same!!

I could watch it all day, every time he breaks it our I think yay vacuum filtration.

I knew a couple girls over the years who were experts at vacuum filtration

vacuum filtration sucks

I love Grignard Reactions

+sdfdsv I should have said "the last ingredient" but oh well.

I thought acid that earlier

+Nile Red Why are there thing written in french on every bottle ?

In Canada English and French are both official languages.

sdfdsv I'm so glad someone else noticed, I almost died laughing.

Because it evens the population and only the intelligent will survive

@@watermaker2.033 just one little taste... 10 hours later: 'dead'

@@akuakkk1908 it was only a joke sir.

@@brainwashedbyevidence948 i see, sorry. And thanks for telling me that

@@akuakkk1908 no that's OK...hahaha😅

lol

I did this earlier today by accident. I was making copper hydroxide to use as a pigment for a limewash paint and completely forgot about this reagent. It dissolved the filter paper and came through the Buchner funnel lol

@@SafetyLucasbahahahahaha I’m collecting dividends from a comment I left 7 years ago Sorry about the contaminated setup!

😂😂😂

I know this is an old comment under even older video, but I'd like to chime in anyway with a recollection of my own experience from... yet older times ;-) Which was during my sec. school, which was called "chemistry technical college" (secondary vocational education preparing students for work in the field as lab technicians or factory middle management, or for a university/ polytechnic studies, if anyone wanted to pursue a higher education. AFAIK there's no equivalent of such schools in US or any "English" education system - but I digress here). Anyway, making that Cu(OH)2 was one of those lab exercises we were supposed to conduct in the first year. The procedure in the handbook called for adding NaOH directly to the solution of CuSO4, and - surprise, surprise! - entire class failed to get anything even remotely resembling what we "were supposed to obtain". The precipitate was slimy and clogged filters right away (paper filters in Büchner's funnels, obviously vacuum filtration), and it pretty soon turned blackish. No one knew "whisky tango foxtrot?", not even our teachers. (That was in times before Google, so searching for answers wasn't as easy as it is today - actually, it was even before the advent of the internet "as we know today" - and, frankly, even before those fancy gizmos latter called "personal computers" appeared). But one smart fellow from our class went to the school library, went through few books there, and then he said that apparently SO4[2-] ions are somewhat catalysing decomposition of Cu(OH)2 into CuO (which is black) and water (which isn't black, except for Blackwater). Unfortunately, I never asked him what exactly was the source of that information, so it is lost forever... ;-) And, oh, BTW - that "yet older time" was like tad over 40 yrs ago, in case anyone wondered ;-) Cheers.

@@MrKotBonifacy Today i tried making copper hydroxide from sodium hydroxide and copper sulphate and was surprised with the black precipitate.. here i find the explanation

@@SandeepKumar-jj7zi So now you know... ;-)

If you add a small amount of copper sulphate to very concentrated sodium hydroxide it’ll actually go further and make copper (I) oxide!

Btw, can I know the exact amount of sodium hydroxide to copper sulphate to make the sodium copper hydroxide complex?

I think he chipped out the round hole on purpose for something but ye shure very impressive

+exotictoad Thanks :)

exotictoad the percentage of stupid people in the world is more than the double of thinking people. And stupid people likes to gossip much more than learning

5 years later, with almost 3 mil subs

Your profile picture matches with your comment. Lol. But now he have more than 3M subs.

Is this drugs???

I hope it is

@@vvv7565 w h a t

Ваня Листьев lmao

same, copper salts have a beautiful array of colors. dark blue, light blue, baby blue, black, black blue, green, green black, and even orange and red with some.

Just Another Emo On KZfaq orange?

@@mistertheguy3073 I looked it up and it may be a suspension of Cu2O

Copper triethanolamine thiocyanate is one of my faves. A brilliant emerald green complex

+Peter Powis I am glad i could help!

😂😂😂..well it was water which gave him yield greater than theoretical....

Aichybatoal but why does it break down into CuO and H2O when doing the direct reaction, and doesn't in the ammonia reaction?

