Chemgineer
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Calcium Sulphate Destroys Glassware
Recently i've been doing a dry distillation of Calcium Nitrate with Sodium Bisulfate. It is a really convenient procedure to produce Ntric Acid
(without any foaming) and also the resulting Calcium Sulfate does dissolve and come out of the flask at the end.
The problem I have is that the Calcium Sulphate seems to be adhering to my flasks and literally pulling borosilicate glass off the surface, then the
next time I use that flask it ends up broken or cracked.
I am using Indian Supertek 500ml round bottom flasks in a heating mantle, am I suffering from poor glassware or just punishing it too much?
[Edited on 28-9-2021 by Chemgineer]
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MidLifeChemist
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I have heard of others being similarly punished by their calcium sulfate deposits. You are not alone. Still, if nitric acid is expensive and flasks
are cheap where you live, then it might be worth it 
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Chemgineer
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I might just add some water next time and accept a lower concentration.
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macckone
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Anecdotal:
Try adding some 90+% sulfuric acid, it seems to protect the glass.
I originally tried it to help dissolve the mix and reduce the amount of water carried over from non-anhydrous salts.
It seems to reduce the water and improve the reaction but I haven't done a quantitative study.
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Chemgineer
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Something else I considered was adding a percentage of Potassium Nitrate, as that reaction with Sodium Bisulfate causes foaming, the foam might help.
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Tsjerk
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I think you heated the flask too much. I never distilled nitric acid from this mix, but when I did I never tried to pull the last bit.
Or it might have been the real anhydrous non-liquid combination between calcium sulfate and glass. I went with a percent of water and a second
distillation from sulfuric acid anyway to get rid of the NO2. Although I don't know how a bit of water would have helped with CaSO4 as a drying agent
in there
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Chemgineer
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I've done this with Potassium Nitrate and Sodium Bisulfate before several times using the same make of flask and no damage, I probably have kept the
reaction going for longer with the Calcium Nitrate.. maybe it's because the calcium sulfate ends up drier than the mix of Sodium Sulfate and
Potassium Sulfate and there is less heat sink for the glass which gets hotter. But to me it looks like the Calcium Sulfate has adhered to the glass
surface and then retracted on cooling putting a layer with it.
[Edited on 28-9-2021 by Chemgineer]
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Chemgineer
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As in the photo there is a general dull area with an excavation of glass top right and then two cracks around the outside of the affected area.
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Chemetix
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What you are experiencing is ion exchange in the glass. Strong concentrated solutions that have different ionic composition to glass will cause some
surface ions to migrate.
Osmotic potential is the force behind the exchange. Sodium ions will want to move into the aqueous solution and calcium will try to move into the
glass. Calcium makes the glass brittle. It becomes a glass with different coefficient of thermal expansion to the rest of the flask and so heating and
cooling will cause stress at the boundaries where ion exchange has most strongly occurred.
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Chemgineer
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Hey thanks, what you say makes allot of sense and I expect you are correct. I suppose the good thing is the heating is applied gradually by the
mantle and failure only seems to only occur on cooling when the calcium sulfate is a solid mass and can't spill from the flask.
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Amos
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Does calcium sulfate not readily precipitate when you combine the two reagents? If it does, there's no reason to leave it in the flask while you
distill; vacuum filter it first and distill the filtrate. If you lack vacuum filtration capabilities, I would add more water as you mentioned and
still manually gravity filter. You won't distill the last bits of nitric acid out of the mixture until the dissolved salt content has nearly reached
saturation, and this will be the most concentrated distillate of the entire process.
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Texium
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He said he’s doing it as a dry distillation, which would seem to be a horribly inefficient and potentially dangerous method, but oh well. So
currently he’s not adding any water at all, just heating the solid mixture in a flask.
@Chemgineer: What sort of yields do you get with this dry distillation? If “foaming” is really such an insurmountable issue with the aqueous
procedure, I would suggest investing in a larger boiling flask… Also, could you please stop Capitalizing Your Chemical Names? They are not proper
nouns, and writing them that way just looks pretentious.
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Metallophile
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I have made this mistake before. I think it's actually kinda strange that elements are not proper nouns, even the ones named after people! But that's
the rule, so I try to follow it.
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Chemgineer
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Quote: Originally posted by Texium  | He said he’s doing it as a dry distillation, which would seem to be a horribly inefficient and potentially dangerous method, but oh well. So
currently he’s not adding any water at all, just heating the solid mixture in a flask.
@Chemgineer: What sort of yields do you get with this dry distillation? If “foaming” is really such an insurmountable issue with the aqueous
procedure, I would suggest investing in a larger boiling flask… Also, could you please stop Capitalizing Your Chemical Names? They are not proper
nouns, and writing them that way just looks pretentious. |
I use 160g sodium bisulfate and 100g of calcium nitrate and I typically get around 50ml of RFNA.
# Edited to remove my capital letters!
[Edited on 29-9-2021 by Chemgineer]
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Fulmen
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What's the temperature? With thoroughly dried chems I would guess you would need to melt the bisulphate (315°C). There are nitrate eutectics that
melt at much lower temperatures, might be worth a shot.
