What initial concentration of Cd2+ is required to result in a cell potential of 0.200 V in a voltaic cell constructed by connecting a nickel electrode that is dipped into 1.00 M NiSO4 solution to a cadmium electrode that is dipped into a solution containing the Cd2+ ions?

Cd ==> Cd^2+ + 2e Eo = ?

Ni^2+ + 2e ==> Ni E =-0.25
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Cd + Ni^2+ ==> Cd^2+ + Ni Ecell=0.2

Look up the Eo value for Cd^2+ and reverse it. Look up the Eo value for Ni since the Eo value is the definition for 1 M solution. You want the total for Ecell to be 0.200 so
EoCd + EoNi^2+ = 0.200 or
x + Eo Ni^2+ = 0.200 and solve for x. Then plug that value into the Nernst equation and solve for (Cd^2+). Post your work if you get stuck.

To determine the initial concentration of Cd2+ required for a cell potential of 0.200 V in a voltaic cell, we can use the Nernst equation. The Nernst equation relates the cell potential (Ecell) to the concentrations of the species involved in the redox reaction.

The Nernst equation is given by:
Ecell = E°cell - (0.0592/n) * log(Q)

Where:
- Ecell is the cell potential
- E°cell is the standard cell potential (at standard conditions)
- Q is the reaction quotient, which is calculated using the concentrations of the species involved in the redox reaction
- n is the number of moles of electrons transferred in the balanced redox reaction
- 0.0592 is the value of the natural logarithm base (ln) divided by the number of moles of electrons transferred

In this case, the balanced redox reaction involved in the voltaic cell can be represented as:

Cd2+ + 2e- → Cd(s)

The number of moles of electrons transferred (n) in this reaction is 2.

Now, let's determine the standard cell potential (E°cell) by referring to standard reduction potential values. The standard reduction potential for the nickel electrode (Ni2+ + 2e- → Ni) is -0.250 V. However, since the reduction potential is given as reduction, we need to flip the sign to represent it according to the oxidation reaction of cadmium. Therefore, the standard cell potential is 0.250 V.

Substituting the values into the Nernst equation:

0.200 V = 0.250 V - (0.0592/2) * log(Q)

Now, we need to rearrange the equation to solve for Q, the reaction quotient:

Q = 10^[(E°cell - Ecell) / (0.0592/n)]

Substituting the given values:

Q = 10^[(0.250 V - 0.200 V) / (0.0592/2)]
= 10^[(0.050 V) / (0.0296)]
= 10^(1.689189189)

Calculate the reaction quotient (Q):

Q ≈ 43.5409

Now, we have the reaction quotient (Q), which is equivalent to the ratio of the concentrations of products to reactants. In this case, since the Cd2+ is a reactant, Q is the concentration of Cd2+. Thus, the initial concentration of Cd2+ required for a cell potential of 0.200 V is approximately 43.5409.