False, H2O and NH3 are sigma donnor but NH3 is more π-acceptor than H2O and not" more donnor than H2O", because NH3 Is a ligand with strong field.. In fact: -Cu2+ is a d9 , so It is rich in electrons Complexes with copper +Il is light blue because There are d-d transition between t2g and eg ... BUT the dark blue is a result of d -> empty π of ligand ( and empty π can't be donnor )

love u

except that there's no oxidation, it was a mistake from nile. this is a dehydration reaction with the formation on an oxide.

Now, 5 years later, he have 4,5 mls subs

How well did it work?

kinda long, it took about 1 hour with constant stirring.

NileRed. NileRed does... oh ya, and me! The local high-school was shut down and it went up for auction. Scored ~2.5 banana boxes worth of equipment for $50 😁

+TheRedKnight I was going to ask that, as well. I think making a MgBr reagent would be really interesting.

MindoverManners I was thinking it might be cool if he made a metallocene polymer

+MindoverManners If he's willing to live dangerously, he should make tBu-Li and demonstrate air-sensitive procedures with it.

+TheRedKnight Ferrocene should be simple enough.

Id rather he stay alive

+zoolapin hey man, be nice.

just joking there!

zoolapin :)

Wym?

@@vivimannequin 1:38

+Cole Ramsey hello!

+Nile Red would you be able to do a video about making thermite with the manganese dioxide from lantern batteries?

@@timroberts9254 Late, but you'd probably need a LOT more manganese dioxide to make a proper thermite.

Lollollollollol

+Cole Ramsey NOOOOOOO :(

+Nile Red its almost too small to notice :)

+Cole Ramsey First thing I noticed. :P

+Nile Red i just checked and i have 16oz of 30% ammonium hydroxide from the science company!

Cole Ramsey Nice! Be careful with it though. Very strong stuff

+Esven Do you know how it is made?

+Esven Zinc stearate is used as a lube for photoconductive drums in photocopiers when they are being rebuilt.

+Nile Red Metallic stearates are all usually produced the same way. Stearic acid is saponified generally with sodium hydroxide. The resulting alkali stearate (in this case sodium stearate) is soluble in water and is diluted rather heavily because the higher the dilution the larger the reactive surface area as is the case with many other surfactant systems, and later the smaller the particulate size will be. Metal stearates are water insoluble so when they are synthesized directly by the addition of a metallic salt to the stearate solution the product precipitates out where it is then washed of all the remaining water soluble reactants. So the full order of operations starts with a pretty simple production of a zinc sulfate solution, either by addition of the salt to water or by using sulfuric acid with elemental zinc metal to produce the metallic salt. After that a sodium hydroxide solution in excess to the amount of stearic acid that is being saponified can be prepared. Once all the reactants are prepared the stearic acid can be melted at 70C and gradually saponified with the sodium hydroxide solution. As this happens it should go from an oily fatty acid to a water soluble soap. This mixture can then be diluted in water and gradually reacted with the zinc sulfate solution. If the solution has been prepared with sulfuric acid just keep in mind that the excess sodium hydroxide and the excess acid will neutralize one another. The product should precipitate out of solution and can be washed and dried. A few additional notes, be careful of aggressive stirring as there can be considerable foaming (As one would expect with a mix of soap and water) and the more dillute the reactants also the smaller the particle size, which can yield a finer powder more suited to showing the chemicals lubricating properties. An interesting alternative way of going about this might be to extract the ~8% sodium stearate content from deodorant sticks where it's used as a gellant, but I have no idea how difficult that might be. Anyway the reason I find this reaction interesting even though it's pretty much something a chem 101 student could grasp is primarily just to do with the interesting effects of working with surfactant systems and how the dilution, at least as the literature describes it, impacts the reaction rate to such a high extent. As well the compound itself is safe while possessing some rather unique physical properties. I suppose if you were so inclined and wanted to do something that might net a few more views a similar process could also be used to make aluminium salts of naphthenic acid and palmitic acid which in the Vietnam conflict were added to fuel oil as an 8-24% additive to produce napalm. The word napalm actually comes from these additives.

+trustthewater Damn, I should have also mentioned that

***** Unfrotunately i dont think they sell that in canada

That is true

I bought 2 kg of copper sulfate from RONA in Canada for $27 tx in. It needed to be recrystallized, as it had a significant amount of basic copper carbonate impurity and I think other impurities.