Depending on what you're planning to use it for, I would suggest doing a recrystallization in methanol. You shouldn't loose much material, and you will more than likely get a very clean product.
I love your videos. I was told in high school I wasn't smart enough to take chemistry. So I left and ended up being a domain level IT Administrator, specializing in AD, Powershell, & Exchange. But I'd rather be a chemist.
Thank you so much! I am surprised they would say that to you in high school.. seems rude.. At least it worked out for you in the long run but I admit being a chemist can be very fun. You could always try it out as a hobby. There is a ton of cool chemistry stuff you can do just for fun, I actually got my start by brewing beer and it kinda took off from there.
Hi Apoptosis, Sorry to ask, but what are those chemical equations that you wrote in your video at 2:01? You wrote: "5 Ca(NO3)2.NH4NO3.10 H2O + 5 K2CO3 --> 5 CaCO3 + 10 KNO3 + 9 H2O + NH3OH + H 2 NH3OH + CaCO3 CaOH2 + NH32CO3 (a bit of calcium hydroxide will favor formation of products)" While I agree about precipitation of CaCO3 out of Ca(NO3)2 and K2CO3 solutions, Ca(NO3)2 (aq) + K2CO3 (aq) --> 2 KNO3(aq) + CaCO3(s) The liberation of NH4OH (yes ammonium is NH4(+) and never NH3(+)) and desintegration of NO3(-) seems not possible under aqueous solution nor into the temperature range of your experiment). This also produces an inbalance into your chemical equation (one NO3(-) has disappeared from your NH4NO3 and the remaining NH3 has decided to form with one of the 10 H2O initially present some NH4OH( that you wrote as "NH3OH + H"). So the correct first equation is simply: 5 Ca(NO3)2.NH4NO3.10 H2O + 5 K2CO3 --> 5 CaCO3(s) + 10 KNO3 + NH4NO3 + 10 H2O Your second equation is also dubious: NH3OH should be NH4OH CaOH2 should be Ca(OH)2 NH32CO3 should be (NH4)2CO3 for a correct writing like 2 NH4OH + CaCO3 Ca(OH)2 +(NH4)2CO3 (but both CaCO3 and Ca(OH)2 are strugling for solubilisation because of their respective Ks (solubility constants) Now regarding 2 NH4NO3 + K2CO3 --> 2 KNO3 + (NH4)2CO3 Some boiling will drive off NH3(g) and CO2(g) away just like it does with chemical backing yeast ((NH4)2CO3). (NH4)2CO3(s) --heat--> 2 NH3(g) + H2O(l) + CO2(g) The presence of a little Ca(OH)2 or CaO will drive off NH3(g) out of NH4NO3 and form some more Ca(NO3)2 (*) 2 NH4NO3 + CaO --> 2 NH3(g) + H2O + Ca(NO3)2 2 NH4NO3 + Ca(OH)2 --> 2 NH3(g) + 2 H2O + Ca(NO3)2 Then the supplemental Ca(NO3)2 can react with one more K2CO3 to deliver one more CaCO3(s) precipitate and more 2 KNO3. Ca(NO3)2 + K2CO3 --> CaCO3(s) + 2 KNO3 (*) This is done onto another YT channel that turns the "calc-ammo-nitrate" to purer Ca(NO3)2 by addition of some CaO and recollection of exhaust of the system that is NH3(g) in another beaker as NH4OH solution. To finish my explaination, Most people forget that chemical displacements are not always as simple as it looks because into this too beautiful Epinal's image, the effect of NH3(g) onto calcium salts has been forgotten and disregarded. In fact there exists complexes of NH3(g) with Ca(2+); for example CaCl2 can catch a lot of NH3(g) and resitue it by heating; the same should apply to other salts. CaCl2(s) + x NH3(g) --> (CaCl2. x NH3)(s) Regards, PHZ (PHILOU Zrealone from the Science Madness forum)
Is it possible, instead of boiling the potassium nitrate solution, if you put it in the refrigerator for two days? Will potassium nitrate be produced and is the final quantity the same?
