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How did you make the sodium acetate? Sounds like you got some sodium carbonate unreacted left in your final product that led to carbon dioxide when exposed to new vinegar.

​@@CinzLab Ah I see, I managed to fix the problem tho. Anyways, here's the procedure I did if you're wondering(I'll only explain the boiling part) 1. I boiled the solution. 2. When I noticed the solution was boiling, I decided to put even more baking soda because I thought it would "supersaturate" the solution even more. 3. I think I made a mistake by doing that because it may have caused traces of Sodium Bicarb in the Sodium Acetate after I evaporated it off.

I do not recommend using ethanol in a hot apparatus due to the inflammable risk, unless in an approlriate lab. Ethanol however is volatile and if you use it to extract the oil, separate the two will not be easy.

When you use solvent for extraction you use solvent with different density in order to easly separate the two. But then you need to remove the solvent without losing yield in the product.

That's for mixing (magnetic stirrer)

@@francesco.cinzano Thanks.

We can't say it. It's not pure. We can assume it contains an appreciable amount of limonene since we know the typical high percentage contained in the orange. (The high evaporation rate confirms its presence in a high percentage, though) Other molecules are also present in smaller quantities. For a quantitative value of purity, we should carry out a quantitative analysis or an NMR.

For the same reason I didn't use acetic acid instead of vinegar: home's chemical availability

@@francesco.cinzano OK I see. I just wondered because where I live sodium carbonate is available as a cleaning agent just at the supermarket and it's really cheap.

It can be or 1) if you cooled the solution quietly it can became oversatured and so require some perturbation (or another crystal) to precipitate the salt; 2) the solution you are cooling is not saturated.

The amount of baking soda should be stoichiometrly correct. Because it's easier to remove unreacted acetic acid (evaporation) than to remove undissolved baking soda (filtration) you can put a bit less than it should be.

When you added baking soda to acetic acid, sodium acetate is already in the baker, but dissolved. You need to evaporate all the water in order to obtain the sodium acetate powder. If you want to (like in the video) observe the crystallization process, you cool down the saturated solution and then see the crystal precipitating.

It depends on your equipment such as your heater and your refrigerator. The more it cools down, the more oversaturated the solution became. If you let it too long it can start precipitation spontaneusly.

Because of the saline solution, it would taste very salty 😋

@@francesco.cinzano OHHH NO! I meam te strawberry🤣

It depends on how fast the oil goes down and separates. It takes about 30 min.

Yup, you need a lot of caution since it is hygroscopic and caustic, and new stoichiometry calculations (Na2CO3 is 2:1 and NaOH is 1:1 with acetic acid)

It was near 100°C in order to obtain a decent evaporation. Otherwise it would take very long to reach the saturation.

There's no difference as long as the steam flows through the peels in the upper flask. It's the steam that extracts the essential oil.

@@CinzLab thanks for the reply, so I'm guessing this goes for all oil extractions. Thanks again.

Never mind you explained it lol

6% according to the label

Since crystallization is a purification process by itself, no other steps are required to purify the product it crystallizes. If you want to purify further you can always do one more cycle, losing in yield.

@@CinzLab I´ve always wondered what sort of impurities would give that golden-orange color in concentrated solutions of usually colorless acetates like sodium acetate.

For food use, such as when making liqueurs (like limoncello), always make sure to work with fruit that has not been treated with pesticides.

Mine to

Are you from tips

It is sold as baking soda. You can get a box of it from grocery stores or baking supplies

The extraction with a solvent is the standard when we have to extract a liquid from another liquid. The extraction of Limonene is also possible with a solvent, like hexane or a non-polar one, and it definitely would maximize the yield. The extraction of Limonene is also possible without a solvent just because limonene oil has a lower density compared with water. So it naturally floats on the surface. If you performed an extraction with different oil, like the eugenol, it still won't mix with water, but its density is instead very similar, and the oil will form a suspension of very small oil droplets in water. The purity of Limonene is directly reliant on the natural composition of the oil, which can slightly change from fruit to fruit. Limonene is however the major component (>80%) of the oil.

@@CinzLab Thank you so much for taking the time to reply to my question. I found it very confusing and you've explained it in a way that was easy to understand

Limonene is totally apolar, being aliphatic, therefore a good solvent must necessarily preserve this characteristic. Furthermore, it must have an appreciable difference in terms of density with respect to water in order to float or sink and make it possible to extract only the apolar phase with the separator funnel. Finally, it must be volatile, in order to be easily removed. Hexane, DCM, acetone... should work.

@@CinzLab thank you !

