Mn(k) | Mn²+(0.2 M) || H+ (pH= ?) | H2 (g, 1.5 atm) | The cell potential of the Pt(k) Cell was found to be 1.04 V. Since it is known that the standard reduction electrode potential of the manganese electrode is -1.18 V, calculate the pH of the solution whose concentration is unknown.

Mn(k) | Mn²+(0.2 M) || H+ (pH= ?) | H2 (g, 1.5 atm) | The cell potential of the Pt(k) Cell was found to be 1.04 V. Since it is known that the standard reduction electrode potential of the manganese electrode is -1.18 V, calculate the pH of the solution whose concentration is unknown.

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: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: In electrochemical cell , the value of potential difference between two electrodes is known as cell…

Q: Given the cell notation M1 | M12+(aq) | | M2+(aq) | M2, calculate the standard potential of the…

A: The cell given is, => M1 | M12+ (aq) || M2+ | M2 Given : Standard reduction potential of M1 =…

Q: Ⓒ Macmillan Learning Calculate the cell potential for the reaction as written at 25.00 °C, given…

A: Given

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

Q: A chemical reaction system is represented by this equation. Ag(s) + Br(aq) + Fe3+(aq) → Fe2+(aq) +…

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

Q: Can you explain it?

A: Given:…

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

Q: Consider the following galvanic cell: Ag(s) | Ag*(3.0 × 10“M) || Fe³*(1.1 × 10³ M), Fe²"(0.040 M) |…

A: Given,

Q: 1. For the following reaction at 25 °C, 3+ SFe2+(aq) + Mn (aq) + 8H+(aq) = 5Fe³+ (aq) + Mn²+ (aq) +…

A: We have find out the (a) the standard potential, (b) the equilibrium constant, and (c) the potential…

Q: 1 Using these metal ion/metal standard reduction potentials: Cd2+ (aq)|Cd(s): -0.38 V: Zn2+…

A: Given, Cu2+(aq) + Cd(s) ➝ Cd2+(aq) + Cu(s) Standard cell potential (E°cell) = ? Standard reduction…

Q: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Given-> [Cr2+] = 0.790 M [Fe2+] = 0.0190 M T = 25°C

Q: at 25 ° C, the galvanic element Pt | MnO4- 0.1M, Mn2 + 0.1M, pH = 1 || Ag + 0.0001M | Ag has the…

A: Welcome to bartleby !

Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A: Ni(s) + 2 H+(aq) ⇔ Ni+2(aq) + H2 (g) Ecello = 0.23…

Q: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Cr(s)+Fe+2 (aq )<==> Cr+2 (aq)+Fe(s) [Cr+2] = 0.768 M [Fe+2] = 0.0170 M

Q: The following cell was constructe SCE||KBr|AgBr(sat'd)|Ag. If the measured cell potential was V,…

A: Disclaimer: There is some discrepancy either in the data or the given options as the answer does not…

Q: Calculate K for scandium fluoride, SCF3, given that the cell potential at 25 °C for the following…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: We have tp Calculate the standards potential value for the following cell reaction…

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 cell potential of the following cell is determined using an unspecified concentration of acid.…

Q: How do I calculate the cell potential of this situation?

A: We have given a galvanic cell in which [Ti3+] = 0.02723 M [TiO2+] = 0.00146 M pH = 3 ESHE = 0.00V…

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: Given that the standard electrode potentials (E°) of metals are:K+/K = -2.93 V, Ag+/Ag = 0.80…

A: standard electrode potentials (E°) is inversely proportional to reducing power Higher standard…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: a) E=+0.61V B) E=+0.16V

Q: For the cell shown, the measured cell potential, ?cell, is −0.3553 V at 25 °C. Pt(s) |…

Q: When the Ag* concentration is 1.36x10-4 M, the observed cell potential at 298K for an…

Q: For the cell shown, the measured cell potential, ?cellEcell, is −0.3669 V at 25 °C. Pt(s) |…

Q: Consider the cell diagram for an electrochemical cell: Pt | Ti2+(aq), Ti3+(aq) || Br2(g), Br-(aq) |…

A: For the electrochemical cell: Pt | Ti2+(aq), Ti3+(aq) || Br2(g), Br-(aq) | Pt having E = 1.40 V , we…

Q: Consider the following galvanic cell at 25°C Pt|Br (aq) (0.25 M), H* (aq) (0.1 M) |Br2 () || O2 (g)…

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

Q: Calculate the cell potential. Is the cell galvanic or electrolytic? Pt|Fe3+(5.00 x 10-4 M), Fe2+…

Q: X(s)|X5+ (0.94 M) || Mn O4 1 minus (1.10 M)|Mn O2(s)|H+ (0.51 M) The reduction potential for X5+ is…

A: The Nernst equation is shown below: Where: Ecell = cell potential E0cell = standard cell potential…

