November 24, 2024, 07:51:09 PM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1] 2 3   Go Down

Topic: NaCl electrolosys  (Read 27466 times)

0 Members and 1 Guest are viewing this topic.

Mr. Pink

  • Guest
NaCl electrolosys
« on: March 31, 2005, 12:54:25 AM »
Hey, im wondering, what are the basics in the electrolosys for table salt? how is the sodium and chlorine collected? how do i prevent the Na from igniting? if you have to melt the NaCl to electrolize it, then if i cant use a Pt electrode, what should i use?
Logged

Offline Mitch

  • General Chemist
  • Administrator
  • Sr. Member
  • *
  • Posts: 5298
  • Mole Snacks: +376/-3
  • Gender: Male
  • "I bring you peace." -Mr. Burns
    • Chemistry Blog
Re:NaCl electrolosys
« Reply #1 on: March 31, 2005, 03:29:58 AM »
"refined" graphite electrodes work fine. You can buy them on ebay.
« Last Edit: March 31, 2005, 03:31:39 AM by Mitch »
Logged
Most Common Suggestions I Make on the Forums.
1. Start by writing a balanced chemical equation.
2. Don't confuse thermodynamic stability with chemical reactivity.
3. Forum Supports LaTex

Offline jdurg

  • Banninator
  • Retired Staff
  • Sr. Member
  • *
  • Posts: 1366
  • Mole Snacks: +106/-23
  • Gender: Male
  • I am NOT a freak.
Re:NaCl electrolosys
« Reply #2 on: March 31, 2005, 03:36:02 PM »
Do a quick search on google for the 'Down's Cell'.  There are plenty of sites which have very detailed explanations and diagrams of how molten sodium chloride is separated into sodium metal and chlorine gas.
Logged
"A real fart is beefy, has a density greater than or equal to the air surrounding it, consists

Offline Mitch

  • General Chemist
  • Administrator
  • Sr. Member
  • *
  • Posts: 5298
  • Mole Snacks: +376/-3
  • Gender: Male
  • "I bring you peace." -Mr. Burns
    • Chemistry Blog
Re:NaCl electrolosys
« Reply #3 on: March 31, 2005, 04:59:25 PM »
Then my opinion always is, "If you can't even spell electrolysis, you probably shouldn't do one." ;)
Logged
Most Common Suggestions I Make on the Forums.
1. Start by writing a balanced chemical equation.
2. Don't confuse thermodynamic stability with chemical reactivity.
3. Forum Supports LaTex

Offline eugenedakin

  • Oilfield Consulting Chemist
  • Retired Staff
  • Full Member
  • *
  • Posts: 658
  • Mole Snacks: +88/-2
  • Gender: Male
  • My desk agrees with the law of entropy
    • Personal Website
Re:NaCl electrolosys
« Reply #4 on: March 31, 2005, 08:26:33 PM »
Hello Mr. Pink,

When electrolysis is performed on an industrial scale, it is performed in a Chlor-Alkali plant.  Salt (as NaCl) is dissolved into water until it is saturated.  Then the salt-saturated-water is placed into a vessel with two electrodes (negatively charged, and positive charges).  The NaCl molecule separates to form Caustic Soda (Sodium Hydroxide) at one electrode and forms Chlorine gas at the other electrode.

Chlorine gas (very poisonous) is collected at one end, and sodium hydroxide is removed at the other end.

I hope this helps,

Eugene
Logged
There are 10 kinds of people in this world: Those who understand binary, and those that do not.

Mr. Pink

  • Guest
Re:NaCl electrolosys
« Reply #5 on: March 31, 2005, 08:52:12 PM »
Quote from: Mitch on March 31, 2005, 04:59:25 PM
Then my opinion always is, "If you can't even spell electrolysis, you probably shouldn't do one." ;)

Well, I never get good grades in Language Arts. But my dad is a jeweler and he does electroplating and electrolysis on a regular basis. He also has his bachelor's in Chemistry so I've learned a lot from him.