"D-limonene is listed in the Code of Federal Regulations as generally recognized as safe (GRAS) for a flavoring agent and can be found in common food items such as fruit juices, soft drinks, baked goods, ice cream, and pudding. D-limonene is considered to have fairly low toxicity." pubmed.ncbi.nlm.nih.gov/18072821/ pubmed.ncbi.nlm.nih.gov/23573938/ Caution in chemistry is mandatory. Many harmless substances in small doses become dangerous in large quantities.

Yes. You can also perform an NMR to best evaluate purity!

For the quantification of chemical compounds mainly instrumental methodologies based on physical principles are used. In this video, as you could see, a quantification was not carried out, but an estimate was based on the composition of the essential oil extracted. To learn more about the methods of quantifying limonene, I refer you to this article: www.perkinelmer.com/PDFs/downloads/APP_Limonene_In_Citrus_Rinds_By_GCMS.pdf

@@CinzLab Thank you very much for this. You are a blessing ♥️. We will be having a reporting about this and I am having a hard time coping up and how to explain it :(

My videos are set to be enjoyable and exhaustive as much as possible about every experiment. A slow and peaceful video is essential to allow people to understand the concepts and also to appreciate the clips. This’s the compromise I found. The reason why I didn't put the yield in the video is the following (I already answered to this question few comments below): as you can see from the video, a water drop joined along with the oil in the test tube and prevented me to quantify exactly the oil extracted. Removing that drop wouldn’t be worth it. I got about 3 ml of oil: the usual yield is claimed online to be 1%, depending on the variable quantity contained in every single fruit.

Thanks for the reply and info. Was that from about 5 oranges?

@@bodo9387 You're welcome. Yes, from 112g of peels. The yield could be maximise extracting the oil from the distillate with a solvent like DCM (di-chloro-methane) but I do not have a fumehood or an equipped workspace to handle it so I preferred to take advantage of its density property and separate it just with the funnel.

@@CinzLab many thanks, that's helpful. Or separating with a centrifuge?

@@bodo9387 that is a good technique too

100°C (at standard pressure): the boilong point of water, that is able to safely codistill the oil without thermal-decompose it.

It is a normal phenomenon called "voltage drop".

@@CinzLab it can only hold 3-4 sec .it cant light lamp after 3-4 sec.

@@mp3huntertr first, provide a description of your set up

Provide a short description of your setup. Did you use something that may have contaminated the electrolyte, for example exposed copper wire partially immerged during charging/discharging?

@@CinzLab i use 6 M KOH and 0.2 M zinc acetate as the electrolyte. zinc foil as the negative electrode, carbon paper as the positive electrode, and the battery like this website www.advancedsciencenews.com/new-air-electrodes-zinc-air-batteries/ There is no other metal in the battery except zinc.

@wayne In the electrolyte should be present mostly zincate ions and some zinc oxide and zinc hydroxide as byproduct. All of them should be colorless however. What about the yellow color? Does it appear in the discharging process or after the discharging/charging sequence? At the moment I'm thinking about an acetate byproduct, as far as you have an organic component in a strongly caustic solution, that could someway decompose it in a sort of long term side-reaction. Do you observe the same phenomenon also without using zinc acetate?

CinzLab During charging and discharging, yellow will be slowly produced, and the color will become deeper and deeper. However, zinc acetate is mainly used as a substance needed to provide a reversible reaction, so it must be added. What are the possible byproducts of zinc acetate?

@@andy915029 what about the carbon paper? What's its composition? Does it seem damaged by the solution?

About 3mL of Limonene. The presence of that drop of water prevented me from carrying out an evaluation with the balance. I didn't remove it just because I thought it isn't worth it, as far as the yield is very low. Usually the yield is about 1% (from NileRed) but it can widely change depending on the single orange. Some organges contain a lot of essential oil, some less. Same for lemons.

Definitely not as efficient as zinc bromide battery showed by the guy. As he says, to make a battery there are a lot of things to consider. Just the fact that in my project I used Na2CO3 instead NaOH as electrolyte killed the efficiency of the cell (and I needed to make x3 to light a LED). Air battery are sensitive to air purity and oxygen concentration and because they need air, aren't so easy to handle (you can't have a isolated case). The zinc bromide seems a great and documentated-useful alternative to this kind of battery.

Biodiesels are long chain fatty acid esters, obtained by vegetable oils (triglycerides) reacting with methyl/ethyl alcohols through a process called trans-esterification. Essential oils, like limonene, have different structure and properties and their flammability doesn't lead to an efficient and useful role in biodiesel.

@@CinzLab so it only runs a steam engine :/

@@giovannicesaramorim9adigan961 just water steam can manage it

@@CinzLab i was saying about fuel, like gasoline. Cuz in a steam engine it doesnt need to explode