Calculate the potential for the Cu2+/Cu*electrode at 25°C when the Cut ionconcentration is 1/3 of the Cu2+ionconcentration.

Given, Cu+ ion concentration is 1/3 of the Cu2+ ion concentration Calculate the potential of…

Answered: • Calculate the potential for the…

• Calculate the potential for the Cu2+/Cut electrode at 25°C when the Cut ion concentration is 1/3 of the Cu2+ ion concentration.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.27QAP

See similar textbooks

Related questions

Q: Calculate the cell potential for a cell at 40°C with a Cu²+ concentration of 0.009 M and a Zn²*…

A: The cell potential at non-standard condition can be calculated from Nernst equation.

Q: A concentration cell is set up using two zinc wires and two solution, one containing 0.250 M ZnCl2…

A: Given data,Concentration of ZnCl2=0.250MConcentration of Zn(NO3)2=1.65M

Q: Calculate the potential developed by a voltaic cell using the following reaction if all dissolved…

A: Calculate the potential developed by a voltaic cell using the following reaction if all dissolved…

Q: Calculate the potential for the following half-cell: Ag+(0.120M) + 1e- → Ag

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

Q: If the half-cell Li(s)|Li+(aq)(1.0 M) is coupled to Standard Hydrogen Electrode, will the Li(s)…

Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

A: The reduction potential of two elements are Since the reduction potential of Titanium is less…

Q: 5. If you constructed a galvanic cell using an electrode X+IX connected to a standard copper…

A: In the cell or galvanic cell , if two standard half-cell electrode are connected then the resultant…

Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

A: Given: Co2+(aq)+2e-→Co(s) -0.31VCd2+(aq)+2e-→Cd(s) -0.43V To find: potential of this galvanic…

Q: A concentration cell involving copper was set up with the following conditions:…

A: Interpretation - To tell about the measured cell potential when a concentration cell involving…

Q: The Standard potential for the reduction of AgClcS) °sto. 222V. Ag Gles)te→ Agcs) +Cl (aq) 0Singthis…

A: Given: RHE: AgCl(s)+e-↔Ag+Cl- …ER=0.222 V To find: Solubility product constant, Ksp

Q: A concentration cell is set up using two zinc wires and two solution, one containing 0.550 M ZnCl2…

A: In concentration cells the both half cells have same electrode but their concentration will be…

Q: A concentration cell is set up using two zinc wires and two solution, one containing 0.300 M ZnCl2…

A: There are two solutions of Zn2+ ions given in the concentration cell. Out of these two solutions the…

Q: Use the standard half-cell potentials listed in the table to calculate the standard cell potential…

Q: Calculate the potential of the following cell at 25°C: (Al IAIP (0.01M) IZn"(0.0085M)I Zn)

A: Al | Al+3(0.01M)||Zn+2(0.0085 M)| Zn

Q: The standard potential for the reduction of AgSCN(s) is+0.09 V. AgSCN(s) + e- ---->Ag(s) +…

A: Given that the standard potential for the reduction of AgSCN is +0.09 V. The standard reduction…

Q: calculate the electrode potentials of the following half cells: HCL (3.50M) | H2 (0.950atm), Pt.

Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

Q: A particular galvanic cell has a redox reaction in which copper and metal displace silver (1) ions…

A: Given ,the reaction is 2Ag+(aq) +Cu(s)-------------> Cu2+(aq) +2Ag(s)

Q: Calculate the potential of the copper electrode immersed in a. 0.0440 M Cu(NO3)2 b. 0.0750 M in…

A: Hi! Since there are multiple questions posted. We are answering first question. If you need further…

Q: Determine the optimum mass ratio of Zn to MnO2 in an alkaline battery.

A: An alkaline battery produces electrical energy according to the following equation,

Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

A: Redox reaction are those in which both oxidation and reduction take place simultaneously.

Q: c. Number of electrons involved in the redox reaction (n): d. Overall reaction for the voltaic cell:…

A: Given: The concentration of Cd2+ = 1.0 M The concentration of Cu2+ = 0.10 M a). The oxidation half…

Q: Use the standard half-cell potentials listed in Table 16.1 to (Links to an external site.)calculate…

A: Given : cell reaction E°cell = E°red + E°oxid

Q: 16. Consider the following half-cells under standard conditions: Electrolyte X* (aq) Y²*(aq) and…

Q: Consider the concentration cell shown below. Calculate the cell potential at 25°C when the…

A: (a)

Q: A concentration cell is set up using two zinc wires and two solution, one containing 0.400 M ZnCl2…

A: Half-cell reactions are given below,

Q: 7. Calculate the potential of a cadmium electrode immersed in a 0.0100 M Cd2+ solution.

