Recrystallization 

Because they aint as gangster lol

Was thinking the same.

Because they are more dilute. Lets take an example: A precipitate was obtained from a solution containing A and B at 1:1 molar ratio. Let's say we precipitate A but maybe 1% of B got caught in A's crystals. Using fresh solvent we redissolve A's crystals and this makes a new solution with ratio 100:1 If you repeat and 1% get caught up in the crystals, this time it will be 1% of 1% so the new amount of impurities will be down to 0.01%

Use cold solvent to wash away any impurities from the recrystallised product without dissolving it.

No that would dissolve it again and it would go through the filter 🤦🏼‍♀️ you want to keep the crystals on the filter

No 🤣

Where are you from?

No, crack is made by mixing cocaine with sodium bicarbonate in hot water and then evaporating all the water

@@isaackalashnikov3681wrong Ehen you do this method you will have the hole Salt in the free base !!! You use bicarbonite and Wait since the freebase Fall out and than throw the water away and dont evapoate it or use Ammoniak thats the purest Crack cokain But you should Wasch the Rest of Ammoniak out with water and the Street recept is to mix the coke powder with bicarbonate and but the dry powder into a microwave and Cook it thats dry cooking and you have more wight for the blackmarkwt because the hole bicarbonate Salt is in it 😂😂😂!

Could you explain me how to get MCT oil from cocunut oil ? Step by step....

Breaking bad (real)

He explains it in a very non meth way

Helps with dmt too

Helps to make high purity bleach crystals from a bleach solution on hand, for storage and longevity of the now pure stable and solid form of Sodium Hypochlorite. My question would this make the sodium Hypochlorite crystals a salt base or HCL solid?

Solids usually have different temps that they crystallize at. Know your temps for the main ingredient you want to keep and your problem is solved

So that the product will precipitate again. Otherwise it will just stay in solution and you can't collect it.

@@ProfessorDaveExplains thank you! that makes it clear.

It's not necessary, it's just taking advantage of the fact that solids have specific solubility that correspond with temperature. "Room temperature" is just a standard reference like zero is between 10, and -10. For example, chlorates have a very low solubility versus chlorides at 0°C, which is much lower than room temp. On the other hand oxides may have no solubility until say 1,500°C. It just depends on what you're trying to do, but most crystals are nitrates, sulphates, or chlorides, and those are easiest to manipulate at 25°C (room temp).

Hallo

@@zainrabee2675 yes

Where are you from?

glass stirring rod

You first have to go find the literature on that product and identify it's properties. If it's an oil then a non polar solvent is often good enough, but some behave differently when it's an organic vs inorganic solvent, so that may be important. So after choosing the best available solvent then try to identify other components that may carry over with it, and the properties of those to see which can be separated with the methods available. I'm not familiar that compound so I can't tell you a specific method.

No. The general principle is just reducing the solubility to a point where the solvate is less soluble than the impurities. Crystalization of the appropriate product is best as a first step where it applies, but not all products crystylise in the same fashion or even in a practical means. One such method is dissimilar separation, where you use two different solvents that won't mix, but the product and impurities are more attracted to one than the other. This is usually a method to separate organic and inorganic molecules, but is also useful between polar and non polar molecules.

The composition. And... yes? I'm not sure.

Let's take quartz or Rudy (corundum) as an example. No, they would after the e process be considered lab grown or artificial, even if you dissolved naturally harvested components and used a seed crystal to kickstart the process. The reason is because they were altered and remade in a lab.

Yes, watch my general chemistry playlist from the beginning.

Drop strings into the solution and let them form onto the string

Yes, evaporative

Yes, there are a few ways, but it depends onr he properties of the solvate. As someone said evaporation of the solvent is one method, which requires either heating or dehydration by some method. One method is to add a solution of another chemical that has a higher affinity with the solvent than the product, and that will reduce the solubility of the product and cause it to crash or precipitate out, although requiring additional purification steps.

Blow up?

What solvent u using?

@@god-8use isopropyl alcohol and add acetone to reduce solubility once its disolved with minimal isopropyl :-)

Hexane or heptane

How about naptha or denatured ethanol ?

Filtering is a physical separation of products. At the point where you are ready to filter,, you have rendered either the intended product or the impurity as a solid that can be separated by a filter, screen, or some other physical process. This can also be just letting the solids settle to the bottom while pouring (decanting) the liquid.

This is organic chemistry.

Yes, if you have the appropriate solvent. Assuming you used a double displacement method to convert the appropriate salt to the available chlorate, the salt will have a higher solubility than the chlorate corresponding to temperature. Typically heating to 100°C and cooling to 0°C twice twice while discarding the liquid each time will result a very pure chlorate because the chloride salt is that much more soluble in water that chlorates are.

Freeze precipitation

Impurities are highly soluble in solvent at room temperature so when recrystallization occurs they remain dissolved in solvent.

It only works if the impurities and product have very different properties. The impurity has to remain dissolved at the cooling temp (check its solubility) and the product has to have a way low solubility at that temp. Take sugar and baking soda for example. Baking soda has low solubility compared to sugar. You can dissolve them both, but if there’s less than 2 grams of sugar per mL of water, it will remain in solution at room temp. Meanwhile, the baking soda will crystallize out of solution until the concentration hits 0.1 grams per mL of water. Of course, solubility increases with each solute added so keep that in mind and expect lower yields for bulk impurities. Now take salt and baking soda for example. Their solubility is 0.35 g and 0.1 g per mL water respectively. You’d have to dilute between 0.1 and 0.35 g/mL to keep salt dissolved and baking soda hyper saturated. However, you’ll never be able to get more than 0.25 g of baking soda out per mL of water. And the closer to 0.35 g/mL you go, the more you risk getting salt in the mix. At the maximum scale, you’d only be able to get (1 - 0.1/0.35 *100)% or ~65% of your product (baking soda) out of solution. Whereas in the first example, you’d have (1 - 0.1/2 *100)% or ~95% of your product recovered

The crystals have a higher affinity toward themselves, meaning they push out impurities into the solution. Let's say that hypothetically you as you said have two solvates with exactly the same solubility properties in that solvent. The two crystals would grow apart from one another, but likely still be interlaced making separation by this method difficult. You would get grains of both products inside of one another and would have to find an alternative method. Thankfully no two chemicals have exactly the same properties and separation is still possible, even if it's a huge pain in the ass.

What is the recovery rate of 2.1 grams of benzoic acid? please reply

@@halaashraf2409 the recovery rate is approximately 2.754 weeks, one day after the blue moon, roughly 32 seconds before lunch time

hmm, well it might, it just depends on the precise melting point, but it's not the ideal situation