thank you!!

Awesome, thank you!

+Lane Haden Thanks man! Love to see more kids interested in home chemistry!

Same man been loving chem since i was 14 great to see others out there like me

+burgerischeap Thanks! Check out my other videos too because I think they're a lot better now.

2. Reply

Whoever's reading this remember God loves you so much!

HAHA! Don't trust me completely! I was like 15 back then

And most expensive

thanks!

No problem !

​@@BackMacScican we take aluminium from sand because sand contain around 10% aluminium

I appreciate your effort sir! question : can I ​use H2SO4 in the begging instead of HCl@@BackMacSci

You’re right about the the SiO2 reacting with the NaOH to form silicate, but the HCl is not able to break the covalent bonds between the Si and O atoms, and SiCl4 will never form when they are combined.

+Bilal Wattoo thanks man!

韩信 hey! I’m an stpm student too 😂

Harith Syahmie r u here to search for the same thing too?

Same here😂

qiqi leng 1 more day before being scolded by teacher for doing nothing!!!!

we are here. together

+Abby Rose thanks! This was a pretty old video though so you should check out my newer stuff too!

I would definitely check them out!

no,you rock!!

Good question, I answer that in another one of my videos by saying it doesn't make that good of a yield of elemental silicon as regular sand, but it does react brighter and faster!

you can use the 10% HCl if you like, but the purification process will take longer. If you are starting a home lab, I highly recommend get the 31% HCl that is commonly available at hardware or pool supply stores.

Good question! You should only add sulphuric acid to the sodium silicate in the correct mole ratio, otherwise you could be wasting reagents.

Hi Kyle, sounds like you have a fun project planned. On the part of the procedure you’re referring to, I added no water to the mixture because it would prevent the NaOH from becoming molten. And we don’t want that because then the Sodium silicate will form very slowly. Thanks for checking out the video!

Hi, thanks for your reply! Ah, that makes sense - and the info i've been reading suggest that beach sand silica in particular is much slower in aqueous NaOH. If you used 60 grams of your crude silicon dioxide with 80 grams of NaOH and the resulting yield of pure silicon dioxide was 40 grams after precipitating with the acid, does that mean that all 20 grams of the original crude 60 grams of silicon dioxide were impurities? Or did the acid precipitation step simply just not precipitate all of the silicon out of the sodium silicate mix? I ask because I hope to just use the crude silicon dioxide without further purification and I thought (going by your results) that I may need to reduce the amount of NaOH a little bit, since it would mean excess NaOH in the sodium silicate mix? Also, what is the least amount of water (in grams) that could be added to, say... 100 grams of the dry sodium silicate? I'm going for a dense yet workable sodium silicate mix, because when dry, the evaporated water will have left pores in it's place that will be throughout the set material, making it weaker. I may also try adding 1-5% glycerin as a plasticizer when mixing in the water - i've heard glycerin and some other types of plasticizers can be used with silicates to increase plasticity slightly, so it's not so brittle. Many thanks!

I think that the 20 grams of crude SiO2 that were not in the yield were left in the solution and didn’t precipitate, as you suggested. As for the amount of NaOH you are thinking of using, I would keep it the same but add more acid than I did. Finally, I do not know how to do the process of adding glycerin to the silicate so I can’t help you there, sorry! Have fun experimenting!

Thanks man, that's great! I won't be going to the precipitation stage, as I just want to make sodium silicate. And your video demonstrates how to make it from beach sand, plain and simple. I'll test out what the effect of adding glycerin is and how much to use. It's for making semi-transparent greenhouse panes - sodium silicate will be worked into white cotton sheet, which should work much like fibreglass or something similar. It seems like it would be a great alternative to plastics (like poly-carbonate) as they all leach out toxic stuff into plants/soil/those who eat the contaminants. And glass is not an option, as earthquakes are very common here these days. I can even see potential for plasticized sodium/potassium silicate as a binder for adding to rough fibrous paper for making boats and other things. If that doesn't work, then there's a way to dissolve cellulose (pretreated in hot acid, then washed) using NaOH and Urea at cold temps around or below 0 degrees Celsius - it produces a transparent plastic! That could also be an interesting one to try for your experiments/videos...? Information on alkali/urea cellulose plastics is severely lacking. Thanks again!

Sounds very enticing as a vid idea!

Yes! The sulfuric acid will dissolve the impurities fine!

+Tate Mac Thank you.