A: Interpretation- To determine the potential of a cadmium electrode immersed in a 0.0100 M Cd2+…

Q: Which of the following electrodes are often used as counter or auxiliary electrode in voltammetry?…

A: Given options are : A. Platinum wire B. Mercury thin film C. Carbon paste D. Calomel electrode Which…

Q: 3.) Consider that the following half'reaction is assigned a half coll vtage of 6 00 V Hg (aq) + 2e…

Q: The electromotive force of the cell for the reaction: Cu2 + + Fe2 + + I- = CuI + Fe3 + is 0.090V.…

Q: Calculate the Ecell between two Cu2+/Cu half-cells, one of which contains 0.001 M Cu2+ and the other…

A: Ecell is defined as the potential difference between the two half cells. The concentration of two…

Q: Write the number only, no need to write the unit (volts). What is the potential of a cell made up of…

A: Cell is made up of two half-cells. Temperature = T = 25°c {0°c = 273K} Temperature = T = 25 +…

Q: A galvanic (voltaic) cell consists of an electrode composed of aluminum in a 1.0 M aluminum ion…

A: From given Two half reactions involved here, They are as follows

Q: A concentration cell is set up using two zinc wires and two solution, one containing 0.300 M ZnCl2…

A: There are 2 solutions of Zn2+ ions in the given concentration cell. Out of these two solutions, one…

Q: A steel railroad bridge uses a zinc sacrificial anode to limit the extent of oxidation of the steel.…

Q: What is the overall spontaneous reaction and cell potential for a voltaic cell made from Mn and Li?

A: For spontaneous reaction according to Standard Electrode potential at 25*C, Mn will reduce and Li…

Q: Calculate the potential of a copper electrode immersed in the solution below. The solution that is…

A: Solution : Electrode potential in electrochemistry is defined as the tendency of a metal to…

Q: If the cell is a standard one, write the spontaneous overall reaction and calculate the voltage that…

A: Since standard reduction potential of Ni+2 is more as compared to Cd+2 so Ni electrode act as…

Q: Calculate the exact half-cell potential for the Ag-AgCl electrode in 1 M NaCl.

A: Note - Since you have asked multiple question, we will solve the first question for you. If youwant…

Q: 2. Using the available materials, design a spontaneous electrochemical cell at standard conditions…

A: At anode, oxidation takes place At cathode, reduction takes place Flow of electrons is from anode to…

Q: A galvanic (voltaic) cell consists of an electrode composed of manganese in a 1.01.0 M manganese(II)…

Q: A voltaic cell is constructed with a Ni//Ni2+ half-cell and a Ag/Ag+ half-cell. The nickel electrode…

Q: A concentration cell is based on the aqueous reaction Cu²"(1.00 M) → Cu²"(0.0100 M) Calculate the…

A: Ans .0591V

Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

A: Cell made-up of two couples Cr(III)/Cr(II) and Co(III)/Co(II) The standard potential of cell can be…

Q: Which of the following is the best reducing agent? You may use the table of standard cell potentials…

A: Reducing agent is the one which undergo oxidation itself. The standard cell potentials of given…

Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

A: The reduction potential of Cd2+(-0.42v) is less than Co2+(-0.28v) hence Cd(s) will undergo oxidation…

Q: A concentration cell is one wherein the concentrations of the same ion in the two electrodes are…

A: The cell potential v/s the concentrations are given as,

Q: Do not have to answer any questions. JUST WRITE THE OBJECTIVES IN YOUR OWN RODS: Objective: To…

A: To write the objective in your own words:

Q: A concentration cell is set up using two zinc wires and two solution, one containing 0.450 M ZnCl2…

A: The oxidation half reaction takes place at anode and cathode are noted as follows, Here, electrode…

Concept explainers

Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.

Question

Calculate the potential for the Cu2+/Cu*
electrode at 25°C when the Cut ion
concentration is 1/3 of the Cu2+
ion
concentration.

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

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

Calculate the minimum difference in standard electrode potentials needed to lower the concentration of the metal M1 to 2.00 10-4 M ¡n a solution that is 1.00 10-1 M in the less-reducible metal M2 where (a) M2 is univalent and M1 is divalent. (b) M2 and M1 are both divalent, (c) M2 is trivalent and M1 is univalent, (d) M2is divalent and M1 is univalent, (e) M2 is divalent and M1 ¡s trivalent.
For each of the following half-cells, compare electrode potentials calculated from (1) concentration and (2) activity data. (a) HCI(0.0200 M),NaCI(0.0300 M)|H2(1.00 atm),Pt (b) Fe(CIO4)2(0.0111 M),Fe(CIO4)(0.0111 M)|Pt
The standard potential of the cell reaction Ag+(aq)+Eu2+(aq)Ag(s)+Eu3+(aq) is E = +1.23 V. Use the tabulated standard potential of the silver half-reaction to find the standard reduction potential for the europium half-reaction.
The standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another electrode potential to use together with the above value and calculate Kspfor AgSCN.
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
From the standard potentials Tl++eTl(s)E0=0.336V TlCl(s)+eTl(s)+ClE0=0.557V calculate the solubility product constant for TlCl.
Calculate the electrode potentials of the following half-cells. (a) Ag+(0.0436 M)|Ag (b) Fe3+ (5.34 10-4M),Fe2+ (0.090 M)|Pt (c) AgBr(sat’d),Br- (0.037 M)|Ag