok to write "AI203" for Al203…

Q: An electro chemi cal cell is set up electrode with co pper CusO4 (ag) and 1.0 mol IL Pb (NO,)z caq)…

A: A numerical problem based on electrochemistry, which is to be accomplished.

Q: A pH meter is calibrated using a pH 4.00 buffer with 174.48 mV, pH 7.00 with 0 mV and pH 10.0 buffer…

A: Given: At 174.48 mV, pH = 4 At 0 mV, pH = 7, At -174.48 mV, pH =10.0 We have to calculate molar…

Q: The selectivity coefficient, Kg+.H*, for a K* ion-selective electrode is 0.00240. When the electrode…

A: For an ion-selective electrode, the potential is given as: E=constant+β0.05916.log[AK++(KK+,H+×AH+)]…

Q: At 25ºC, you conduct a titration of 20.00 mL of a 0.0400 M AgNo3 solution with a 0.050 M NaI soution…

Q: Write the half-reaction and calculate the electrode potential of 1. a zinc electrode in 0.0400 M…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: se standard reduction potentials to calculate the standard free energy change (AG") for the reaction…

A: We have to find∆G

Q: The cell SCE//Ag2CrO4(sat’d), CrO4-2 (x M)/Ag is used for the determination of pCrO4. The half…

A: We can calculate this using Nernst Equation E Ag2CrO4 = EAg2CrO4 - 0.059 /2 (log [CrO4]2-) We know…

Q: At 25C, you conduct a titration of 20.00 mL of a 0.0400 M AgNO3 solution with a 0.050 M NaI solution…

Q: What mass of Ni(s) may be deposited from an aqueous NiCl2 solution if a current of 2.50 A is applied…

A: Reaction occuring Ni+2 (aq) + e- --------> Ni(s)

Q: At 25 C, a titration of 15.00 mL of a 0.0560 M AgNO, solution with a 0.0280 M Nal solution is…

Q: The following standard electrode potentials have been measured at a temperature of 298 K. Ag+ + e− →…

A: In a cell, there are two components, one is an anode and the other is a cathode. The oxidation…

Q: The cell: SCE//HA(0.250M), NaA(0.170M)/H2(1.00bar), Pt has a poten- tial of -0.721V at 298K. (The…

A: Given cell:

Q: hey wanted to produce a cell with an operating potential of 1.05 V and calculated that Q for the…

Q: For the electrochemical cell: Au / Aul(s)//HI(M), H₂ (1atm.) / pt. What are (a) The half cell…

A: Given in following question representative a electrochemical cell Au/AuI(s)// HI(M),H2(1atm)/pt.…

Q: The standard oxidation potential of Ni/Ni2+ electrode is 0.3 V. If this is combined with a hydrogen…

Q: Give a clear explanation handwritten answer..please give answer all sub parts..

Q: [3] Given the Standard Reduction Potentials at 25°C, Mn++2e Mn E° =-1.185V and Hg+2e - Hg E° =…

A: 1- When the standard reduction potential is negative that means it is an oxidation half reaction and…

Q: At 25 °C, a titration of 15.00 mL of a 0.0200 M AGNO, solution with a 0.0100 M NaI solution is…

A: Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Q: A Hg working reactiois WIII occur on the electrode when the electrode potential is scanned from 0.0V…

A: As the electrode potential is scanned from 0 to -0.50V . From 0 to -0.30V the reduction potential of…

Q: The concentration of NO3- in a water sample was determined using ion-selective electrode. A 25.00 mL…

Q: From the following standard reduction potential data: Cu+ + e−-> Cu…

A: Reduction is the process of removal of oxygen or the addition of hydrogen or electron. The potential…

Q: Given the following standard reduction potentials: MnO4 (aq) + 8H*(aq) + 5 e - - Mn2*(aq) + 4 H20()…

A: The expression of Nernst equation is shown below: E =E0cell -0.0591n log Q Where; Ecell= cell…

Q: Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be…

A: The Nernst equation relates the cell potential, standard cell potential, the temperature and…

Q: True or false: The reaction, SO42- + 4H+ +2I- -->H2SO3 + I2 +H2O, will occur spontaneously under…

Q: Use standard reduction potentiais to calculate the equilibrium constant for the reaction: Sn2+(aq) +…

Q: The redox titration we did in lab used 0.010 M Cr2072¯ to titrate 0.060 M and 20 mL Fe2+ The…

A: In redox titrations, addition of titrant alters the concentrations of reduced and oxidised form of…

Q: For Ag+(ag) + e- → Ag(s), Eº = +0.80 V and for Zn²+(aq) + 2e- → Zn(s), Eº = -0.76 V. a) Identify…

A: For a Galvanic cell, cell potential can be calculated using the Nernst equation. Here, the zinc is…

Q: = -0.763 V) immersed in Calculate the potential of a zinc electrode (E+ /Zn a 0.0130 M in 2+ Zn…

A: To calculate the potential of Zn electrode.

