Extracting Potassium Chloride

[@lizzyreeve2676]

enjoyed the tasting excerpt

[@AndreasNilsson96]

Awesome. I have a salt called Seltin & this was exactly the video I needed. Thank you!

[@marcusolsson2126]

Have the same salt, did it work for you?

[@AndreasNilsson96]

@@marcusolsson2126 Yes, go for it!

[@marcusolsson2126]

@@AndreasNilsson96 Didn't work for me... In the video he says take of when it boils I do that nothing happend no crystals?

[@SimonMannen978]

Omg Skandinavia?

[@Handle-c8l]

@@marcusolsson2126cool it in your freezer and don’t add to much water

[@adelinyoungmark1929]

zingy is a perfect way to describe it. ive bought a 5 kilo bag of sodium free salt and i tried some and it tasts zingy. E&F did a vid trying all the alkali chlorides and the best im pretty sure was just plain NaCl.

[@fredluden2298]

For your copper sulfate sulfuric acid video did you ever calculate the concentration by using the density?

[@atari7001]

The solubilities of the carbonates are much further apart, which is much more efficient than the chlorides. For almost perfect separation, use electrolysis. Kclo3 is almost completely insoluble, while the naclo3 is very soluble. Interestingly, naclo4 is soluble in organic solvents, while nothing else is...

[@yahyanassar9205]

Is it possible to, turn potassium citrate to potassium chloride ? Thanks.

[@peksoleb3869]

does the mixture need to be fully saturated?

[@fiokgoogle8779]

Wery on the point and i was looking for a proof that at the result is KCl and not NaCl and from the cristalisations form its wery dificult to say , but with flame test its a clear opservation. Greeting from Hungary 🎉

[@Michael-rg7mx]

What's the difference between chloride and perchlorate?

[@ScrapScience]

Chloride is an ion formed from a chlorine atom with an extra electron, giving it a 1- charge. Perchlorate is an ion formed from a chlorine atom surrounded by four oxygen atoms, again giving a 1- charge.

[@JukkaCantDrift]

So perchlorate is a Better oxidizer?

[@alockworkorange7296]

I was sure ur title was gona be wrong because in america our diet salt is like 95-99% kcl but now it all makes sence

[@muyfoods]

Thanx for it😁😁 Can we separate salts using its single cristal by growing ??

[@koukouzee2923]

Yea

[@elepthia]

how can we extract Potassium Chloride from sea salt?

[@ScrapScience]

I've no idea. There's not enough potassium in seawater to make it worth your time or effort in my opinion. You'd likely need to find some kind of adsorbent which selectively adsorbs potassium ions to some degree, since relying on simple precipitation methods woud be tricky for such a low concentration of K+.

[@sebastiannolte118]

For some reasone its not working for me, i dissolve the salt into water then boil it and then filter it with 2layers of the same stuff he uses yet no crystals are forming ?

[@ScrapScience]

You need to dissolve the salt while the water is at boiling temperature, not beforehand. You also need to use only just enough water to get everything to dissolve - having too much water won't allow anything to crystallise.

[@baseddino]

are you using them for an electrolyte blend and thats why it dosent matter if theres salt in yours

[@chemistryofquestionablequa6252]

He’s using them for a chlorate cell

[@ryanallen1014]

For some reason I cannot get much at all to crystalize. My salt substitute (ss) is the same composition as the one featured in the video. I dissolved in distilled water, stirring well the whole time. Decanted and filtered multiple times. I use a small excess of water to the whole container of the ss. I boiled some to reduce the solution by almost half, then set out on my back balcony with the temperature not reaching positive didgets for over 24 hours and barely anything has precipitated out. If anyone has some advice or can tell me where I went wrong and how to fix it, I would appreciate it greatly. My end goal was potassium chloride to react with ammonium nitrate to use in making nitric acid. So with another container I bought Im going to react it directly with ammonium nitrate and distilled water. I will split the total amount of water needed for the reaction into both my chloride salts and nitrate salt to dissolve the and filter into my reaction vessel directly and then hopefully crash out a mixture of sodium and potassium nitrate which should work together to make my nitric acid via distillation of a reaction between the nitrate salts and sulphuric acid yielding very pure and concetrated nitric acid.

[@Moritz___]

Wel why you using kcl and not just plain nacl

[@FireAndFumes]

Bit late but make sure its very very saturated as it happened to me too. Add salt to the beaker then add some water bring it to a boil, then if its not dissolved add some more water. Its better for there to still be some undissolved salt at the bottom when you filter as you can just add more water after. If you didn't do this and added too much water bring it to a boil and boil it until there's some salt crystals on the bottom, then filter.

[@arne.wryningen9074]

Can you do this with regular table salt?

[@ryanallen1014]

No, because regular table salt is just sodium chloride (and most likely a small amount of iodine).

[@bhavukdhiman8950]

How to make potassium perchlorate

[@ragingking1424]

R we using just distilled water or?

[@beasttrad4362]

ALWAYS dH20 (yes, distilled.)

[@dennisford2000]

Could you just dissolve it slowly in cool water and just sodium chloride dissolve at minimum, a warm rinse and cool with the salt water discarded.

[@ScrapScience]

I'm afraid not. A lot of the more soluble sodium chloride would be trapped in the crystals of potassium chloride, preventing them from dissolving and making this type of extraction very inefficient. Dissolving and recrystallising is just more effective and faster here.

