please solve (b)

Assume that Cu2+(0.01M) and Sn2+(0.01M) are dissolved in an aqueous solution of pH=0.0. (a) Calculate the potential at which the plating of Cu and Sn can start when the potential of an inert electrode (Pt) is gradually changed from 1.6V (vs. NHE) to the negative values. Cu2++2e=CuSn2++2e=SnE0=0.34V(vs.NHE)E0=0.14V(vs.NHE) (b) When the potential of Pt electrode is swept from 1.6V to the negative value at pH=14, what happens in the order of Cu plating, Sn plating and H2 evolution? Describe the reason why the pH of aqueous solution should be kept high enough in the industrial plating process of Sn. Assume that Cu2+(0.01M) and Sn2+(0.01M) are dissolved in an aqueous solution of pH=0.0. (a) Calculate the potential at which the plating of Cu and Sn can start when the potential of an inert electrode (Pt) is gradually changed from 1.6V (vs. NHE) to the negative values. Cu2++2e=CuSn2++2e=SnE0=0.34V(vs.NHE)E0=0.14V(vs.NHE) (b) When the potential of Pt electrode is swept from 1.6V to the negative value at pH=14, what happens in the order of Cu plating, Sn plating and H2 evolution? Describe the reason why the pH of aqueous solution should be kept high enough in the industrial plating process of Sn