I believe this will slow down the rate of reaction significantly if you try to dissolve the SiO2 in aqueous NaOH, but give it a try and let me know if it works!

Does potassium hydroxide react with silicon and dissolve, and what is the percentage, please? Greetings

Does potassium hydroxide react with silicon and dissolve, and what is the percentage, please? Greetings

+Ryan Williamson Thanks Ryan, your method makes sense but I was 15 when I made this so I followed my source's instructions exactly.

Subscribed because this is great

+teddy susanto honestly it's probably around 95%

I'm not too sure! I would have to do more research about its production. But this process is not too harmful to the environment!

oooh good question. I wouldn't waste your time on that sand. Only purify sand that is composed of mostly SiO2.

Haha i think the product would be inert enough to eat, technically. BUT DONT DO IT

Semiconductors

95%

Yes you can!

Thanks mate! I just finished the reaction of the crude SiO2 and NaOH . Now i'm letting the reaction products dissolve overnight. Can't wait to see the results! Thanks for the info and the awesome video!

not usually, no. Almost all sand has impurities like the carbonates seen in this video. You should purify your sand by this process before melting the SiO2 into glass. Make sure you are using a furnace that can reach 3,200˚F otherwise you'll just heat up the SiO2.

+AJ Pollard Haha ok you caught me on that one...

Glad you took that one good, I was afraid you wouldn't after I posted it.

NurdRage: Dissolve Glass With Drain Cleaner

AJ Pollard No, it is ok to stir it with glass, but just not in a glass container,

This is proof how inexperienced this kid is and things like thermite he shouldn't be doing. It's all fun until he builds a nuclear reactor in his back yard and it melts down. Or worse.

Nitrous you can

SiO2 is litteraly just sand tho

In this case yes. You are literally stripping calcium carbonate and iron oxide from the silica in sand

If the river sand is silicon dioxide-based then yes!

+Alper Gökcek Haven't tried to test for that and don't know how... haha. Why?

Because i want to make homemade piezocrystal for experimental purposes.

Quantum entanglement

basically NaOH+SiO2--> sodium metasillicite and bunch of different sillicates like Na2(SiO2)7 which then react with sulfuric acid to get create many forms of sillicic acid then some silicic acid decomposes in the presence of sulfuric acid after drying all of the sillicic acid decomposes into K2SO4 and sillicone dioxide(sand) and K2SO4 is water soluable

It is pure silicon dioxide.

+Greg L. The theory is that the mass loss is due to CaCO3 impurities.

I would just call it a "Chemical Purification of Beach Sand"

Me too!

【Price and details of silicate dryer】www.best-dryer.com/dryer-machine/sand_dryer.html?yt/cxf

I use stoichiometry. If you want to know how to use this method, watch Khan Academy's Videos on stoichiometry and do many many practice problems! www.khanacademy.org/science/chemistry/chemical-reactions-stoichiome

No, water doesnt react with calcium carbonate

it may be the sound of a small amount of water turning into steam very quickly as a result of the sulfuric acid disproportionating.

Thank you so much. Excuse me, do you have any idea on how to make silica gel which act as a stationary phase on tlc plate?

Or silica gel which use to absorb moisture.

I would just called it a Chemical Purification of Sand

Porque la arena trae CaCO3 ,caliza,triturada.

Because sand gets CaCO3 in the beach

+Apex Window Cleaning Services You can buy SiO2 in pounds on amazon or ebay for dirt cheap if I'm not wrong!

They put silica sand in the furnace during the smelt to lower the melting point of the ore and used it during the folding process to refine the iron.

SiO2 + Mg --> Si + MgO silicon is a semi conductor, very useful moreover I have read that silica (silicon dioxide SiO2) is quartz, however I'm not sure

Eat it

@@rvnaumenko5 NOOOO

Hopefully will get a quick reply

Park here for the formula too

haha

If you are curious about the purity of the final SiO2 in this video, it should be >99% as long as you fully convert the sodium silicate to SiO2. Good question, and I apologize that I'm shit at response time lol.

@@BackMacSci thank you for that

+desta Yakob it won't burst it may only decompose if heated too strongly

HCl = hydrogen chloride. Add water and you have Hydrochloric acid. Hydrogen chloride solubility in water 823 g/L (0 °C), 720 g/L (20 °C), 561 g/L (60 °C). So as you heat it up, some hydrogen chloride and water will evaporate off. But having something cold will condense both water vapor and hydrogen chloride that is now more soluble in the condensed and colder water.