At 25 °C, a titration of 15.00 mL of a 0.0200 M AGNO, solution with a 0.0100 M NaI solution is conducted within the cell SCE || titration solution | Ag(s) For the cell as written, what is the potential after the addition of each volume of Nal solution? The reduction potential for the saturated calomel electrode is E = 0.241 V. The standard reduction potential for the reaction Ag+ + e → Ag(s) is E° = 0.79993 V. The solubility constant of AgI is Kp = 8.3 x 10-17. 0.500 mL E = V

At 25 °C, a titration of 15.00 mL of a 0.0200 M AGNO, solution with a 0.0100 M NaI solution is conducted within the cell SCE || titration solution | Ag(s) For the cell as written, what is the potential after the addition of each volume of Nal solution? The reduction potential for the saturated calomel electrode is E = 0.241 V. The standard reduction potential for the reaction Ag+ + e → Ag(s) is E° = 0.79993 V. The solubility constant of AgI is Kp = 8.3 x 10-17. 0.500 mL E = 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: For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3559 V at 25 °C. Pt(s) | H₂(g, 0.767…

Q: Consider the electrolysis reactions cathode Cu?"(aq, 0.177 M) + 2e-= Cu(s) H,O) =0,(g, 1 bar) + 2H*…

Q: 2(g) |H '(aq) || Pb<'(aq) | PBS04(s) | Pb(s) he following standard reduction potentials. q) + 2 e¯ ®…

A: Cell equation, Sn2+ + Cu2+ ---> Sn4+ + Cu Cell potential is affected by concentration. As the…

Q: A concentration cell based on the following half reaction at 288 K Ag +e Ag; SRP = 0.80V is made…

A: Reaction on L.H.E.: Ag(s) ⇌Ag+(0.354M) + e- A⏜A (oxidation) Reaction on R.H.E. Ag+(1.4 M)+e-⇌Ag(s)…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The call reaction at anode is, H2(g) ------> 2H+(aq) + 2e- Standerd cell potential of the cell =…

Q: For the cell shown, the measured cell potential, ?cell, is −0.3681 V at 25 °C. Pt(s) |…

Q: The measured cell potential, Ecell, for the cell shown is –0.3549 V at 25 °C. Calculate the H*…

A: If standard reduction potential values of two half cells are given then the half cell with less…

Q: The reduction potential for all other half-reactions are measured relative to the half-reaction…

Q: A galvanic cell was prepared by immersing an anode and a cathode of the same material (of A type) in…

Q: [Review Topics] [References] An electrochemical cell consists of a standard hydrogen electrode and a…

Q: а. Write the balanced electrochemical reaction. Use the reduction potentials to determine E°: i.…

A: An electrolytic cell is a cell which requires an outside electrical source to initiate the redox…

Q: Consider the following silver-cadmium cell: Cd(s)/Cd2+(0.50 M)//Ag+(0.0025 M)/Ag(s). Compute the…

A: To calculate the cell potential for the given silver-cadmium cell at 25oC, we can use the…

Q: Consider the following cell: Fe(s) | FeBr2(0.018 M) || NaBr(0.065 M) | Br2(e) | Pt(s) a) Using the…

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

Q: Determine the cell potential and the equilibrium concentrations of the following concentration cell:…

A: The given cell notation is: Cu|Cu2+0.020 M||Cu2+2.0 M|Cu It is a concentration cell (electrolytic…

Q: Calculate the cell potential, ?, for the given reactions at 25.00 °C using the ion concentrations…

Q: The standard reduction potentials for Mg2+/Mg (E'= -2.37 V) and Fe2*/Fe (E'= -0.44 V). When a piece…

A: Concept- By the help of nernst equation, this problem can be solved. Ecell=Eocell− 0.0592/n log10Q…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3657 V at 25 °C. Pt(s) | H₂(g, 0.777…

A: Ecell = 0.3657 V PH2 = 0.777 atm The balanced reduction half reactions 2 H+ (aq) + 2 e- ----->…

Q: The equilibrium constant, K. for a redox reaction is related to the standard cell potential, E by…

A: Part (A) : Temperature , T =25°C=(25+273)K=298 K Given reaction is : Fe(s) + Ni2+ (aq) →Fe2+ (aq) +…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3621 V at 25 °C. Pt(s) | H₂(g, 0.765…

A: Answer: This question is based on Nernst equation which is shown below: Ecell=Ecell0-0.0592nlogQ…

