Making copper hydroxide
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- Опубліковано 2 жов 2024
- Apparently I made my $250 Patreon goal... I guess I have to commit for 6 months now?
Hey guys, today we make a little copper hydroxide for the purpose of making some Schweizer's Reagent to dissolve cotton!
That will be posted in a future video and it is actually a revisit of an old video.
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Nile talks about lab safety: • Chemistry is dangerous.
"The other ingredients are pretty basic" I see what you did there
+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.
Why do so many horribly toxic things in chemistry look so dang delicious to drink
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😅
I love vacuum filtration.
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
That's some very nice vacuum filter paper... It'd be a shame if someone... Schweitzer'd it.
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!
"How efficient are you?" " i always give 103%"
😂😂😂
"They're pretty basic" - sodium hydroxide pun?? Eh eh? like it
I know it's an old vid, but when I worked on making copper complexes, I ran in to info that the sodium hydroxide direct to copper sulfate turns to copper oxide, at least partially, due to the strong ph. You have to have an excess of copper sulfate, and add a more dilute NaOH slowly, then it will precipitate smoothly. On the flip side, if you add a large enough excess of NaOH, it will actually form a sodium copper hydroxide complex salt that will redissolve and if I remember right, is very dark blue, almost black, similar to the ammonia complex, but is a little different if you look at the 2 by eye. Hope it helps someone.
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?
these are really high quality demonstrations. thankyou
I binge your videos so often, they just so intereating and i learn stuff aswell. Just a win win, never a waste of time😌
I haven't taken inorganic chem yet, but I love the colors. It makes me really look forward to doing some reactions similar to this.
103%? You should start your gold busisness. You would have some gold times.😉😀.
😂😂😂..well it was water which gave him yield greater than theoretical....
Nile Red went a long path from a chipped 1l beakers to having his own lab. Well done!
I think he chipped out the round hole on purpose for something but ye shure very impressive
I love that blue
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 UA-cam orange?
@@mistertheguy3073 I looked it up and it may be a suspension of Cu2O
I can actually explain why it's better to add ammonia before precipitating the Cu(OH)2 with NaOH. The reaction of hexaaquacopper(II) to copper hydroxide is much faster than the reaction of tetraamminediaquacopper(II) to copper hydroxide (NH3 is a stronger ligand donor than H2O, making it a bit harder to pull off the metal center), and so impurities accidentally get trapped inside the product. If you first make the ammine complex, then the precipitation is slower, allowing for a purer precipitate! It's the same concept as recrystallization: if you're patient and let a crystal grow slowly, it will be more regular and pure than if you had just boiled off your solvent or something.
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 )
i just do not understand why you do not have more subs. your videos are fantastic and i learn something every time i watch them.
+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.
The problem with adding NaOH directly to the CuSO4 solution is temperature. The NaOH makes a lot of heat, which accelerates the oxidation to CuO.
Excellent video and great explanations!! I added NaOH to CuSO4 and wondered why the copper hydroxide was slimy and took forever to filter!! By the time I had filtered it and dried it out it was very dark green - I was disappointed that I really had Copper Oxide, not the Copper Hydroxide I wanted to make...I couldn't find explanations anywhere why my experiment had failed - so glad you posted this!! I now know why it went wrong and how to do it successfully!! Thanks!!!
+Peter Powis I am glad i could help!
He sound full of pride in this videos in comparison to actual videos
That magnet stir thing was neat, didn't even know those existed.
Is this drugs???
I hope it is
@@vvv7565 w h a t
Ваня Листьев lmao
16g of sdoium hydroxide
new stuff?
+zoolapin hey man, be nice.
just joking there!
zoolapin :)
Wym?
@@vivimannequin 1:38
I'm an IT guy and have very little knowledge about chemistry but instead of sleeping after work, I find myself enjoying this guy's videos. Very interesting!
Do you have any plans to do any organometallic reactions?
+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
"The other ingredients are pretty basic..."
Acid what you did there, mate!
1:06 *S D O I U M H Y D R O X I D E*
I Love you and the knowledge you have brought us.
I have some copper oxide that should be fairly pure. There may be aluminum or acetic acid contamination if any is present.
It's yours if you are interested.
(material state: Crystalline formation)
You're a great chemistry tuber, you're encouraging me to experiment with a few things I can use in my electronics hobby. Am currently making my own magnetical stirrer. I have purchased the proper stirring bars so the only part left is making the case for the motor holding the magnets.
oh my gosh thank you so much for this video and the dissolving cotton in schweizers reagent! i'm currently working on a chemistry experiment presentation and while trying different instructions i could never quite understand why my copper hydroxide looked so weird slimey and not fluffy bright blue when making it with naoh. i've been searching everywhere and now i know that i'm not doing anything wrong, it's just the way it is.
