A Zn wire and Ag/AgCl reference electrode saturated with KCI (E = 0.197 V) are placed into a solution of Z.SO̟. The Zn wire is attached to the positive terminal and the Ag/A£CI electrode is attached to the negative terminal of the potentiometer. Calculate the [Zn²+] in the solution if the cell potential, Ecel , is – 1.093 V . The standard reduction potential of the Zn²+/Zn half-reaction is –0.762 V.

A Zn wire and Ag/AgCl reference electrode saturated with KCI (E = 0.197 V) are placed into a solution of Z.SO̟. The Zn wire is attached to the positive terminal and the Ag/A£CI electrode is attached to the negative terminal of the potentiometer. Calculate the [Zn²+] in the solution if the cell potential, Ecel , is – 1.093 V . The standard reduction potential of the Zn²+/Zn half-reaction is –0.762 V.

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

Related questions

Q: A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a…

A: We will calculate the concentration of Zn2+ ion by using Nernst Equation.

Q: Calculate the standard reduction potential of PuO22+ to Pu(s), given the following standard…

A: Answer:Extensive properties are the ones that depend on the size of the system and are additive in…

Q: Consider the following two oxidation potentials. Determine the spontaneous E° cell that would result…

Q: True or False: The reaction, S20g2- + Ni(OH)2+ 20H¯→ 2S0,2- + NiO, + 2H,0, will occur spontaneously…

A: The reaction is said to be spontaneous, if Ecell is positive. The given reaction is S2O8–2 +…

Q: True or False: The reaction, S₂0g2+ Ni(OH)₂ + 2OH2SO42+NiO₂ + 2H₂0, will occur spontaneously under…

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: Given that, a cell reaction is Cu2+aq + Zns →Cus + Zn2+aq. The concentrations are [Cu2+] = 1.16 M…

Q: A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a…

Q: When the Agt concentration is 8.20 x 10-4 M, the observed cell potential at 298 K for an…

Q: Using these metal ion/metal standard reduction potentials: Cd2+ lCd : -0.38 V ; Zn2+ lZn : -0.76 V…

Q: Using the Nernst equation calculate the cell voltage for: Fe(s) + Cd²+(aq) → Fe2+(aq) + Cd(s) when…

A: Given- [Fe2+] = 0.19 M [Cd2+] = 2.0 M E°cell = -0.44 V E°cell = -0.40 V

Q: An electrochemical cell is constructed with a Zn (s) electrode in contact with a 0.0520 M solution…

A: Given: Concentration of Zn2+ = 0.0520 M Concentration of Ag+ = 0.00420 M And temperature = 5.0 oC

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cr³+ (aq)…

Q: A voltaic cell consists of an Mn/Mn2+ half-cell and a Cd/Cd2+ half-cell. Calculate [Mn2+] when…

Q: A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a…

A: Given,The cell potential, Ecell = - 1.098 VThe standard reduction potential of the Zn2+/Zn…

Q: A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a…

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

Q: A Zn wire and Ag/AgCl reference electrode saturated with KCI (E = 0.197 V) are placed into a…

Q: 4. Standard reduction potentials are temperature dependent. Standard reference data is collected at…

A: To find standard electrode potential for the reaction.

Q: Xglx3+ (1.93 M) || Mn O, 1 minus (1.20 M)|Mn²* (0.27 M)|H* (2.72 M) The reduction potential for X3+…

A: Given values : (I) concentrations of :1. X3+=1.93 M2. MnO4-=1.20 M3. Mn2+=0.27 M4.…

Q: › At 25 °C, a titration of 15.00 mL of a 0.0280 M AgNO3 solution with a 0.0140 M Nal solution is…

Q: A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation,…

Q: What is the emf of a cell consisting of a Pb²* / Pb half-cell and a Pt/H* / H₂ half-cell if…

A: The objective of this question is to calculate the electromotive force (emf) of a cell consisting of…

Q: %3D Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr+] = 0.792 M…

A: The given equation is:- Cr(s) + Sn2+(aq) → Cr2+(aq) + Sn(s) Here, no of electrons transferred = 2…

Q: see the attached

A: A. We can use the Nernst Equation to generate an equation that relates the potential of the given…

Q: A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a…

A: Given; Standard electrode potential of Ag/AgCl is 0.197 V Ecell is -1.077V Standard reduction…

Q: Calculate the potential measured for the following cell at 298 K. Cr(s) | Cr3+ (ag) (0.0025 M) I|…

Q: A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a…

Q: Calculate the value of Eºcell for the following reaction as written: HINT: Identify what is being…

