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NaOH + SO4

 
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rickgresham
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PostPosted: Mon Nov 02, 2009 10:00 am    Post subject: NaOH + SO4 Reply with quoteFind all posts by rickgresham

Does anyone know whether NaOH and SO4 will react and what the products would be?

Thanks.
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argentinechemistry
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PostPosted: Mon Nov 02, 2009 10:28 am    Post subject: Re: NaOH + SO4 Reply with quoteFind all posts by argentinechemistry

Yes. This is a neutralization process, where an acid and a base form a salt and water. I think you meant H2SO4 instead of SO4.
This reaction is produced at room temperature. At first you will get the acid salt and then it'll be produced the neutral salt by heating.You will see some bubbling. At that moment is when the reaction is carried out. Protons and hydroxide groups form the water:

(H+) + (OH)- -------- H2O
(Na+) + (HSO4)- ----- NaHSO4

Then you heat the solution. You'll notice more bubbling:
(H+) + (OH)- -------- H2O
(Na+) + (SO4)2- ----- NaSO4

So the complete and balanced ecuation is like this:

NaOH + H2SO4 -------- NaHSO4 + H2O

NaOH + NaHSO4 ------ Na2SO4 + H2O (by heating the previous reaction)

Or just making them react with temperature:

2 NaOH + H2SO4 ------ Na2SO4 + 2 H2O


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argentinechemistry
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PostPosted: Mon Nov 02, 2009 10:35 am    Post subject: Reply with quoteFind all posts by argentinechemistry

If you meant just SO4, you'll get H2O2 instead of water with 2 moles of caustic soda

2 NaOH + SO4 ------- Na2SO4 + H2O2
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PostPosted: Mon Nov 02, 2009 8:25 pm    Post subject: Reply with quoteFind all posts by expert

argentinechemistry is right: there is no such compound SO4. If it was, then it would probably generate H2O2.
Obviously it was a mistake. The task meant SO3 or OsO4
With both compounds NaOH will react very violently.
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rickgresham
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PostPosted: Mon Nov 02, 2009 8:58 pm    Post subject: Reply with quoteFind all posts by rickgresham

Isn't the anion sulfate SO4(2-)? http://en.wikipedia.org/wiki/Sulfate

I believe I read it's the second or third most prevalent ion in seawater. I have no formal chemistry training, so I'm not sure what I'm missing here.

Thanks,
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PostPosted: Tue Nov 03, 2009 12:35 am    Post subject: Reply with quoteFind all posts by expert

SO4(2-) and SO4 are two different things:
SO4(2-) is sulfate - anion (correct)
SO4 -hypotetical and not real molecule
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mr247
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PostPosted: Sun Nov 13, 2016 10:18 pm    Post subject: Reply with quoteFind all posts by mr247

I have a condition in which H2S oxidize to produce sulfate ion "SO4(2-)". Is this sulfate ion can react with NaOH to produce Na2SO4?
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PostPosted: Sun Nov 13, 2016 10:33 pm    Post subject: Reply with quoteFind all posts by expert

H2S may oxidize under certain conditions into H2SO4 sulfuric acid that can dissociate in aqueous solution to two protons H+ and SO4 (2-)
Sodium hydroxide also dissociates to Na+ and OH-

When acid and base such as NaOH mix, they will form salt and water
2NaOH + H2SO4 = Na2SO4 + 2H2O

You can write the same in ionic form, and it is the same reaction:

2Na(+) + 2OH(-) + 2H(+) + SO4(2-) = 2Na(+) + SO4(2-) + 2H2O
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mr247
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PostPosted: Mon Nov 14, 2016 2:42 am    Post subject: Reply with quoteFind all posts by mr247

Thanks for quick response. This is related to crude distillation unit. We have H2S in crude feed and we are injecting NaOH into the crude feed. There is problem in chocking of pump strainer. When analyze the plugging material found a Na2SO4. So trying to confirm if SO4(2-) ions can react with NaOH.
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What happen when sulfate ion (SO4(-2)) react with NaOH.
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PostPosted: Wed Nov 23, 2016 11:41 pm    Post subject: Reply with quoteFind all posts by expert

H2S reacts with NaOH producing Na2S

Both H2S and Na2S can oxidize, ultimately into Na2SO4. This salt is water soluble.

NaOH is also water soluble and ionizes NaOH ==> Na(+) + OH(-)
if SO4(2-) present, all ions will be in a free exchange. If water removed, Na2SO4 may crystallize. When water added, the crystals will dissolve and Na2SO4 will ionize to Na(+) and SO4(2-) again
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spadanco
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PostPosted: Mon Aug 21, 2017 5:25 am    Post subject: Re: NaOH + SO4 Reply with quoteFind all posts by spadanco

argentinechemistry wrote:
Yes. This is a neutralization process, where an acid and a base form a salt and water. I think you meant H2SO4 instead of SO4.
This reaction is produced at room temperature. At first you will get the acid salt and then it'll be produced the neutral salt by heating.You will see some bubbling. At that moment is when the reaction is carried out. Protons and hydroxide groups form the water:

(H+) + (OH)- -------- H2O
(Na+) + (HSO4)- ----- NaHSO4

Then you heat the solution. You'll notice more bubbling:
(H+) + (OH)- -------- H2O
(Na+) + (SO4)2- ----- NaSO4
Thanks for using the post

So the complete and balanced ecuation is like this:

NaOH + H2SO4 -------- NaHSO4 + H2O

NaOH + NaHSO4 ------ Na2SO4 + H2O (by heating the previous reaction)

Or just making them react with temperature:

2 NaOH + H2SO4 ------ Na2SO4 + 2 H2O


Argentine Chemistry
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