I had a teacher who read up online that if you add NaOH to CuSO4 directly to ppt out the hydroxide, other products are formed due to side reactions. And it pretty much always clumps together - gelatinous ppt, it isn't just you who has this problem. Anyway hope to see your next video!
Nicely done. I think I've said it before but copper salts are some of my favorite compounds because of the colors.
I'd like to see some more inorganic chem videos or maybe some videos on some of the rarer or stranger organometalic compounds.
And a Q&A video!
Copper triethanolamine thiocyanate is one of my faves. A brilliant emerald green complex
I will always love your channel
Imagine mixing this in someone's tide detergent
On the chemicals page it says 16g sdoium hydroxide
+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
Nilered loves me all, that means no love for you people, only me. Alright Niley, when are we tying the knot?
I just reacted table salt with H2SO4 and it makes a yellow liquid and the solution get cold and I can't see any gas being produced??? Just confused why...
I'm so jealous of your glasswear. Who has that big of a watch glass?
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 😁
there's a typo on the 'you will need' slide': "16g sdoium hydroxide"
Lollollollollol
Can you make a video about Phosphine gas? It's very interesting. You should also make a video about interhalogenes.
You really want Nile to risk his life for you?
+Quintinohthree You mean with the interhalogenes? I wasn't speaking about ClF3 just about the safer ones like ICl3. Or do you mean phosphine? I don't think it would be as dangerous. It is similar to silane (pyrophobic) but a bit more reactive.
+Quintinohthree Its okay. I will sacrifice myself for science. Seriously though, i dont want to make phosphine. I don't feel safe enough doing that. That goes for HCN and other poisonous gases
+Nile Red But what about interhalogenes?
Garabos 053 I might eventually look into messing around with those
I think you've made Cu2(OH)2SO4 not Cu(OH)2, because Cu(OH)2 decomposes quickly when stored and is a bit darker than your precipitate.
always great colors going on with copper
The reason why the solution turns black if you add NaOH directly to CuSO4 is because it is an acid/base reaction that produces a lot of localized heating. The higher temperature favors the oxidation of the copper to CuO (black precipitate).
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.
thank you
"After all the stuff has been added to the beaker"
Me: hehe cool blue
A nitrous oxide video would be pretty funny
Yield: 103%
Lego: perfect.
That blue 🔥
Copper Hydroxide appears to be delicious.
Great video Nile. Question though, how did ammonia "turn" into ammonium? I assume it got a proton from the water, since it's a base?
Also, the reaction on 3:10 there, precipitation and a redox reaction?
The left over blue solution can be the copper ammonia complex & it can be converted to copper hydroxide by adding NaOH again to it :);)
Nice video. Can you make a video on making copper oxide 2 or copper oxide black powder that we use in fireworks to make blue stars. ? Be great the cheapest and easiest way possible. Thanks dude.
It would be awesome if you did online lectures im chemistry!
Can u do a video on preparation of dimethyldichlorosilane and its following uses and hydrolysis reactions. I use it at work and have done a little reading but would be cool to see what u can find on it.
Jesse! We have to cook.
🤔 So between this and piranha... The mob has a new cleaner crew 😂
I'd like to see you make glass water.
I thought cuso4 + naoh will do the trick.. why there is a need for ammonia.
Updated: he explained it in the video
Someone now what is the equation of the reaction between the [Cu(NH3)4(H2O)2](OH)2 and the NaOH? I would be thankful.
Can You do a Video using electrolysis to Synthesize Copper Hydroxide?
I recently had to make copper oxide and I used this method to separate my copper from my manganese and copper salt mixture, made copper hydroxide and heated it up to decompose it to copper oxide. I am a final year student in South Africa =)
at 0:18 it looked liked windows 11 wallpaper
@nilered a 100g serving of Maitake mushrooms contain roughly 28% of our daily value of Cu. Can you extract copper ions or even raw copper from mushrooms?
By my rough and generalized calculations if this is possible, 400g of maitake (wet) could produce about 1.008g of copper. It would take roughly 395oz to make 1oz of Cu.
Nile, you can make copper hydroxide by electrolysis right? Copper electrodes and water with magnesium sulfate(epson salt)?
And also Sodium Hydroxide can be created my electrolysis of salt water? (Along with chlorine gas of course)
I guess this is technically an experiment anyone could do with ammonia on hand, but I suppose the creation of sodium hydroxide might be dangerous for many, who fail to take precautions to the creation of chlorine gas.
