Electrolysis of Aqueous nickel fluoride

Question

In an electrolytic cell containing a solution of Nickel (II) fluoride, what would be the anode and cathode reactions that take place? Here is what I came up with:

Anode: The fluoride will get oxidized instead of OH-

2F- + 2e ➡️ F2 (g)

Cathode:

2H+ + 2e ➡️ H2 (g)

1. For the cathode reaction, I have found some websites that say the nickel is the one that gets reduced instead of H+. My question is why would that be since I thought only a metal is produced at the cathode only if it is less reactive than hydrogen, which in this case nickel is not. Thanks!

Answer 1

Half Reaction E^ored(V)

F2 + 2 e– →2 F– +2.87

Ni2+ + 2 e– →Ni –0.25

Reduction of H from +1 to 0 in water

2 H2O + 2 e– →H2 + 2 OH– –0.83

The reaction you wrote for the cathode, 2H+ + 2e→ H2 (g), isn't really the one associated with water directly. Between the Ni and H2O reactions I put above, the Ni2+ one will require less voltage to cause it to occur