Q: Calculate Ecell for the following cell: Pt(s) | H2(g) | H *(aq) || Pb2*(aq) | PBSO4(s) | Pb(s) given…

Q: At 25 °C, a titration of 15.00 mL of a 0.0560 M AgNO3 solution with a 0.0280 M Nal solution is…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3521 V at 25 °C. Pt(s) | H,(g, 0.785…

Q: rship X Report - Go X tActivity.do?locator=assignment-take Grammarly X NGLSync Pc X OWLv2 | OnliX +…

Q: Hi, can you write which is oxidation and which reduction with equation for Fe/Sn, Fe/Zn, Fe/Al,…

A: Oxidation takes place when there is an increase in the oxidation state or loss of electrons.…

Q: Use the Rererences to access mportant values II heeded Tor uis qu 2-ele2 Consider the following cell…

Q: Standard reduction potential E° Fe3+ / Fe2+ =0.77V What is the value (reduction potential for…

A: Solution: Standard reduction potential: It is the reduction potential of the given element or…

Q: The concentration of NO3- in a water sample is determined by a one-point standard addition using a…

Q: John makes a galvanic cell with the half-reactions Mt3+(aq) + 3e1- -->Mt(s), and R2+(aq) + 2e1- -->…

A: This question can be solved using the formula which state that greater cell potential represent…

Q: Given that standard reduction potentials at 298.15 K are E° Mg*2 /Mg = -2.37 V and E° Sn2*/Sn =…

Q: The selectivity coefficient, Kgr, for a K ion-selective electrode is 0.00437. When the electrode is…

A: Given: Selectivity coefficient =0.00437 [K+] = 3.63 x10-5 M pH= 6.65 Potential =-0.175 V vs SCE pH…

Q: The F− concentration of a solution was determined by measurements with a liquidmembrane electrode.…

Q: At a temperature of 25 ° C the galvanic element Pt | MnO4- 0,10M, Mn2 + 0,1M, pH = 1 | Ag + 0.0001M…

A: Given: 1) At a temperature of 25 ° C the galvanic element: Pt | MnO4 0.10M- , Mn0,1M+2 pH = 1 |…

Q: t 25C, you conduct a titration of 20.00 mL of a 0.0400 M AgNO3 solution with a 0.050 M NaI solution…

A: In electrochemistry, the Nernst equation is an equation that relates the reduction potential of an…

Q: The selectivity coefficient, Kg-je, for a K* ion-selective electrode is 0.00348. When the electrode…

Q: 1) a) What is i) a standard solution? ii)a reduction-oxidation (redox) reaction? b) A standard…

A: 1.(a) i) A standard solution is a solution which is prepared with great precision that the…

Q: Given the standard reduction potentials (Eo ’) for ubiquinone (Q) Q + 2H+ + 2e- ---> QH2 E o ’ =…

A: Given that FMNH2 is oxidized and Q is reduced.

Question

e) Using the half reaction below
sHE
Pou3-
HPO,2 + 2H* + 2e
HPO+H;O E--0,234 V
and acid dissociation constants for H3PO4 (K=7.11 × 10°; K2 = 6.32 × 10*, K7.1
x 1014), calculate standard reduction potential for the half reaction
he Oy
H2POª + H* + 2e
HPO + H;O

Expert Solution

Step 1

Step 2

Step 3

Step by step

Solved in 5 steps with 5 images

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

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
Atomic masses can be determined by electrolysis. In one hour, a current of 0.600 A deposits 2.42 g of a certain metal, M, which is present in solution as M+ ions. What is the atomic mass of the metal?
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?
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?
The Nernst equation allows determination of the cell potential for a galvanic cell at nonstandard conditions. Write out the Nernst equation. What are nonstandard conditions? What do , n, and Q stand for in the Nernst equation? What does the Nernst equation reduce to when a redox reaction is at equilibrium? What are the signs of G and when K 1? When K 1? When K = 1? Explain the following statement: determines spontaneity, while determines the equilibrium position. Under what conditions can you use to predict spontaneity?
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)?
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1, calculate the equilibrium constant at 25C for the reaction A13+(aq)+6F(aq)A1F63(aq)K=?
What is electrochemistry? What are redox reactions? Explain the difference between a galvanic and an electrolytic cell.
Consider the following galvanic cell: a. Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow. b. Determine the standard cell potential. c. Which electrode increases in mass as the reaction proceeds, and which electrode decreases in mass?