a concentration cell was made by putting 5 mL of 0.050 M Pb(NO3)2 solution into one half-cell in a test plate. for the neighboring well in the test plate, weplaced 5 mL of a PbI2 solution that was made by mixing 9 mL of 0.050 KI solution with 3 mL of 0.050 M Pb(NO3)2 solution inside. Pb Electrodes were placed in eachcell, and a KNO3-soaked string was used as the salt bridge.
data was collected and we recorded the average cell potential t be 0.02751 V
The question asks us to:
A .Use the cell potential for the Pb-PbI2 cell and the known [Pb2+] to calculate the [Pb2+] in
equilibrium with PbI2.
Can anyone help? thank you
Pb - PbI2 cell
oxidation reaction : Pb(s) --->Pb+2 (sat. with PbI2) + 2e-
Reduction reaction : Pb+2 + 2e- ----> Pb(s)
Overall reaction :
Pb+2 -----> Pb+2 (sat)
Ecell = Eo - 0.0592/n log Q
Q = [Pb+2 (sat)] / [Pb+2]
Eo = 0
n = 2 electrons
0.238 = -0.0592/2 * log [Pb+2(sat)] / [0.13]
[Pb+2(sat)] = 1.184*10^-9 M
Calculating the [PB2+] in a voltaic Pb-PbI2 cell using the recorded cell potential
Use the Nernst euation and the cell potential for the Pb-PbI2 cell and the known [Pb2+] to calculate the [Pb2+] in equilibrium with PbI2. The measured avgerage cell potential of Pb-PbI2 is 0.084 V the known [Pb2+] is 0.050 M Eo of Pb2+ (aq) + 2 e- --------> Pb(s) is -0.13 V 0.050 M KI Mixed 9 mL of 0.050 M KI with 3 mL of 0.050 M Pb(NO3)2 .
Which of the following is a proper notation for the voltaic cell consisting of of one half-cell with a zinc electrode in 1 M Zn(NO3)2 solution and the other half-cell with a lead electrode in 1 MPb(NO3)2 solution and a KNO3 salt bridge. Pb2+(1 M) | Pb(s) || Zn(s) | Zn2+(1 M) Zn2+(1 M) | Zn(s) || Pb(s) | Pb2+(1 M) Pb(s) | Pb2+(1 M) || Zn2+(1 M) | Zn(s) Zn(s) | Zn2+(1 M) || Pb2+(1 M) | Pb(s)
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Page 1 and 2 are instructions. Please help me solve K for page 3
and page 4 and please check the other work on Page 3.
Thanyou very much. Will Rate!
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