How can you determine the solubility product (Ksp) using standard cell potential?

The solubility product constant (Ksp) can be determined using standard cell potential by referencing the reduction potentials of the involved equilibrium reactions. In electrochemistry, the standard cell potential provides insight into the Gibbs free energy change for a reaction.

When you have a saturated solution of a sparingly soluble salt, its dissolution can be represented as an electrochemical reaction. The relationship between the cell potential and the solubility product can be expressed using the Nernst equation and the Gibbs free energy equation. The Ksp can be directly related to the standard cell potential (E°) of the half-reactions involved. By knowing the reduction potentials, one can derive the Ksp by setting the change in Gibbs free energy (ΔG) to the expression involving cell potential (ΔG = -nFE°), where n is the number of moles of electrons transferred and F is Faraday's constant.

Thus, understanding the reduction potentials allows chemists to connect electrochemical measurements to solubility principles, making option B the correct choice for determining Ksp.