Chemistry Question

[Jack Ruby]

I was at work tonight.

When ever I am at work I have a lot of time to think(my job is very easy and boring). It just so happens that a lot of my thinking is about this type of thing. Anyways to the point.

I was wondering if you good creat NaClO3 in the following Manner and then if you wished you could convert it to KClO3.
Common house hold bleach is roughly 6-7% solution of NaHClO.

Now I have come to the theory that I cam make this into NaClO3 as Follows.

2 H2O2(aq) + 2 NaHClO(aq) ---------> 4 NaClO3(aq) + 6 H2(g)

i have not tested this but would like to know if there is some reason it wouldn't work before I try?

This is Directed more to Mega and other with a Chemistry BACKGROUND.

[Pu239 Stuchtiger]

"Common household bleach" is sodium hypochlorite, NaOCl.

[a_bab]

...and it won't work because bleach is a much powerful oxidant then hidrogen peroxide.

[Mr Cool]

And you won't get hydrogen gas being made, since if formed it'd start as atomic hydrogen, which is very reactive. It'd probably reduce the NaHClO (or NaClO) to NaCl and H2O, and it would probably also reduce NaClO3.

(Also you should double-check when balancing equations...)

<small>[ March 28, 2002, 07:42 AM: Message edited by: Mr Cool ]</small>

[megalomania]

Actually you get H₂O₂ + NaClO --> NaCl + H₂O + O₂

Nice try though, the formation of a more complex substance like sodium chlorate will require more finesse than mixing stuff together :)

[a_bab]

But at least when you'll need table-salt, you'll know what to do :rolleyes:

[vulture]

Another process of making NaClO3 would be bubbling Cl2 gas through a hot NaOH solution. This method has some practical problems though, for example the toxicity and the low solubility of chlorine gas in the solution.

What you could try is adding ammoniumpersulfate to bleach. Ammoniumpersulfate is normally used to etch printed electronic surfaces IIRC.

BTW, what's the code for subscript?

[Jack Ruby]

Well Crap...

I had my hopes up and everything. Good thing I asked.

Thank you for you help

[vulture]

Isn't permanganate a stronger oxidizer then hypochlorite or chlorate?
If this is true one could try oxidizing it in an acidic environment.
(NOT with H2SO4 -> Mn2O7 formation!)

Hypochlorite to chlorate conversion:
3NaClO + 4KMnO4 + 4HCl -> 3NaClO3 + 4MnO2 + 2H2O + 4KCl

chlorate to perchlorate conversion:
3KClO3 + 2KMnO4 + 2HCl -> 3KClO4 + 2MnO2 + H2O + 2KCl

Only problem is you've got a lot of byproducts....

<small>[ April 03, 2002, 04:17 AM: Message edited by: vulture ]</small>

[stanfield]

want some NaClO3 ? go to France, here you can buy a 10 kg of NaClO3 with 99+ purity for 15$.

see ya !

[Neosanity015]

I have a chemistry question.>
Can someone tell me how I can find out the number of moles of solute
in a solution using the percentage by weight? I am trying to use a
balanced equation for making HMTD and Acetone Peroxide. I need to
find how many moles of HCl are in a 31.45% solution and how many
moles of H2O2 in the 6% solution. Any help is greatly appreciated.
Thanks.

~Neosanity

[kingspaz]

ok,
relative molecular mass of H2O2 = 1+1+16+16 = 34g
for say 100ml of 6% solution,
6/100*34=2.04g of H2O2 in 100ml of 6% solution.
number of moles = 2.04/34 = 0.06mol
i'm tired so that could be wrong!

[Jhonbus]

That's right as long as the H₂O₂ solution is 6% w/v. But it could be w/w or v/v, which would change the numbers slightly, or a lot, depending on the density of H₂O₂ compared to water.

<small>[ April 23, 2002, 08:37 PM: Message edited by: Jhonbus ]</small>

[vulture]

I get so sick of the various ways of indicating peroxide concentration, why can't they just put the volume, mass percentage and density on the container??

[Pu239 Stuchtiger]

Vulture, for your above hypothesis: I would try using HMnO4 instead of KMnO4; far cleaner process.