In the past I have had success producing potassium nitrate from calcium nitrate and potassium chloride, however i have yet to find a very reliable source of potassium chloride. I have however found a reliable source of potassium sulfate and wondered if that would be a viable method of producing potassium nitrate. I tried to find out myself by looking at the solubility of both potassium nitrate and what would be the byproduct, calcium sulfate, but have been unsuccessful at understanding weather it would work as I am not very knowledgeable about how the solubility of chemicals translate from paper to the real world.
Yep that would absolutely work 100% and was actually my initial idea for this video. The only difference is that calcium sulfate is slightly more soluble and much harder to filter than calcium carbonate, so your final product will be a bit more impure. Definitely a way better option than using potassium chloride.
This was soooo so cool if they had shown me this in chemistry class maybe I wouldn’t have fcken failed it it all felt so conceptual it didn’t make sense but this puts it into action
lol yeah you are 100% correct. I'm used to talking to people with a knowledge level where those terms are essentially interchangeable, but in a professional setting the difference is extremely important and it would definitely be a solution and not a suspension.
I'm trying to do this same thing right now but I'm using KCl salt substitute. I used to use this with the old ammonium nitrate to collect ammonium chloride and potassium nitrate. I'm currently waiting on crystals to form but they did not form cooling to room temp from hot supersaturated soln. I used more water than normal trying to get the calcium salt to dissolve so I've boiled it back down and into the fridge.. This is from instant ice packs, idk if it's the double salt or cheap version. I notice an inversion of solubility of calcium chloride and ammonium chloride sol between liquid ammonia and acetic acid. I plan to just wash the remaining mother liquor, after collecting potassium nitrate, with either ammonia or vinegar and take advantage to recrystallize. wish me luck
Wishing you luck! It is surprising no crystals formed upon cooling.. maybe they need a nucleation or a little glass stir rod scratch on the inside of the beaker.. I also did develop a way to make the CAN into plain calcium nitrate, but not sure when I'll release the video. All you have to do is boil CAN with calcium hydroxide which eliminates all the ammonia as gas. Then filter off the calcium hydroxide and you've got fairly pure calcium nitrate
ammonium carbonate scared me when I actually tried this on my own many years ago, I was getting into growing plants and stuff I was still in highschool, this was like one of the first 5 reactions I ever did, exactly as well I ordered potassium carbonate and I had calcium nitrate my neighbor gave me, I was quickly discouraged when the pot I was adding things to started to smell of cleaning products, but I perservered and ended up with some very crude KNO3 as I didnt have a scale or any proper equipment, I know I did it though because of that cursed ammonium carbonate smell. Good times I had forgotten about that reaction completely what a funny coincidence.
That is a funny one, I'm actually kinda surprised I've had the channel this long and just now getting around to this reaction. And yeah I also hate ammonium carbonate, but mostly because I can't for the life of me get it to crystallize.
Also the most successful video on my channel - guess why... 🙄 I had to use pure calcium nitrate, because calcium ammonium nitrate fertilizers are banned here... You should have recrystallized your product because it's always very impure when using this pathway.
Yeah I kinda figured it retrospect its likely impure.. luckily potassium nitrate has the steepest solubility curve I've ever seen so maybe I'll make that its own video on recrystallization. I'm guessing you also used potassium carbonate? I was initially going to use potassium sulfate but then I remembered you suggested using carbonates for this type of reaction in the comments of my ammonium nitrate video lol
@@integral_chemistry Yeah, potassium carbonate. Calcium carbonate is even less soluble and better filtrable than calcium sulfate. The precipitation of gypsum is only useful if you want to - displace nitric acid from its soluble calcium salt by addition of sulfuric acid - synthesize heavy metal nitrates from their soluble sulfates without using nitric acid
@@experimental_chemistry you are certainly right about the better filtration thats for sure.. Good point on the uses though, definitely would have been a better method for making copper nitrate from sulfate than my method just trying to take advantage of their differences in solubility..
“Moles” are a convenient way of referring to the number of molecules in a substance. One mole of any substance is 6.022x10^23 molecules, and “molarity” refers to the number of moles of a substance dissolved in one liter of solution.
Adding on to what Walton Chan said - a mole can be thought of as "the chemist's dozen." It's just a number that helps keep track of the extremely large numbers involved with molecules.
