[bumblord1]

Hello, all! I am doing a chemistry project, and I need some help figuring out this reaction.

I will be preforming electrolysis with my reactants in water. They are KClO₃ and Na₂O₃. I'm going to use lead strips to connected to my anode/cathode cords.

Why will precipitate form, and what is the reaction? My guess is that there's some sort of redox involved, but I don't exactly know where and how. Does the lead react to the equation?

Here is my guess:

KClO₃ + Na₂O₃  K₂CO₃ + 2NaClO₃

Judging by research, I think the precipitate will form on the anode side, but I'm not entirely sure why. Can someone please explain?

[Borek]

No such thing as Na₂O₃.

[bumblord1]

Whoops, I'll fix that. It's Na₂CO₃.

The total reaction should be:

KClO₃ + Na₂CO₃  K₂CO₃ + 2NaClO₃

[Enthalpy]

K₂CO₃ is very soluble in water, quite more than Na₂CO₃.
NaClO₃ too is much more soluble in water than KClO₃.
Does something else happen by electrolysis?

[Arkcon]

Whoops, I'll fix that. It's Na₂CO₃.

The total reaction should be:

KClO₃ + Na₂CO₃  K₂CO₃ + 2NaClO₃

There are a number of problems, and you have to clarify what you mean, so we can help.

You have to balance the equation.  That's a trivial point, but don't neglect it.

As was mentioned, all products and reactants are soluble.  As such, there should be no precipitate, and also no reaction just by mixing in water.

I don't understand the electrolysis.  You want a re-dox, and you may get one with electrolysis.  You can get one with each reactant and product alone, or water alone (neutral salt for conductivity needed, but still).  You can certainly get a reaction with lead strips during electrolysis, again, with each reactant and product alone or with plain water.  So what are you trying to do?

[Enthalpy]

Potassium perchlorate is less soluble in water, and electrolysis (but I ignore the conditions!) is one way to obtain perchlorate from chlorate. Could this happen here?