A: Answer: In a cell reaction, oxidation always occurs at anode and reduction always occurs at cathode…

Q: ||| ELECTROCHEMISTRY Calculating standard reaction free energy from standard... Using standard…

Question

A Zn wire and Ag/A£CI reference electrode saturated with KCI (E = 0.197 V) are placed into a solution of ZNSO, . The Zn wire
is attached to the positive terminal and the Ag/AgCl electrode is attached to the negative terminal of the potentiometer. Calculate
the [Zn+] in the solution if the cell potential, Ecell , is – 1.093 V. The standard reduction potential of the Zn²+/Zn half-reaction
is –0.762 V.
[Zn**] =

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

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

A Zn wire and Ag/AgCl reference electrode (E° = 0.197 V) are placed into a solution of ZnSO4. The Zn wire is attached to the positive terminal and the Ag/AgCl electrode is attached to the negative terminal of the potentiometer. Calculate the [Zn2+ ] in the solution if the cell potential, Ecell, is -1.091 V. The standard reduction potential of the Zn2 +/Zn half-reaction is –0.762 V.
One-half of an electrochemical cell consists of a pure nickel electrode in a solution of Ni2+ ions; the other half is a cadmium electrode immersed in a Cd2+ solution. Use the following standard emf series Table (if required). Standard Electrode Electrode Reaction Potential, V" (V) Au³+ + 3e → Au +1.420 O2 + 4H+ + 4e Pr2+ + 2e 2H2O +1.229 Pt -+1.2 Ag+ + e Fe+ + e → Ag Fe2+ +0.800 +0.771 Increasingly inert (cathodic) O2 + 2H,O + 4e Cu²+ + 2e 4(OH) +0.401 Cu +0.340 2H* + 2e Pb2+ + 2e H2 0.000 Pb -0.126 Sn2+ + 2e Sn -0.136 Ni2+ + 2e Ni -0.250 Co2+ + 2e Cd²+ + 2e Fe+ + 2e Co -0.277 Cd -0.403 Fe -0.440 Cr+ + 3e Cr -0.744 Increasingly active (anodic) Zn2+ + 2e¯ Zn -0.763 AF+ + 3e Al -1.662 Mg²+ + 2e Mg -2.363 Na+ + e –→ Na -2.714 K* + e -→ K -2.924 If the cell is a standard one, write the spontaneous overall reaction and calculate the voltage that is generated. Ni2+ + Cd ---> Ni + Cd2+ and +0.153 V Ni + Cd2+ ---> Ni2+ + Cd and +0.153 V Ni2+ + Cd ---> Ni + Cd2+ and -0.153 V Ni + Cd2+ Ni2+ + Cd…
An electrochemical cell is constructed using 0.50 M NiSO4 and a solid nickel electrode in one half cell and 2.0 M ZnCl2 and a solid zinc electrode in the other half cell. The cell is run at 25oC. What voltage would be expected from this cell? Enter the response to 2 significant figures.
. Consider a galvanic cell with the anode containing a Zn metal electrode and a 0.10 M Zn(NO3)2solution and the other half-cell containing a Sn metal electrode and a 0.10 M Sn(NO3)2 solution. If themeasured Ecell value is +650 mV and the Zn2+/Zn reduction potential is assumed to be −790 mV, what isthe Sn2+/Sn reduction potential? Show all work.
A Pt wire is immersed in a solution containing V2+ and V3+ at equal activities of 0.01000. This half-cell is connected through a salt bridge to a Ag-AgBr half-cell in which aBr-= 0.100. The EMF of this galvanic cell is measured to be 0.385 V at 25 C and the electrode in the vanadium solution is the negative electrode. What is the standard electrode potential of the V2+-V3+ electrode? Write out the galvanic cell reaction.
Calculate the Ecell Value at 298 K for the cell based on the reaction: Cu(s)+2Ag*(aq) Cu²+(aq) +2Ag(s) where [Ag*] = 0.00375 M and [Cu2+] = 8.25×104 M. The standard reduction potentials are shown below: Ag"(aq) +e → Ag(s) E° : 0.7996 V Cu²+ (aq) + 2e¯ → Cu(s) E° = 0.3419 V 3rd attempt Feedback Ecell= 0.47713 V
50.0 mL of 0.100 M Co3+ solution is titrated with 35.00 mL of 0.130 M MnO42- solution. The potential is measured against the Ag-AgCl reference electrode. Find the measured cell potential. E0 (Ag/AgCl) = 0,197 V Co3+ + e- ↔ Co2+ E0 = 1,92 V MnO4- + e- ↔ MnO42- E0 = 0,56 V