Adding onto what they both said, I think a good way to think about it is like this: Say you need to react equal parts carbon and oxygen to make carbon monoxide (which is a molecule composed of one carbon and one oxygen). You can't just use equal masses of both because oxygen atoms weigh more than carbon atoms, so instead you use moles. Every element (and chemical) has a "molar mass" which is the mass (in grams) of one mole of that element/compound. You can use that number to convert between grams and moles so that you use the right amount of reagent in your process.
It would be very tough to get reasonable purity but it's possible. Best strategy is to maximize the difference in solubility of the two products, and the product here aside from potassium nitrate is ammonium sulfate, which is more soluble until the water is literally boiling.
@@integral_chemistry i tried before calcium nitrate with sulfuric acid but it was a mess difficult to filter. Now i am thinking the potassium way or lead way the lead way is scarying me the toxicity level is to high 😔
I would love it if you could list some uses of the chemicals you make in these videos, both uses in industry as well as any uses that the chemical might have to someone making it at home. Great videos!
It's weird, I did that in every one of my earliest videos and then I just stopped for some reason.. No idea why but I'll definitely try and start again.
@@integral_chemistry Without sounding like one of "those" guys, I love the idea of being able to synthesize things I need if I ever actually need to do that. Being self sufficient basically. You mentioned a while back that you were interested in making a book detailing how to create several important medicines at home and I would be super interested in buying that.
Depending on what you're planning to use it for, I would suggest doing a recrystallization in methanol. You shouldn't loose much material, and you will more than likely get a very clean product.
Good idea^^ I figure this is pretty impure actually so I may just do that reguardless
What about acétone ?
Please do record your transformation of Calcium Ammonium Nitrate to pure Calcium Nitrate. Thanks and continued success with your channel.
I love your videos. I was told in high school I wasn't smart enough to take chemistry. So I left and ended up being a domain level IT Administrator, specializing in AD, Powershell, & Exchange. But I'd rather be a chemist.
Thank you so much! I am surprised they would say that to you in high school.. seems rude.. At least it worked out for you in the long run but I admit being a chemist can be very fun. You could always try it out as a hobby. There is a ton of cool chemistry stuff you can do just for fun, I actually got my start by brewing beer and it kinda took off from there.
@@integral_chemistrydid you take any courses or just learn by experimenting and reading?
Hi Apoptosis,
Sorry to ask, but what are those chemical equations that you wrote in your video at 2:01?
You wrote:
"5 Ca(NO3)2.NH4NO3.10 H2O + 5 K2CO3 --> 5 CaCO3 + 10 KNO3 + 9 H2O + NH3OH + H
2 NH3OH + CaCO3 CaOH2 + NH32CO3 (a bit of calcium hydroxide will favor formation of products)"
While I agree about precipitation of CaCO3 out of Ca(NO3)2 and K2CO3 solutions,
Ca(NO3)2 (aq) + K2CO3 (aq) --> 2 KNO3(aq) + CaCO3(s)
The liberation of NH4OH (yes ammonium is NH4(+) and never NH3(+)) and desintegration of NO3(-) seems not possible under aqueous solution nor into the temperature range of your experiment).
This also produces an inbalance into your chemical equation (one NO3(-) has disappeared from your NH4NO3 and the remaining NH3 has decided to form with one of the 10 H2O initially present some NH4OH( that you wrote as "NH3OH + H").
So the correct first equation is simply:
5 Ca(NO3)2.NH4NO3.10 H2O + 5 K2CO3 --> 5 CaCO3(s) + 10 KNO3 + NH4NO3 + 10 H2O
Your second equation is also dubious:
NH3OH should be NH4OH
CaOH2 should be Ca(OH)2
NH32CO3 should be (NH4)2CO3
for a correct writing like
2 NH4OH + CaCO3 Ca(OH)2 +(NH4)2CO3
(but both CaCO3 and Ca(OH)2 are strugling for solubilisation because of their respective Ks (solubility constants)
Now regarding
2 NH4NO3 + K2CO3 --> 2 KNO3 + (NH4)2CO3
Some boiling will drive off NH3(g) and CO2(g) away just like it does with chemical backing yeast ((NH4)2CO3).
