Sodium Hydrogen Sulfate

[Psionicdragon]

Hi everyone,

Can this be used as an acid bath for removing layers of live rocks?

[HighlandReefer]

It will reduce the pH low enough to dissolve the rock surfaces, so I assume it will work for you.

[disc1]

NaHS is a base.

Correction it's amphoteric.

[HighlandReefer]

Not an acid, then it will not work for this purpose I assume. :)

[HighlandReefer]

This through me off: ;)
http://en.wikipedia.org/wiki/Sodium_bisulfate


Sodium bisulfateFrom Wikipedia, the free encyclopediaJump to: navigation, search
Sodium bisulfate


IUPAC name[hide]Sodium hydrogen sulfate
Other names[hide]Sodium acid sulfate
Bisulfate of soda

Sodium bisulfate, also known as sodium hydrogen sulfate (NaHSO4), is an acid salt. It is a dry granular product that can be safely shipped and stored. The anhydrous form is hygroscopic. Solutions of sodium bisulfate are acidic, with a 1M solution having a pH of < 1.

One production method involves mixing stoichiometric quantities of sodium hydroxide and sulfuric acid which react to form sodium bisulfate and water.

NaOH + H2SO4 → NaHSO4 + H2O
A second production method involves reacting sodium chloride (salt) and sulfuric acid at elevated temperatures to produce sodium bisulfate and hydrogen chloride gas.

NaCl + H2SO4 → NaHSO4 + HCl
The liquid sodium bisulfate is sprayed and cooled so that it forms a solid bead. The hydrogen chloride gas is dissolved in water to produce hydrochloric acid as a useful coproduct of the reaction.

There are only two producers in the USA: Jones-Hamilton Co. uses the sulfuric acid/sodium chloride process, which produces the anhydrous form. Jost Chemical uses the sodium hydroxide/sulfuric acid method, which produces the monohydrate.

[disc1]

No, I got thrown off. I read hydrosulfide. NaHS. I don't know how I read that wrong.

Sodium hydrogensulfate NaHSO4 is also amphoteric, but the second Ka is much much lower than the one I thought was said.

I would still think a stronger acid may be in order to take off a layer of rock, but if you just want to take a little little bit of rock, then somehing like HSO4- might work.

[disc1]

Really, I don't know what I'm thinking. Who in their right mind would want to smell rotten egg while they cleaned their rock?

And who has access to NaHS?


I need some 1,3,7-trimethyl-xanthine this morning.

[disc1]

Fix my double post with a pic...

http://www.erowid.org/chemicals/caffeine/images/archive/caffeine_3d.jpg

[HighlandReefer]

HCL is your choice I assume? Muriatic Acid is around 33% HCL which is what is normally recommended for this purpose. :)

[HighlandReefer]

Really, I don't know what I'm thinking. Who in their right mind would want to smell rotten egg while they cleaned their rock?

And who has access to NaHS?


I need some 1,3,7-trimethyl-xanthine this morning.

:lol:

I've done this many a morning before enough coffee. ;)

[disc1]

Actually, now that I got my eyes open, the HSO4- would probably get it done. Think of it as half neutralized sulfuric acid. PKa1 for that molecule is below zero. You will never put a proton on the naked oxygen. This can't act as a base. pKa 2 is right at 2 I think. So you've got a really strong acid there.

Technically, if you wanted to get crazy and keep stirring all day, I think you can get quite a lot of NaHSO4 in solution and make a really strong acid.

[Psionicdragon]

haha, honestly, i would not like to smell rotten eggs while I do this. However, I was half asleep when I order the acid and didn't read the ingredient.

I was trying to order HCL, but ordered "Dry Acid".

[disc1]

This half asleep thing seems to be rampant in this thread.

:lol2:

[Psionicdragon]

This half asleep thing seems to be rampant in this thread.

:lol2:

haha, yes it is :P

One more question, can this be used to recharge DI resins?

[disc1]

One more question, can this be used to recharge DI resins?

That probably not. You don't want all those sodium ions in there for recharging DI.

[Psionicdragon]

aw :(

Thanks David and HIghland, for your help.