Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: bumblord1 on May 26, 2017, 11:17:35 PM
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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 :rarrow: 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?
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No such thing as Na2O3.
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Whoops, I'll fix that. It's Na2CO3.
The total reaction should be:
KClO3 + Na2CO3 :rarrow: K2CO3 + 2NaClO3
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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?
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Whoops, I'll fix that. It's Na2CO3.
The total reaction should be:
KClO3 + Na2CO3 :rarrow: 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?
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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?