(NH4)2CO3(s) --heat--> 2 NH3(g) + H2O(l) + CO2(g)
The presence of a little Ca(OH)2 or CaO will drive off NH3(g) out of NH4NO3 and form some more Ca(NO3)2 (*)
2 NH4NO3 + CaO --> 2 NH3(g) + H2O + Ca(NO3)2
2 NH4NO3 + Ca(OH)2 --> 2 NH3(g) + 2 H2O + Ca(NO3)2
Then the supplemental Ca(NO3)2 can react with one more K2CO3 to deliver one more CaCO3(s) precipitate and more 2 KNO3.
Ca(NO3)2 + K2CO3 --> CaCO3(s) + 2 KNO3
(*) This is done onto another YT channel that turns the "calc-ammo-nitrate" to purer Ca(NO3)2 by addition of some CaO and recollection of exhaust of the system that is NH3(g) in another beaker as NH4OH solution.
To finish my explaination,
Most people forget that chemical displacements are not always as simple as it looks because into this too beautiful Epinal's image, the effect of NH3(g) onto calcium salts has been forgotten and disregarded.
In fact there exists complexes of NH3(g) with Ca(2+); for example CaCl2 can catch a lot of NH3(g) and resitue it by heating; the same should apply to other salts.
CaCl2(s) + x NH3(g) --> (CaCl2. x NH3)(s)
Regards,
PHZ
(PHILOU Zrealone from the Science Madness forum)
I’d be really interested in seeing the calcium ammonium nitrate converted to calcium nitrate!
Just wash it with isopropyl alcohol which should dissolve the ammonium ions.
Would be interested in seeing videos on purifying 'hardware store' reagents.
I actually did that a few months ago! Video is called "turning fertilizers into pure chemicals"
Is it possible, instead of boiling the potassium nitrate solution, if you put it in the refrigerator for two days? Will potassium nitrate be produced and is the final quantity the same?
Yes, please record the purification of the calcium nitrate, that would be so helpful
In the past I have had success producing potassium nitrate from calcium nitrate and potassium chloride, however i have yet to find a very reliable source of potassium chloride. I have however found a reliable source of potassium sulfate and wondered if that would be a viable method of producing potassium nitrate. I tried to find out myself by looking at the solubility of both potassium nitrate and what would be the byproduct, calcium sulfate, but have been unsuccessful at understanding weather it would work as I am not very knowledgeable about how the solubility of chemicals translate from paper to the real world.
Yep that would absolutely work 100% and was actually my initial idea for this video. The only difference is that calcium sulfate is slightly more soluble and much harder to filter than calcium carbonate, so your final product will be a bit more impure.
Definitely a way better option than using potassium chloride.
You can buy giant bags of potassium chloride for water softener use here in California. Not sure about purity. I am not a chemist.
This was soooo so cool if they had shown me this in chemistry class maybe I wouldn’t have fcken failed it it all felt so conceptual it didn’t make sense but this puts it into action
Thank you
You just solved a big problem for me
Being pedantic but isn't a suspension a solid that is dispersed. The KNO3 was disolved 🧐
lol yeah you are 100% correct. I'm used to talking to people with a knowledge level where those terms are essentially interchangeable, but in a professional setting the difference is extremely important and it would definitely be a solution and not a suspension.
I'm trying to do this same thing right now but I'm using KCl salt substitute. I used to use this with the old ammonium nitrate to collect ammonium chloride and potassium nitrate. I'm currently waiting on crystals to form but they did not form cooling to room temp from hot supersaturated soln. I used more water than normal trying to get the calcium salt to dissolve so I've boiled it back down and into the fridge.. This is from instant ice packs, idk if it's the double salt or cheap version. I notice an inversion of solubility of calcium chloride and ammonium chloride sol between liquid ammonia and acetic acid. I plan to just wash the remaining mother liquor, after collecting potassium nitrate, with either ammonia or vinegar and take advantage to recrystallize. wish me luck
Wishing you luck! It is surprising no crystals formed upon cooling.. maybe they need a nucleation or a little glass stir rod scratch on the inside of the beaker.. I also did develop a way to make the CAN into plain calcium nitrate, but not sure when I'll release the video. All you have to do is boil CAN with calcium hydroxide which eliminates all the ammonia as gas. Then filter off the calcium hydroxide and you've got fairly pure calcium nitrate
very cool video i may have to try this as i do use a lot of potassium nitrite.
ammonium carbonate scared me when I actually tried this on my own many years ago, I was getting into growing plants and stuff I was still in highschool, this was like one of the first 5 reactions I ever did, exactly as well I ordered potassium carbonate and I had calcium nitrate my neighbor gave me, I was quickly discouraged when the pot I was adding things to started to smell of cleaning products, but I perservered and ended up with some very crude KNO3 as I didnt have a scale or any proper equipment, I know I did it though because of that cursed ammonium carbonate smell. Good times I had forgotten about that reaction completely what a funny coincidence.
