Question

Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a...

Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of Zn electrodes, each immersed in ZnSO4 solution. One solution is created to be exactly 0.500 M, and the potential on its electrode is measured to be 0.075 V higher than the other electrode. What is the concentration of the other solution? Enter your answer in M.

Homework Answers

Answer #1

The Cell under consideration is expressed as

     Zn|Zn2+ (C1) || Zn2+ (C2 )|Zn

The EMF of this cell is calculated as

    

From the given data we get

     

The unknown concentration C2 is calculated as

    

     

           

           

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a...
Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of Zn electrodes, each immersed in ZnSO4 solution. One solution is created to be exactly 0.400 M, and the potential on its electrode is measured to be 0.045 V higher than the other electrode. What is the concentration of the other solution? Enter your answer in M.​
One half of an electrochemical cell consists of a pure nickle electrode in a 0.001 molal...
One half of an electrochemical cell consists of a pure nickle electrode in a 0.001 molal solution, and the other half is a cadmium electrode immersed in a 0.5 molal solution. The electrode potential is given by , where is the standard electrode potential and c is the molal concentration of the ions in the solution. The cell potential is most likely? a) -0.65 V b) -0.15 V c) -0.073 V d) +0.75 V
Electrochemical Cell Potentials Table 1: Electrochemical Cell Potentials Cell Measured Total Potential from Multimeter (V)1 Individual...
Electrochemical Cell Potentials Table 1: Electrochemical Cell Potentials Cell Measured Total Potential from Multimeter (V)1 Individual Half-Cell Potentials Cell Reactions5 ΔG (kJ)6 (Cu) Electrode Standard Potential (V)2 Metal Electrode Experimental Potential (V)3 Metal Electrode Theoretical Potential (V)4 Metal Electrode Potential % Error Cu | Sn 0.469 0.34 V 0.34-0.469 =-0.129 Cathode:       Cu2+ + 2e- -> Cu Anode:            Sn ->Sn2++ 2e- Net:          Cu2+ + Sn -> Cu + Sn2+ Cu | Al 0.796 0.34 V 0.34-0.796 =-0.456 Cathode:   Cu2+ +...
What is the calculated value of the cell potential at 298 K for an electrochemical cell...
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H2 pressure is 5.00×10-3 bar, the H+ concentration is 1.46 M, and the Zn2+concentration is 3.42×10-4 M ? 2H+(aq) + Zn(s) ----> H2(g) + Zn2+(aq) Answer: _____ V ? The cell reaction as written above is product-favored (spontaneous) for the concentrations given: _______(true/false)?
A) A galvanic cell Zn(s)|Zn2+(aq) || Ni2+(aq)|Ni(s) is constructed using a completely immersed Zn electrode that...
A) A galvanic cell Zn(s)|Zn2+(aq) || Ni2+(aq)|Ni(s) is constructed using a completely immersed Zn electrode that weighs 43.2 g and a Ni electrode immersed in 503 mL of 1.00 M Ni2+(aq) solution. A steady current of 0.0555 A is drawn from the cell as the electrons move from the Zn electrode to the Ni electrode. Which reactant is the limiting reactant in this cell? Enter symbol ___________ How long does it take for the cell to be completely discharged? _____s...
A voltaic cell contains two half-cells. One half-cell contains a nickel electrode immersed in a 1.00...
A voltaic cell contains two half-cells. One half-cell contains a nickel electrode immersed in a 1.00 M Ni(NO3)2 solution. The second half-cell contains a titanium electrode immersed in a 1.00 MTi(NO3)3 solution. Ni2+(aq) + 2 e− → Ni(s)     E⁰red  = −0.257 V Ti3+(aq) + 3 e− → Ti(s)     E⁰red = −1.370 V (a) Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell. ____V (b) Write the overall balanced equation for the voltaic cell....
A voltaic cell is set up with copper and hydrogen half-cells. Standard conditions are employed in...
A voltaic cell is set up with copper and hydrogen half-cells. Standard conditions are employed in thecopper half-cell, Cu2+(aq, 1.00 M)|Cu(s). The hydrogen gas pressure is 1 atm, and [H+] in the hydrogen half-cell is the unknown. A value of 0.500 V is recorded for Ecellat 298 K. Determine the pH of the solution.
A student measures the potential of a cell made up with 1.0 M CuSO4 in one...
A student measures the potential of a cell made up with 1.0 M CuSO4 in one solution and 1.0 M AgNO3 in the other. There is a Cu electrode in the CuSO4 and a Ag electrode in the AgNO3. A salt bridge connects the 2 half cells. The student finds that the potential, or voltage of the cell, E°cell is 0.45 V and that the Cu electrode is negative. a. At which electrode is the oxidation occurring? ___________ b. Write...
In order to determine the identity of a particular transition metal (M), a voltaic cell is...
In order to determine the identity of a particular transition metal (M), a voltaic cell is constructed at 25°C with the anode consisting of the transition metal as the electrode immersed in a solution of 0.018 M M(NO3)2, and the cathode consisting of a copper electrode immersed in a 1.00 M Cu(NO3)2 solution. The two half-reactions are as follows: M(s) <--------> M2+(aq) + 2e– Cu2+(aq) + 2e– <--------> Cu(s) The potential measured across the cell is 0.79 V. What is...
ou want to set up a series of voltaic cells with specific cell potentials. A Co2+(aq,...
ou want to set up a series of voltaic cells with specific cell potentials. A Co2+(aq, 1.0 M)| Co(s) half-cell is in one compartment. Choose the half-cell that you could use so that the cell potential will be close to 0.14 V with the cobalt cell as the cathode. E°Co/Co2+ = -0.28 V E°Al/Al3+ = -1.66 V E°Cu/Cu2+ = +0.337 V E°Sn/Sn2+ = -0.14 V cadmium aluminum copper tin
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT