Consider the Voltaic Cell Based on the Following Reaction: Zn(s) $\to$

Consider the voltaic cell based on the following reaction: Zn(s) + Ni²⁺(aq) $\to$ Zn²⁺(aq) + Ni(s)
Two students are assigned to measure the standard cell potential at 25°C.Student one claims that both solutions of ions have to be at exactly 1.00 M concentration,but student two is sure that the measurement will be the same if the concentrations of the two solutions are equal,but not necessarily 1.00 M.What do you think?

A) Student one is right because,by definition,standard cell potentials must be measured at concentrations of 1.00 M.
B) Student one is right because she understands the Nernst equation and what it describes.
C) Student two is right because she understands the Nernst equation and what it describes.
D) Student two is right because cell potentials do not depend on the concentration.
E) Both are right because cell potentials do not depend on the concentration.