Great job, nice crystallography as usual. I've found the dollar store to be a good source of CaCl2. They sell it in dry-air type room desiccators. Used to come in flake form, now it comes in prills, sometimes mixed with carbon pellets which are easy to pick out.
when you dumped the water into calcium oxide in the first step i immediately thought "oh no, gunna fling hot mud" but that pop wasnt too bad 😂 been there
Love your stuff, haha. I do my own. I'm not explaining and showing and my work like you are I like the way you present your videos its just simple, love the presentation!
Thanks @Cranial Construction. I appreciate it I know it's just s thing snd it helps to interact with people for the almighty algorithmic deities lol but thanks it means a lot zero traning but um making my own HNO3 fot gold refining/ gold recovery
When I was a kid, you could go to any service station and fill up the tires on your bike for free. And then eventually they started charging for it. First as a quarter, now I don’t know what. I think of Humphrey Davy every time I put air in my tires. After his invention of nitrous oxide, he was encouraged to commercialize it. He declined and said “let it be as free as the air we breathe“. I figure he’s rolling over in his grave every time I fill up my tires.
This one had me curious because of the purification steps. The stuff is ridiculously hard to purify without notable losses. I want to try clean calcium carbonate in distilled water with a source of HCl nearby... making it pure to begin with is so much easier than trying to clean it up as the chloride 🤣
@daox923 what about getting stuff oout if pine resin like pine sap they form sap balls they have a dozen or more uses in bushcraft and survival but I'm sure you coukd distill over some interesting compounds I'm sure okay so you can make turpentine from pine RESIN then you dina steam distillation and your left with turpentine and then in the boiling vessel you have Colophony! Which is ROSIN used for a Flux for soldering it's good for making esters Camphor Terpiniol Synthetic fragrances (lots of terpene chemistry Pyrolyais of rosin will get you hydrocarbons which is freaking sick!! These morons doing pyrolysis burning plastic bottles using fuel to do it and they think they have like 75 some 98% or 100% efficient lop don't they understanding their fuel isn't gasoline its kerosene hexane heptane etc... loll they aren't collecting different fractions at Temps these would distill over at so wouldn't it have like benzene and sh?
Hi, I have calcium nitrate how can I convert it to potassium nitrate, do I react it with potassium hydroxide or potassium chloride? And how do I separate the two compounds?
Both will work, but they have to be be processed differently. If you use potassium hydroxide, just add enough until no more calcium hydroxide precipitates out of solution and then filter the precipitate of calcium hydroxide and recover the potassium nitrate from the aqueous solution by boiling and concentrating it. For the potassium chloride route, just dissolve stoichiometric amounts of potassium chloride and calcium nitrate in enough hot water until everything is in solution. When the solution cools down, potassium nitrate will crystallize in needle shaped crystals (when it reaches room temperature you can put the solution in the freezer or in an ice bath to make more potassium nitrate crystallize out of solution). After that, just filter out the crystals.
I think adding a solution of potassium carbonate or potassium sulfate will do. This will precipitate the respective calcium salt (insoluble) whereas the potassium and nitrate ions will stay in solution.
I’m going to distill the hardware store hydrochloric but I think it contains iron from process equipment. But from watching this video and the acetone dilute the yellow color, maybe it’s an organic contamination
@@cranialconstruction2218 Indeed! If you did in fact crystallize the anhydrous calcium chloride and not the dihydrate, then it should be easy to react with any soluble sulfate or use in a desiccator. You will have to use it soon though.
It makes me very happy to watch your videos!
Great job, nice crystallography as usual. I've found the dollar store to be a good source of CaCl2. They sell it in dry-air type room desiccators. Used to come in flake form, now it comes in prills, sometimes mixed with carbon pellets which are easy to pick out.
Great tip!
when you dumped the water into calcium oxide in the first step i immediately thought "oh no, gunna fling hot mud" but that pop wasnt too bad 😂 been there
Haha...yeah that's a surprise : )
Love your stuff, haha. I do my own. I'm not explaining and showing and my work like you are I like the way you present your videos its just simple, love the presentation!
Thanks @Cranial Construction. I appreciate it I know it's just s thing snd it helps to interact with people for the almighty algorithmic deities lol but thanks it means a lot zero traning but um making my own HNO3 fot gold refining/ gold recovery
When I was a kid, you could go to any service station and fill up the tires on your bike for free. And then eventually they started charging for it. First as a quarter, now I don’t know what. I think of Humphrey Davy every time I put air in my tires. After his invention of nitrous oxide, he was encouraged to commercialize it. He declined and said “let it be as free as the air we breathe“. I figure he’s rolling over in his grave every time I fill up my tires.
That's for sure. I'm sure if he lived today he would have a slightly different look on life.
This one had me curious because of the purification steps. The stuff is ridiculously hard to purify without notable losses. I want to try clean calcium carbonate in distilled water with a source of HCl nearby... making it pure to begin with is so much easier than trying to clean it up as the chloride 🤣
make video about how to extract chlorophyll from leaves
Interesting idea
@daox923 what about getting stuff oout if pine resin like pine sap they form sap balls they have a dozen or more uses in bushcraft and survival but I'm sure you coukd distill over some interesting compounds I'm sure okay so you can make turpentine from pine RESIN then you dina steam distillation and your left with turpentine and then in the boiling vessel you have Colophony! Which is ROSIN used for a Flux for soldering it's good for making esters
Camphor
Terpiniol
Synthetic fragrances (lots of terpene chemistry
Pyrolyais of rosin will get you hydrocarbons which is freaking sick!!
These morons doing pyrolysis burning plastic bottles using fuel to do it and they think they have like 75 some 98% or 100% efficient lop don't they understanding their fuel isn't gasoline its kerosene hexane heptane etc... loll they aren't collecting different fractions at Temps these would distill over at so wouldn't it have like benzene and sh?
Hi, I have calcium nitrate how can I convert it to potassium nitrate, do I react it with potassium hydroxide or potassium chloride? And how do I separate the two compounds?
Both will work, but they have to be be processed differently. If you use potassium hydroxide, just add enough until no more calcium hydroxide precipitates out of solution and then filter the precipitate of calcium hydroxide and recover the potassium nitrate from the aqueous solution by boiling and concentrating it. For the potassium chloride route, just dissolve stoichiometric amounts of potassium chloride and calcium nitrate in enough hot water until everything is in solution. When the solution cools down, potassium nitrate will crystallize in needle shaped crystals (when it reaches room temperature you can put the solution in the freezer or in an ice bath to make more potassium nitrate crystallize out of solution). After that, just filter out the crystals.
potassium sulfate would work
I think adding a solution of potassium carbonate or potassium sulfate will do. This will precipitate the respective calcium salt (insoluble) whereas the potassium and nitrate ions will stay in solution.
Dibasic potassium phosphate also works and it you mix at 70 degrees Celsius the dibasic calcium phosphate precipitates in the anhydrous state!
I’m going to distill the hardware store hydrochloric but I think it contains iron from process equipment. But from watching this video and the acetone dilute the yellow color, maybe it’s an organic contamination
It's hard to tell exactly. Thankfully, you can crystallize the calcium chloride in spite.
@@cranialconstruction2218 Indeed! If you did in fact crystallize the anhydrous calcium chloride and not the dihydrate, then it should be easy to react with any soluble sulfate or use in a desiccator. You will have to use it soon though.