Cellulose was a strange word untill I realized what it is (English is my second language afrikaanse is my first)
It's funny how your Canadian accent is noticeable in your older clips.
10% cleaning ammonia in your country ? Best I can get is 2%.
Robert Heal yay communism
I noticed that your beaker has a missing piece.
Going to add it to a one litre beaker that has a chip in it
I've found Cu(OH)2 precipitated from NaOH decomposes to CuO quite easily.
Could you make Benedict's reactive
Where do you get your chemicals? I was planning to order through Flinn Scientific, but I am neither a school nor a teacher. Any affordable and easily accessible suppliers?
+Nicolas Giandrea It really just depends on what chemical you want and how much effort you're willing to put in to get it. A lot of things you could buy directly off of eBay, but you may not always get the best quality. It seems like a lot of common chemicals/materials can also be extracted from products you can get at Lowes or a pool supply store. Of course, if you can find an online chemical supplier that doesn't require you to have a business, that's great, but know that some of them charge way more than eBay sellers for the same product with often insignificant quality differences.
Duda Diesel is also a good supplier, but they're kind of limited in what they offer since they're focused on biodiesel applications. I've ordered acetic acid from them twice though (and one magnetic stirrer), and it always came perfectly fine.
+Nicolas Giandrea The Science Company is a good place to order chemicals. You can see in this video that Nile bought his ammonia from The Science Company.
+Eli Wiel Yup. To ship to Canada too it only cost me like a total of $120 :(
everyone in the lab chill until *1 0 3 % Y I E L D*
I did a chemistry project a few months back where I had to make 3 grams of Cu(OH)2. I see why you used the ammonia with it. Adding the NaOH directly didnt make a light blue color and when we dried it in an oven, it became very hard and brown since it oxidized. We were able to vacuum filter it, but not for long, but we should've done it longer as we would've had the percipitate
It’s 2am. Help.
"cellulose is in the paper you write on"
**me dissolving that paper in water**
I wouldn't be surprised if this was once used or still is used as a paint pigment. Many paints were quite toxic historically, some still are.
Do you know how to make brady's reagent?
Is this the same stuff that formed during my electrolysis with copper as anode and iron as cathode
while water and baking soda solution was my electrolyte.
why am i watching this, im not a chemistry student....
How to make poly aluminium chloride
4:25 it’s so cool it looks like it’s glowing!
0:30 so i eat paper = don't have to eat fiber?
"sdoium hydroxide" think thats supose to be sodium hydroxide :P
I know the solution of copper hydroxide will probably kill me but I wanna drink it. Look at that color
No worries, I thank you for your time, and for the great video's
Where did you buy that vacuum filter? I urgently need one
Reagent instead of "reaijent"
Scholizerz
Clouthinaket
Copper hydroxide could be mixed with graphite to make a very hood anode paste for use as a battery. Cathode can be any reactive metal. 1.8V for zinc 2.4V for aluminum, 2.6V for magnesium and 1.2V for iron. Electrolyte is KOH or NaOH solution.
Stump remover is made from potassium nitrate. What you want to buy at the stores is called Root killer.
how do clean the glass vacuum filter?
Don't let the anomia hydroxide float(a joke )(I can't tell jokes)
It's sad that you only have ~100.000 followers. :( I think you deserve way more than Nurd Rage or others because you put tons of afford into your videos and clearly show the procedure. Thanks for making videos. Keep going!
Now, 5 years later, he have 4,5 mls subs
And how can you get the peptides from copper? Can you make a video?
I love how you say Schweizer...
when i did the exact (almost, different ammonia) process, my end product was dark blue not light blue. help!!!!!!!!!!!!
Nevan's lab maybe you didn't wash it so well and it got contaminated with some copper sulphate
Make copper azole wood preservative
1:32 Now for the other ingredients they're pretty basic.
I see what you did there ^-^
3:24 Had a stoke on a chemical
Why does my copper hydroxide always turn to a dark greenish color?
omegadelta phoenix yeah but what is it contaminated with
ZThesixeZ it happened to me too using CuSO4 and NaOH. It's because it breaks down into CuO and water. The copper (II) oxide is black, and so the stuff takes on that color.
I'm a bit surprised, that direct NaOH give bad quality.
Have you tried different dilution? Inert atmosfere (N2).
Different temperatures?
Maybe start with CuCl2?
And adding excess of NH3 in first step, when you really want Cu(OH)2 - maybe it's not necessary?