That is a funny one, I'm actually kinda surprised I've had the channel this long and just now getting around to this reaction. And yeah I also hate ammonium carbonate, but mostly because I can't for the life of me get it to crystallize.
Hey wassup I’m not a fed btw
easy? it certainly is NOT easy to understand most of what he is saying. 😐
What do you don’t understand, you don’t need to know about moles etc just follow the recipe
Oh, this was the project you mentioned some time ago.
lol yep this is the one!
What ingredients did your fertilizer have? they seem to be different across regions, what is the percentage of nitrate, ammonia etc? Thanks
88% is awesome
Also the most successful video on my channel - guess why... 🙄
I had to use pure calcium nitrate, because calcium ammonium nitrate fertilizers are banned here...
You should have recrystallized your product because it's always very impure when using this pathway.
Yeah I kinda figured it retrospect its likely impure.. luckily potassium nitrate has the steepest solubility curve I've ever seen so maybe I'll make that its own video on recrystallization. I'm guessing you also used potassium carbonate? I was initially going to use potassium sulfate but then I remembered you suggested using carbonates for this type of reaction in the comments of my ammonium nitrate video lol
@@integral_chemistry
Yeah, potassium carbonate.
Calcium carbonate is even less soluble and better filtrable than calcium sulfate.
The precipitation of gypsum is only useful if you want to
- displace nitric acid from its soluble calcium salt by addition of sulfuric acid
- synthesize heavy metal nitrates from their soluble sulfates without using nitric acid
@@experimental_chemistry you are certainly right about the better filtration thats for sure.. Good point on the uses though, definitely would have been a better method for making copper nitrate from sulfate than my method just trying to take advantage of their differences in solubility..
2:23: Please do.
Someone please explain moll or moller muller? To me please.
“Moles” are a convenient way of referring to the number of molecules in a substance. One mole of any substance is 6.022x10^23 molecules, and “molarity” refers to the number of moles of a substance dissolved in one liter of solution.
Adding on to what Walton Chan said - a mole can be thought of as "the chemist's dozen." It's just a number that helps keep track of the extremely large numbers involved with molecules.
Adding onto what they both said, I think a good way to think about it is like this: Say you need to react equal parts carbon and oxygen to make carbon monoxide (which is a molecule composed of one carbon and one oxygen). You can't just use equal masses of both because oxygen atoms weigh more than carbon atoms, so instead you use moles. Every element (and chemical) has a "molar mass" which is the mass (in grams) of one mole of that element/compound. You can use that number to convert between grams and moles so that you use the right amount of reagent in your process.
Can we start with potassium sulfate and ammonium nitrate?
It would be very tough to get reasonable purity but it's possible. Best strategy is to maximize the difference in solubility of the two products, and the product here aside from potassium nitrate is ammonium sulfate, which is more soluble until the water is literally boiling.
@@integral_chemistry i tried before calcium nitrate with sulfuric acid but it was a mess difficult to filter. Now i am thinking the potassium way or lead way the lead way is scarying me the toxicity level is to high 😔
Please make thé vidéo of calcium ammonium nitrate to calcium nitrate 🙏🏻
Sounds like an interesting video! Thanks!
I would love it if you could list some uses of the chemicals you make in these videos, both uses in industry as well as any uses that the chemical might have to someone making it at home. Great videos!
It's weird, I did that in every one of my earliest videos and then I just stopped for some reason.. No idea why but I'll definitely try and start again.
@@integral_chemistry Without sounding like one of "those" guys, I love the idea of being able to synthesize things I need if I ever actually need to do that. Being self sufficient basically. You mentioned a while back that you were interested in making a book detailing how to create several important medicines at home and I would be super interested in buying that.
great video mate..