« Last Edit: March 31, 2005, 10:51:40 PM by Mr. Pink »
Logged

Mr. Pink

  • Guest
Re:NaCl electrolosys
« Reply #6 on: March 31, 2005, 08:55:20 PM »
Quote from: eugenedakin on March 31, 2005, 08:26:33 PM

Chlorine gas (very poisonous) is collected at one end,


Don't worry, i know whats safe and whats not. Anyone who doesnt know that chlorine is poisonous (i dont think i spelt that right either, or the word "either") shouldn't be in chemistry or even a WWI historian.
Logged

Offline jdurg

  • Banninator
  • Retired Staff
  • Sr. Member
  • *
  • Posts: 1366
  • Mole Snacks: +106/-23
  • Gender: Male
  • I am NOT a freak.
Re:NaCl electrolosys
« Reply #7 on: April 01, 2005, 11:56:19 AM »
Also, you absolutely cannot obtain sodium metal from the electrolysis of aqueous NaCl.
Logged
"A real fart is beefy, has a density greater than or equal to the air surrounding it, consists

Mr. Pink

  • Guest
Re:NaCl electrolosys
« Reply #8 on: April 01, 2005, 02:21:15 PM »
Quote from: jdurg on April 01, 2005, 11:56:19 AM
Also, you absolutely cannot obtain sodium metal from the electrolysis of aqueous NaCl.

Ah, thank you, thats what i wanted to know.
Logged

Viper3k

  • Guest
Re:NaCl electrolosys
« Reply #9 on: April 01, 2005, 10:46:37 PM »
I did this exact electrolysis on aqueous NaCl.

The gases were released and after a few hours there was a brown sediment forming and a sort of greeny layer on top. I have no idea what they were.
Also, could you use carbon rods taken from alkaline batteries for electrodes?
Logged

Offline Mitch

  • General Chemist
  • Administrator
  • Sr. Member
  • *
  • Posts: 5298
  • Mole Snacks: +376/-3
  • Gender: Male
  • "I bring you peace." -Mr. Burns
    • Chemistry Blog
Re:NaCl electrolosys
« Reply #10 on: April 01, 2005, 11:25:02 PM »
don't know.
Logged
Most Common Suggestions I Make on the Forums.
1. Start by writing a balanced chemical equation.
2. Don't confuse thermodynamic stability with chemical reactivity.
3. Forum Supports LaTex

Mr. Pink

  • Guest
Re:NaCl electrolosys
« Reply #11 on: April 04, 2005, 06:50:56 PM »
::Edit:: The synthesis of explosives is not appropriate material here.

Well, i wasnt planning on using it as an explosive; my personal objective is to collect all (or at least the more common) of the elements in thier pure form. Do you think that i would be responsible enuf to put the detailed warnings at the bottom, but not responsible enough to keep the sodium from exploding?
« Last Edit: April 06, 2005, 07:12:50 PM by Mr. Pink »
Logged

Garneck

  • Guest
Re:NaCl electrolosys
« Reply #12 on: April 09, 2005, 06:15:35 PM »
Quote from: jdurg on April 01, 2005, 11:56:19 AM
Also, you absolutely cannot obtain sodium metal from the electrolysis of aqueous NaCl.

Of course, you can only get hydrogen.

But, hmmm, what about if you use a mercury electrode? I always thought you can get NaOH during that.. correct me if I'm wrong.
Logged

Offline Mitch

  • General Chemist
  • Administrator
  • Sr. Member
  • *
  • Posts: 5298
  • Mole Snacks: +376/-3
  • Gender: Male
  • "I bring you peace." -Mr. Burns
    • Chemistry Blog
Re:NaCl electrolosys
« Reply #13 on: April 09, 2005, 07:32:40 PM »
Quote
Do you think that i would be responsible enuf to put the detailed warnings at the bottom, but not responsible enough to keep the sodium from exploding?

Spelling and grammar aside, that's not the point.
Logged
Most Common Suggestions I Make on the Forums.
1. Start by writing a balanced chemical equation.
2. Don't confuse thermodynamic stability with chemical reactivity.
3. Forum Supports LaTex

lordofdarkness

  • Guest
Re:NaCl electrolosys
« Reply #14 on: June 22, 2005, 05:47:54 AM »
Helloz
I done this b4
I was successful
I made my own downcell and melted salt using and oxy acetyline welders flame
I got enough sodium 2 make fireworks!!!!!
Logged
Pages: [1] 2 3   Go Up
« previous next »
Sponsored Links