Analysis of the lead/lead(ll) iodide concentration cell: Write the overall react

Question

Analysis of the lead/lead(ll) iodide concentration cell: Write the overall reaction equation, indicating which species where at the cathode and which were at the anode. Use the Nernst equation, the cell potential you measured, and the known [Pb^2+]_cathode to calculate the [Pb^2+]_anode in equilibrium with Pbl_2. Determine the (I^-] in equilibrium with Pbl_2. Calculate the K_sp of Pbl_2. The accepted value of the K_sp of Pbl_2 is 9.8 Times 10^-9. Calculate the percent error in for the value of K_sp. How does your experimental of Pbl_2 compare to the accepted value?

Explanation / Answer

You missed a lot of information here as the experiment you are doing, the E potential measured (For part b), and the whole cell potential. I can only know that one of the reactants is PbI2 but I don't know the other one so I can help with the first part of this problem.

a). I need more data of this experiment so I can write the overall reaction and the half reactions too.

b) The nerst equation is the following:

E = E° - 0.059/n log Q

If you provide the value of E, all you need to do is solve for Q:

E = E° - 0.0295 log Q

E - E° / 0.0295 = log Q

10(E° - E / 0.0295) = Q

[Pbanod] / [Pbcath] = Q

[Pbanod]/[Pbcatho] = 10(E° - E / 0.0295)

[Pbanod] = [Pbcatho]10(E° - E / 0.0295)

c) Once you calculate the concentration of Pb anode, you can calculate concentration of I

d) write the reaction nd it would be:

PbI2(s) ----------> Pb2+ + 2I-

Ksp = [Pb2+] [I-]2

e) the error you may calculate:

% = (Kspexp / Ksptheo) * 100

Provide the values and more info about the experiment so I can help you with this question. Post them in a new question if you want. Hope this helps a little.

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