Pale blue species forming during electrolysis of NaHCO3

Question

I have a solution of 3500 ml $\ce{H2O}$ + 454 g $\ce{NaHCO3}$ in electrolysis at a potential of 12.5V using a lead anode and copper cathode. The surface areas aren't measured but they are enormous. I made the electrodes myself from lead and copper foil.

The idea was to make NaOH from $\ce{NaHCO3}$ (an inexpensive source $\ce{NaHCO3}$ $$0.86/454g and NaOH $7/500g) meanwhile producing the PbO₂ layer on the lead anode.

Everything seemed to be going as expected until I see there's a pale blue species being produced. What could it be? I'm thinking H₂O₂, water having the potential to completely become peroxide, so I used the 5V output instead and the blue species vanished.

I've read electrolysis of salts in basic solution usually result in the salt reaching its highest state of oxidation at the anode.

Eg.:

$\ce{NaCl + H2O ->Cl- + OH- -> HClO + OH- ->ClO2- + H2}$ eventually becoming $\ce{ClO4-}$

(correct me if I'm wrong but I believe that's the way that reaction carries out),

or

$\ce{(NH4)2SO4 -> (NH4)2S2O8}$

EDIT It's just copper. Apparently in a solution of NaOH, there is some oxidation of a Cu cathode. I've seen it occur many times afterward. Hydrogen peroxide cannot be made without special laboratory equipment.

Answer 1

The blue color was caused by copper being stripped from the wire. btw, when your hair turns orange, it is because it is being stripped of color, among other other things (chemical bonds), which will cause it to be brittle and also absorb any hair dye to the extreme that it feels waxy...I'd suggest you cut off a piece of hair for a test before dunking your whole head in bleach (chlorine will turn it greenish).

P.S. Use nitric acid to dissolve Cu.