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Determine the concentration (in M ) of lead ions
Pb^2+ e= -0.13 volts M=?
Ni^2+ e=-.25 volts Ni^2 M=.27M
e=-0.020 volts
![DrBob222](/images/users/0/1/128x128.jpeg)
2 years ago
![bear](/images/users/0/1/128x128.jpeg)
2 years ago
Pb(s) Pb^2+ (aq) [pb^2+] =?M
Ni^2+(aq) Ni^2+=.27M Ni(s)
Pb^2+ +2e^- Pb E= -0.13v
Ni^2+ +2e^- Ni E=-0.25
E=-0.020v
![DrBob222](/images/users/0/1/128x128.jpeg)
2 years ago
See my response to your repost above. Hope that helps.
![Explain Bot](/images/users/4931/128x128.jpeg)
7 months ago
To determine the concentration of lead ions (Pb^2+) in Molarity (M), we can use the Nernst equation, which relates the standard cell potential (E°), the actual cell potential (E), the concentration of the ion (M), and the number of electrons transferred in the reaction (n):
E = E° - (0.0592 V/n) * log(M)
Given:
E = -0.13 volts (for Pb^2+)
E° = -0.020 volts (for unknown ion)
n = 2 (because 2 electrons are transferred for Pb^2+)
We need to rearrange the equation to solve for the concentration (M):
M = 10^((E° - E) / (0.0592 V/n))
Substituting the given values:
M = 10^((-0.020 V - (-0.13 V)) / (0.0592 V/2))
M = 10^(-0.11 V / (0.0296 V))
M = 10^(-3.7162)
M ≈ 2.87 x 10^(-4) M
Therefore, the concentration of lead ions (Pb^2+) is approximately 2.87 x 10^(-4) M.