Q: 1) The standard reduction potentials of Cu2+ (aq) Cu(s) and Ag+ (aq) Ag(s) are +0.34 and +0.80 V,…

A: Calculate the cell potential of the given galvanic cell. Given At Anode Cu/Cu2+; E°=-0.34 V At…

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: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.30 M), Cr³+ (2.0 M) || Co2+ (0.20 M) | Co…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + With(so much) =…

Q: Calculate the potential measured for the following cell at 298 K. Cr(s) | Cr3*(aq) (0.0055 M) ||…

A: Given that: molarity of Cr/Cr3+ = 0.0055 M molarity of Ni/Ni2+ = 1.27 M Eocell = 0.50 V To find:…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: Standard reduction potential of nickel = -0.257 V Standard reduction potential of silver = 0.7996 V…

Q: What is the balanced chemical equation for this galvanic cell reaction? Cr(s) | Cr3*(aq), 1M || CI-…

Q: Consider the following cell reaction: Cd(s) + 2 H*(? M)=Cd²+(1.00 M) + H₂(g)(1.00 atm) If the cell…

A: The cell reaction given is, Given: Cell potential = 0.168 V And temperature = 298 K

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: 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: The standard reduction potential of the zinc cation is -0.76 V. The measured cell potential for the…

Q: Based on these data, what is the value of the formation constant, K, of (Cu(NH,)

A: Given: [NH3] = 1 M [Cu(NH3)42+] = 1 M [Cu2+] = 2 x 10-14 M

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 constructed with a nickel electrode that was dipped into 1.3 M NISO4 solution…

A: Answer:- This question is answered by using the simple concept of calculation of concentration using…

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

Mn(k) | Mn²+(0.2 M) || H+
(pH= ?) | H2 (g, 1.5 atm) | The
cell potential of the Pt(k) Cell
was found to be 1.04 V. Since
it is known that the standard
reduction electrode potential
of the manganese electrode is
-1.18 V, calculate the pH of the
solution whose concentration is
unknown.

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 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

The cell potential of the following cell is determined using an unspecified concentration of acid. What is [H*]given that the measured cell potential is -0.366 V and the anode reduction potential (E°) is 0.222 V at 25°C? Ag(s) | AGCI(s) | CI(1.0 M) || H*(aq, ? M) | H2(g, 1.0 atm) | Pt(s) 4.9 x 10-5 M 3.7x 10-3 M O 6.1x 10-2 M
Please don't provide handwritten solution .....
Using these metal ion/metal standard reduction potentials: Cd2+ (aq)| Cd(s): -0.38 V; Zn2+ (aq) Zn(s): -0.78 V; Ni2+ (aq) |Ni (s): -0.29 V; Cu2+ (aq)| Cu(s): 0.30 V. Calculate the standard cell potential in V for the cell reaction Cu²+ (aq) + Cd(s)→Cd²+ (aq) + Cu(s) Report your answer with 2 places past the decimal point. Do not put unit in your answer. Type your answer...
Using the provided standard reduction potentials, which of the following cells is an example of a Galvanic cell? A Zn(3)| Zn*r||Cu*|Cu(e) В © Au(s)|Au|| Mn**|Ma(e) 2+ Co(s)| Co*" Fe* |Fe(e)
edit: Calculate the cell potential for the following galvanic cell at 25°C: Al(s) Al3+ (0.0632 M)|| Au3+ (0.255 M)|Au(s)
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
Calculate the EMF of the following electrochemical cell: Pt | VO2+(0.25 M), V3+(0.10 M), H+ (0.001 M) || TI3+ (0.10 M), TI+(0.05 M), | Pt Indicate whether the cell is galvanic or electrolytic. Evo2+/v3+ = 0.361 V, ET³+/T+ = 1.25 V Ans: 1.23 V, galvanic
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!
A galvanic cell was constructed with a nickel electrode that was dipped into 1.1 M NiSO4 solution and a chromium electrode that was immersed into a solution containing Cr3+ at an unknown concentration. The potential of the cell was measured to be 0.557 V, with the chromium serving as the anode. The standard cell potential for this system was determined to be 0.487 V. What was the concentration of Cr3+ in the solution of unknown concentration?
Pt(k)| Fe³+(aq), Fe²+(aq) // I-(aq) | 12(k) | Calculate the standard cell potential for the Pt(k) Cell and interpret whether the reaction taking place in the cell will proceed spontaneously under standard conditions. E° (Pt|Fe³+, Fe²+) = 0.77 V . E°( 12 | I-) = 0.53 V
The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =
Consider the following cell: Ni(s)|Ni2+(aq, 0.100 M)||Cl–(aq, 0.200 M)|Cl2(g, 1.50 atm)|Pt If the standard voltage for this cell is 1.59 V at 25oC, calculate the voltage of this cell.