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Topic: Oxidizing Chlorides  (Read 3855 times)

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Offline shalikadm

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Oxidizing Chlorides
« on: February 07, 2013, 12:02:30 AM »
A book states like this:
CO3-,MnO4-.CrO42-,Cr2O742-,HNO3,ClO3-,ClO4- can oxidize Cl- to Cl2.

I have this questions in my mind:
  • I haven't read about this CO3- thing anywhere.I think it's a printing mistake..Am I correct ?
    What will be the most suitable correct one for this ?
  • Do we have to use HCl ? Can't we use something like KCl instead ..both have Cl-,isn't it?
  • Can we use KClO4 instead of HClO4?...As in KMnO4...I feel that though HNO3 do the thing,but KNO3 doesn't.
Someone please explain these things to me..thanks !

Offline Borek

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Re: Oxidizing Chlorides
« Reply #1 on: February 07, 2013, 04:38:43 AM »
No idea about this CO3- thing. Perhaps they meant half of the peroxodicarbonate.

Oxyacids are more effective as oxidizing agents in low pH, so you want H+ to be there.
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Offline shalikadm

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Re: Oxidizing Chlorides
« Reply #2 on: February 07, 2013, 07:08:22 PM »
My second thought,
I think that we can't use an oxidizing agent if we want cl2 from KCl...we need the stronger oxidizing method, electrolysis to get Cl2 out of the salt...but we can use an oxidizing agent with HCl to gain Cl2..Am I correct ?
Thanks !

Offline shalikadm

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Re: Oxidizing Chlorides
« Reply #3 on: February 08, 2013, 08:48:37 AM »
My second thought,
I think that we can't use an oxidizing agent if we want cl2 from KCl...we need the stronger oxidizing method, electrolysis to get Cl2 out of the salt...but we can use an oxidizing agent with HCl to gain Cl2..Am I correct ?
Thanks !
Sorry for my above post....molten KCl was in mind....
Just take an aqueous solution of K+Cl -...Can we yield Cl2 using one of the oxidizers mentioned above ?
Another one....Let's think I have an aqueous solution of FeCl2...Do we yield Cl2 and Fe3+,when oxidized ?

Offline shalikadm

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Re: Oxidizing Chlorides
« Reply #4 on: February 13, 2013, 06:57:59 AM »
any idea ?

Offline ajkoer

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Re: Oxidizing Chlorides
« Reply #5 on: February 26, 2013, 11:35:41 PM »
Here is a possible example of a carbonate in a two step reaction resulting in the oxidation of HCl to Cl2:

(H2CO3 + NaOCl) + HCl -->  (NaHCO3 + HOCl) + HCl --> NaHCO3 + H2O + Cl2 --> NaCl + H2O + CO2 + HOCl....

The action of Carbonic acid on NaOCl is slow forming Hypochlorous acid. In the presence of HCl:

 HCl + HOCl <---> Cl2 + H2O

It is actually a path to form Hpochlorous acid to place Sodium carbonate or hydrogen carbonate (or the Metal hydroxide or the Metal oxide) in Chlorine water, thereby neutralizing the highly ionic HCl and leaving HOCl.
 
« Last Edit: February 27, 2013, 12:04:51 AM by ajkoer »

Offline Borek

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Re: Oxidizing Chlorides
« Reply #6 on: February 27, 2013, 03:39:56 AM »
I would not say it is oxidation with carbonic acid - it is oxidation with hypochloric acid.
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Offline 408

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Re: Oxidizing Chlorides
« Reply #7 on: February 27, 2013, 07:14:55 AM »

  • Do we have to use HCl ? Can't we use something like KCl instead ..both have Cl-,isn't it?
  • Can we use KClO4 instead of HClO4?...As in KMnO4...I feel that though HNO3 do the thing,but KNO3 doesn't.



Aqueous perchlorate is a shitty oxidizing agent.  it will not oxidize chloride to chlorine.

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