Q: The cell potential for this reaction is, V when [ Zn2*] = 1.0 M and [Pb2*] = 2.0 x 10-4 M. Pb2+ (aq)…

A: The cell potential is calculated by Nernst equation . E = E° - (0.0591/n) log Qc E = cell potential…

Q: Use the References to access important values if needed for this question. Use standard reduction…

A: " Since you have posted multiple questions, we will provide the solution only to the first question…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr*] = 0.810 M and…

A: The cell reaction given is, => Cr (s) + Fe2+ (aq) ⇔ Cr2+ (aq) + Fe (s) Given: [Cr2+ ] = 0.810 M…

Q: If at 25°C the standard electrode potential of the Ag/Ag* electrode is 0.799 V, and the equilibrium…

Q: 24. Given the following electrode (reduction) potentials: Fe3+ + e --> Fe2*; E° = 0.77 V Cu2* + 2e¯…

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au*(aq) =…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3725 V at 25 °C. Pt(s) | H₂(g,0.849…

Q: 12.) The following cell is prepared and found to have a standard cell potential of 1.74 V: Pt (s)|Cl…

A: Cell representation:

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given Ecell =0.189we know E°cell is 0 for hydrogen cell.

Q: Half cell 2: A platinum electrode in a solution containing both 1.0 M Fe2*(ag) and 1.0 M Fe3* (aq)…

A: Given: Eo reduction for half cell 1=+0.34 VEo reduction for half cell 2=+0.77 VEo reduction for half…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3643 V at 25 °C. Pt(s) | H₂ (g,0.895…

A: Cell potential, Ecell= -0.3643 VHalf-cell reactions are also given.

Q: What is the cell reaction and cell potential for a spontaneous cell formed form the following…

A: Given Ag+ + 1 e- → AgEAg+/Ag0 = 0.80 VFe2+ + 2e- → FeEFe2+/Fe0 = -0.44 V

Q: 1. Calculate the cell potential, AG (J), and the equilibrium constant Keq for the following…

A: Calculation of Cell potential of the cell

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

Q: The measured cell potential, Ecell, for the cell shown is –0.3549 V at 25 °C. Calculate the Ht…

A: Given: E∘cell is -0.3549 V. H2→2H+aq+ 2e- Eo=0.00 V Cd2+aq+ 2e-→Cds Eo=-0.403 V…

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: The saturated calomel electrode, abbreviated SCE, is often used as a reference electrode in making…

A: For the galvanic cell we know that, the electrode having greater standard reduction potential will…

Q: Calculate E° cll from the tabulated standard reduction potentials for each of the following…

A: In the given reaction MnO4- is getting reduced while Fe+2 is getting oxidised.

Q: Consider the following electrochemical cell in which X is an unknown metal: Pt | Cl-(1 M) | Cl2( 1…

A: Here, in the given cell notation, first of all the notation has to be understood. Pt | Cl- (1 M) |…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3537 V at 25 °C. Pt(s) | H₂(g, 0.837…

A: Cell potential, Ecell= -0.3537 VHalf-cell reactions are also given.

Q: For the cell shown, the measured cell potential, Ecell, is -0.3651 V at 25 °C. Pt(s) | H₂(g, 0.797…

Q: A galvanic cell was prepared by immersing A type) in a solution containing a low solub concentration…

Q: 26. Given the following electrode (reduction) potentials: Ag* + e --> Ag; E° = 0.80 V Zn2+ + 2e -->…

Q: Using these metal ion/metal standard reduction potentials: Cd²+ (aq)| Cd(s): -0.38 V; Zn²+ (aq…

A: To determine the standard cell potential, we use- E∘cell = E∘cathode -E∘anode Cathode is the…

Q: If at 25°C the standard electrode potential of the Ag/Ag' electrode is U.799 V, and the equilibrium…

A: Fe+3 + Ag ------> Fe+2 + Ag+ EoAg|Ag+= 0.799 V K = 0.531 V

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

At 25 °C, a titration of 15.00 mL of a 0.0200 M AGNO, solution with a 0.0100 M Nal solution is conducted within the cell
SCE || titration solution | Ag(s)
For the cell as written, what is the potential after the addition of each volume of Nal solution? The reduction potential for
the saturated calomel electrode is E = 0.241 V. The standard reduction potential for the reaction Ag+ + e-
E° = 0.79993 V. The solubility constant of AgI is Kgp = 8.3 × 10-1".
Ag(s) is
>
0.500 mL E =
V
18.90 mL
E =
V

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

Step 5

Step 6

Step 7

Step 8

Step 9

Trending now

This is a popular solution!