KNO3 NaNO3 Ca(NO3)2 MP
24.............................76...........142
.................31............69...........142
26.............................74...........145
65............................ 35...........150
46.............24............30...........160
20.............................80...........162
.................19............81...........214
.................14............86...........214
40.............60...........................222
We're not banging rocks together here. We know how to put a man back together.
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Texium
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That would
be about a 98% yield based on calcium nitrate, if we assumed that what you collect is 100% nitric acid, but since RFNA contains additional dissolved
NO2, that amount wouldn’t even be possible to obtain from that amount of reagents… Are you sure you’re using anhydrous calcium nitrate? If not,
you likely aren’t getting true RFNA.
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Chemgineer
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| Quote: Originally posted by Texium | | That would
be about a 98% yield based on calcium nitrate, if we assumed that what you collect is 100% nitric acid, but since RFNA contains additional dissolved
NO2, that amount wouldn’t even be possible to obtain from that amount of reagents… Are you sure you’re using anhydrous calcium nitrate? If not,
you likely aren’t getting true RFNA. |
Not fully anhydrous no, this probably helps keep the temperatures lower, the product does fume though when opening a closed bottle.
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Chemgineer
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Ok i've just measured the specific gravity with a measuring cylinder and scales, the HNO3 from calcium nitrate seems to be 1.41 sg @ 18 deg C which
would make it 68%..... so azeotropic.
My previous HNO3 from a similar dry process with potassium nitrate and sodium bisulfate comes in at 1.46 sg @18 deg C which would make it 81%.
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rockyit98
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you doing it wrong. you need to add H2SO4 to concentrated Solution of Ca(NO3) slowly while mixing. CaSO4 will precipitate out. remove them and distill
the dilute solution till azeotropic forms.
"A mind is a terrible thing to lose"-Meisner
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Amos
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| Quote: Originally posted by rockyit98 | | you doing it wrong. you need to add H2SO4 to concentrated Solution of Ca(NO3) slowly while mixing. CaSO4 will precipitate out. remove them and distill
the dilute solution till azeotropic forms. |
It should be very obvious that sulfuric acid isn't easy to come by for the OP, or they wouldn't be attempting to make nitric acid this way.
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clearly_not_atara
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If you want to do a dry distillation, you can probably protect your glassware by using a eutectic mixture of sodium and potassium bisulfate instead of
just one or the other.
Eutectic (44% KHSO4 by moles; 50% by mass): 133 C [1]
NaHSO4: 315 C [2]
KHSO4: 197 C [2]
1:
https://www.researchgate.net/publication/230557353_Conductiv...
2: Wikipedia
[Edited on 04-20-1969 by clearly_not_atara]
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Amos
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| Quote: Originally posted by clearly_not_atara | If you want to do a dry distillation, you can probably protect your glassware by using a eutectic mixture of sodium and potassium bisulfate instead of
just one or the other.
Eutectic (44% KHSO4 by moles; 50% by mass): 133 C [1]
NaHSO4: 315 C [2]
KHSO4: 197 C [2]
|
If the reaction is successful though, bisulfates will still end up as solid sulfates
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Fantasma4500
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i had some distillation mixture of H2SO4 and CaSO4 standing around
i dumped it into a plastic bottle to be situated next to my toilet, to help remove calcium deposits every now and then
about a year later i found the bottle again
and there was about a fist-sized chunk of crystals in there
i eventually found out it was CaSO4 crystals
https://gyazo.com/74e95b60263131dfad29986ace145977
now what i understand is that i hit a particular H2SO4 concentration in which CaSO4 is soluble in
and upon diluting this further, it precipitated out the CaSO4, very slowly
so there must be maybe 10-20% "sweetspot" with H2SO4/H2O concentration in which CaSO4 is soluble.
so that might work for ya.
i would say maybe 20% or even less is where the CaSO4 dissolve- its only a vague guess
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Chemgineer
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| Quote: Originally posted by Chemetix | What you are experiencing is ion exchange in the glass. Strong concentrated solutions that have different ionic composition to glass will cause some
surface ions to migrate.
Osmotic potential is the force behind the exchange. Sodium ions will want to move into the aqueous solution and calcium will try to move into the
glass. Calcium makes the glass brittle. It becomes a glass with different coefficient of thermal expansion to the rest of the flask and so heating and
cooling will cause stress at the boundaries where ion exchange has most strongly occurred. |
I am wondering if the quality of the glass might have a bearing on this issue, the flasks which I have seen fail are all from the same manufacturer
(supertek) and were quite cheap. I've noticed in other reactions that better quality flasks such as Quickfit or Glassco brand seem to be more none
stick on the inside surface so possibly a smoother surface finish.
I'm just not quite ready to risk a better flask to failure on this reaction yet!
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bluamine
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In such a temperature degree you'll end up with some 'burnt' plaster which even doesn't get hydrated!!!
@clearly_not_atara: does this method make the glassware "passive"?
Wikipedia mentions that calcium sulfate is slightly soluble in warm hydrochloric acid if my memory is still good, it may help you @chemingeneer
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