[@dennisford2000]

@@ScrapScience are you sure you have compound crystals or two crystals mixed z

[@ScrapScience]

Oh interesting, yes that's a good point. I'm honestly not sure whether the salt is just a mixture of the two compounds, or if they were crystallised together. If it's just mixed, your idea would probably be effective, yeah.

[@baluvlogs5727]

Hi friend...please clear measurement potassium chloride prepare in house what is the ingredients in adding potassium chloride

[@bobsunkees3392]

Salt substitute

[@yasyasmarangoz3577]

How to make sure, that there is no NaCl?

[@ScrapScience]

It's very unlikely that this process can remove the NaCl in the salt completely, but a large enough number of recrystallisations might be able to. To check for the presence of sodium, you can perform a flame test of the salt. If the flame looks faintly purple, you should have pretty pure KCl, but if there's any indication of a yellow sodium flame (which should show up even at low concentrations), it can obviously be purified further.

[@yasyasmarangoz3577]

@@ScrapScience Oh, what a coincidence. I only wanted to make that chemical to test that! Yes, it doesn't need to be 99,999% pure. But what I actually wanted to know is, is the NaCl crystallizing slowlier? Or why do we just get KCl?

[@ScrapScience]

Ah rightio. The reason that KCl crystallises out to a greater extent is from the difference in the solubility curves. If you have a look at a graph of such data: d2vlcm61l7u1fs.cloudfront.net/media%2F9cc%2F9cc03ce7-7f2e-41ef-a3c1-f11d44f18759%2Fphp1FftoW.png You'll find that the solubility of KCl changes (between 100C and 0C) by a much greater extent than does NaCl. As a result, cooling a saturated solution of both KCl and NaCl will crystallise much more KCl than NaCl, seeing as pretty much all the NaCl remains in solution (the solubility has hardly changed) while nearly half the KCl is crystallised.

[@yasyasmarangoz3577]

@@ScrapScience thx m8! Keep up the good work you're great.

[@Jeff-ml2ek]

Let a small amount of the salt sit in the microwave.If there is purple plasma than you should have potassiumchloride

[@vaggs75]

Why do you boil it though? You didn't explain it.

[@ScrapScience]

Boiling the solution is just for dissolving the maximum amount of salt possible in the smallest volume, the goal is to get the solution saturated at 100C. Upon cooling, the solubility of KCl decreases, and it crystallises out.

[@vaggs75]

@@ScrapScience Wouldn't you get the same result if you just mixed them at room temperature. Also, could you do the same experiment with sea salt, or other salts?

[@ScrapScience]

Mixing them at room temperature would only work if the salt were crushed into an impossibly fine powder. Mixing the salt up at room temperature (without it being an impossibly fine powder), would allow for some NaCl to be trapped within crystals of KCl, making the process only slightly effective. Dissolving all the salt and cooling the solution allows our KCl to crystallise out in an almost pure form, as the NaCl will just remain in solution. Sea salt is primarily NaCl, which has a very shallow solubility curve. This means the solubility of the NaCl won't change much between 100C and room temperature, so it's very difficult to make crystals like we are doing here. The same process definitely works for other salts though. In fact, it's a very common purification technique for soluble compounds (for example, potassium nitrate or copper sulfate).

[@vaggs75]

@@ScrapScience Thanks a lot! That makes sense now. Could you try playing around with solubility of NaCl and KCl at 90 C? I saw in a diagram that KCl is more suluble, so the NaCl will settle down, while the KCl will remain in solution.

[@markselten4985]

Nice trick

[@oxygen2623]

Is that pure KCl safe to consume?

[@kennethstudstill]

Yes, it's mixed with NaCl just for taste.

[@davidbivens2246]

This doesn’t make any sense both the calcium chloride and the potassium chloride are soluble in water.. when it crystallizes you are getting both crystals. Not just potassium chloride.

[@ScrapScience]

Potassium chloride has a much steeper solubility curve than sodium chloride, so cooling down a saturated solution significantly favours the crystallisation of potassium chloride.

[@Handle-c8l]

The pottasium chloride will fall out first as long as their is excess water

[@saudkhanmychannel4471]

Bro make a video about acetyl cloride

[@LarryaproudU.S.citizen]

You can buy this in bulk on eBay and Amazon cheap.

[@Skippy_op4]

Holy shit mate where are you from in Australia

[@ScrapScience]

Tasmania's the one

[@mak004]

are you from australia

[@ScrapScience]

Yep, correct

[@vincewolfhagen6982]

Nice

[@coralk]

It’s so werid to think tht we eat this because the y put this stuff in Dorito crisps

[@BEYOUTOTHEFUL]

i need potassium chloride for my water system , can i just sue salt, thank you Angela

[@jessefish2273]

Wow scientist

[@sharadkumarsingh8972]

Waiting for 8 bit computer

[@deepajain3070]

Can we talk onwer of chenal Very need full

[@johnwoody5109]

I'm on a cash diet

[@johnwoody5109]

I'm one day old

[@johnwoody5109]

Hired

[@MultiJerm1]

How is that KCL thats just salt get wet and dry up...salt again nothing else. Ad water to dry salt boil it dry in pan is the same. Salt again.. why is it called kcl now? There nothing changed

[@ScrapScience]

The product I'm using contains a 50-50 mixture of potassium chloride and sodium chloride from the start. We're selectively extracting the KCl because its solubility curve in water is much steeper than that of NaCl. The NaCl stays in solution while we allow the KCl to crystallise out.