Step by step

Solved in 9 steps

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

For the cell shown, the measured cell potential, Ecell, is -0.3587 V at 25 °C. Pt(s) | H, (g, 0.839 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2 H* (aq) + 2 e H, (g) E° = 0.00 V Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V Calculate the Ht concentration. [H*] = %3D rIC ho C TV OLER EEDO DCD 24 4/2 DELL PrtScr Insert Home End F8 F9 F10 F11 F12 F4 F5 F6 F7
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20oC (293K) is measured as +1.03 V. Calculate the experimental standard cell potential, Eocell, for the reaction
4. The cell diagram for an electrochemical cell is given below: Mn(s) | Mn* (aq, 1.0 mol dm) || Ag* (aq, 1.0 mol dm)|Ag (s) In the above cell, the standard electrode potential of the silver hal f-cell is =0.80 V. E°cell = +1.98 V Write the equation for the reaction occurring at the anode and cathode. Write the overall cell equation Determine the standard electrode potential of the Mn2*/Mn half-cell What is the strongest oxidizing agent in the above cell? What is the strongest reducing agent in the above cell? a) 1) ii) b) i) i1) c) After the cell was used, the change in mass of the silver electrode was found to be 5.40 IS g Caleulate the change in mass of the manganese electrode.
The following half-cells are on the left and coupled with the standard hydrogen electrode on the right to form a galvanic Calculate the cell potential. If the cell were shorted, indicate whether the electrodes shown would act as an anode or a cathode. a. Cu Cu²+ (0.0567 M), (Cu²+/Cu = 0.337 V) V Potential = b. Cu | Cul (sat'd), KI (0.0939 M), (ECul/Cu = -0.185 V) Potential = V 3+ c. Pt | Fe³+ (0.160 M), Fe²+ (0.08340 M), (E Potential = V Fe³+/Fe²+ = = 0.771 V)
For the cell shown, the measured cell potential, Ecell, is -0.3619 V at 25 °C. Pt(s) | H₂(g, 0.721 atm) | H¹ (aq, ? M) || Cd²+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2 e H₂(g) Eº = 0.00 V Cd²+ (aq) + 2e → Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+] = TOOLS x10 M
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (PH, )= latm) immersed in a solution of unknown [H*]. If the cell potential is 0.216 V, what is the pH of the unknown solution at 298 K? pH =
Consider the following cell reaction: Fe(s) + 2 H"(? М) —Ғе*"(1.00 М) + H-(g)(1.00 atm) →Fe? If the cell potential at 298 K is 0.164 volts, what is the pH of the hydrogen electrode? pH
Calculate AGº for the following cell reaction: TI(s) | TI* (aq) || Pb3* (aq) | Pb(s) From AG°, determine the standard potential for the half-reaction TI* (aq) + e¯ Tl(s) AG; for TI* (aq) is –32.4 kJ/mol. AG; for Pb?+ (ag) is -24.39 kJ/mol. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E° (V) Pb2+ (ag) + 2e - Pb(s) -0.13 AG° = Standard reduction potential for the half-reaction :
The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?+ (0.20 M) || H* (test solution)|H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn²+ is -0.76 V. (Enter your answer to two significant figures.) pH = %3!
For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq) + 2e– Zn(s) is Eored = –0.76 V What is the standard reduction potential for Tl+(aq) + e– Tl(s) Eored = ? V a. +0.17 V b. –0.17 V c. –0.34 V d. +0.34 V
For the cell shown, the measured cell potential E cell -0.365; V at 25 degrees * C . Pr(s)|H 2 (g,0.803 am)|H^ + (aq,?M)||Cd^ 2+ (aq,1.00 M)|Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values E ^ o are 2H^ + (aq)+2e^ - longrightarrow H 2 (g) E ^ o = 0.00V Cd^ 2+ (aq)+2e^ - longrightarrow Cd(s) E ^ o= - 0.403V Calculate the H^ + concentration.
Given the electrochemical reaction, Mg/ Mg 2(aq) // Zn2(aq) / Zn, E+1.61 V. If the standard reduction potential of Zn²-Zn is -0.76V. What is the standard reduction potential of Mg2+ = Mg? -2.37 V (В 0.85 V -0.85 V 2.37 V