Hi, Nice video. I have 3 comments about your experiment. 1°) Your iron nail may be galvanized (Zinc coating corrosion inhibitor that protect the iron from straightforward rusting... Zn serve as sacrificial metallic reducer to restore any corroded iron spot) This doesn't interfere with your experiment since Zn is above Fe in reducing power just like iron is above copper. So Cu(2+) remains the more oxydant cation vs Fe(2+) and Zn(2+)... This means that at first you get fast dissolution of colorless ZnSO4 and precipitation of Cu(0)... then green FeSO4 and more Cu(0). 2°) The green Fe(2+) tends to oxidize upon contact with air (or dissolved O2 from the air) to produce yellow/orange/red Fe(3+). What is observed into your open to the air tube. Fe2(SO4)3 is slightly acidic when into solution and does form at least partially red rust and sulfuric acid. Fe2(SO4)3 + 6H2O 2Fe(OH)3 + H2SO4... Part of the red mud supposed to be cemented Cu(0) may thus be rust (iron (III) hydroxide). 3°) You of course know that inox metal often contains Fe/Cr/Ni by decreasing %. All 3 metals are more reducing than Copper... (Cr>Fe>Ni) In principle your inox spoon must have been coated by reduced copper while swirling to dissolve your CuSO4... meanwhile you have some Cr(3+) \ Fe(2+) \ Ni(2+) sulfates - all 3 in different shades of green - that did pass into solution. PHZ (PHILOU Zrealone from the Science Madness forum)
Thanks sir very Informative, 1. Sir can we increase the amount of water(solvent) to dissolve CuSO4 completely in water? 2. If CuSO4 is not completely dissolved in water then does it will affect reaction?
1. Yes, you can increase the amount of water (solvent) to dissolve CuSO4 (copper sulfate) completely. The solubility of a compound, such as CuSO4, is often affected by temperature and the amount of solvent present. Generally, increasing the amount of solvent, in this case water, can help increase the amount of solute (CuSO4) that can dissolve. Copper sulfate is relatively soluble in water. If you add more water to a given amount of CuSO4, it will provide more space for the CuSO4 molecules to spread out and interact with the water molecules. This can lead to more CuSO4 molecules dissolving in the water until the solution becomes saturated. However, it's important to note that there's a limit to how much solute can dissolve in a given amount of solvent at a specific temperature. Once the solution becomes saturated, further addition of CuSO4 will not dissolve, and any excess CuSO4 will settle at the bottom of the container. If you're trying to dissolve a larger amount of CuSO4 than seems to be dissolving in a certain volume of water, you might need to increase the amount of water, stir the solution to help facilitate the dissolving process, and potentially adjust the temperature (if the solubility is temperature-dependent). Just remember that even though you can increase the amount of water to increase the potential for dissolving, there is still a limit to how much CuSO4 can dissolve in a given volume of water. 2. Yes, the degree to which CuSO4 (copper sulfate) is dissolved in water can affect reactions that involve this compound. The solubility of CuSO4 in water determines the concentration of copper ions (Cu²⁺) and sulfate ions (SO₄²⁻) present in the solution. These ions play a crucial role in various chemical reactions. If CuSO4 is not completely dissolved in water and there is undissolved solid present, it can impact reactions in a few ways: Reaction Rate: Reactions involving dissolved ions can occur more readily than reactions involving solid particles. If CuSO4 is not fully dissolved, the reaction might proceed more slowly because the ions have limited contact with the other reactants. Stoichiometry: The amount of CuSO4 available for reactions will be determined by the amount that has dissolved. If only a portion has dissolved, the stoichiometry of the reaction might be affected, leading to incomplete or unexpected products. Equilibrium: For reactions that reach equilibrium, the concentration of dissolved species can impact the position of the equilibrium. If the concentration of copper or sulfate ions is lower due to incomplete dissolution, the equilibrium might shift, affecting the overall reaction outcome. Precipitation Reactions: In some reactions, if the concentration of dissolved ions exceeds their solubility product, a solid precipitate can form. If not all of the CuSO4 is dissolved, the potential for such precipitation reactions might change. To optimize reactions involving CuSO4, it's generally preferred to work with fully dissolved solutions. This ensures that the concentrations of the relevant ions are accurately controlled and that the reaction kinetics are not hindered by undissolved solids. If complete dissolution is not achieved, the reaction conditions might need to be adjusted or further steps taken to promote dissolution, such as increasing the amount of solvent, stirring, or adjusting the temperature.
hi sir, pls can u confirm whether copper is reddish brown or pink in colour. bcaz in the net its reddish brown but in this video it is pink .i was astonished good vids sir keep it up
I have one doubt citric acid+bakingsoda+sulphuricacid+magnesiumhydroxide all two neutralization in one test tube then what is our final product in the end can you creat a video on it please
When you mix citric acid, baking soda, sulfuric acid, and magnesium hydroxide in a test tube, a series of chemical reactions will occur. Let's break down the reactions step by step: Citric acid (a weak acid) reacts with baking soda (sodium bicarbonate, a base): Citric acid + Baking soda → Sodium citrate + Carbon dioxide + Water The produced carbon dioxide gas will likely bubble out of the solution. Magnesium hydroxide (a base) reacts with sulfuric acid (a strong acid): Magnesium hydroxide + Sulfuric acid → Magnesium sulfate + Water The final products of these reactions would be sodium citrate, magnesium sulfate, water, and carbon dioxide gas. However, since the reactions involve various substances and conditions, the exact outcome could depend on the quantities and concentrations of the reactants, the temperature, and other factors. Please note that mixing strong acids and bases like sulfuric acid and magnesium hydroxide can be potentially hazardous, as they can react vigorously and release heat. It's important to handle such chemicals with care and avoid creating mixtures that could lead to dangerous reactions.
Sir I have a doubt if amount of iron is same that of cuso4 then same amount of copper that of the iron is formed or iron completely displace cu and cu becomes the nail?
Quantity does not matter because after certain amount of time copper is over deposited on the surface of iron nail so ion nail items from inside cannot come out for the reaction
Sir I Have A Question, Can We Add Something (metal or non metal compound) to speed up the deposition of copper on iron nail and formation of ferrous sulphate as it took the whole night to deposit.
Excuse me but is there a way to increase the structure of the copper and make it a large monocrystal? Or tell me what is the main factor that can make a large monocrystal of the copper please
![[LIVE] : ONE ลุมพินี 88 | คู่เอก "ป้อมเพชร vs อัสลามจอน"](http://i.ytimg.com/vi/1ZqTVVbMgbo/mqdefault.jpg)
Who is here from 10th standard 😊
I'm from next toppers too
@@timepasplayz4268 me too 😛❤️🇮🇳
Grade 7th💀
Me 7th 😁
I'm in seventh grade learning MOLE CONCEPT
I owe the development of My practical skills in science during this pandemic to You.
Thank you 🙏🏻
Hi,
Nice video.
I have 3 comments about your experiment.
1°)
Your iron nail may be galvanized (Zinc coating corrosion inhibitor that protect the iron from straightforward rusting... Zn serve as sacrificial metallic reducer to restore any corroded iron spot)
This doesn't interfere with your experiment since Zn is above Fe in reducing power just like iron is above copper.
So Cu(2+) remains the more oxydant cation vs Fe(2+) and Zn(2+)...
This means that at first you get fast dissolution of colorless ZnSO4 and precipitation of Cu(0)... then green FeSO4 and more Cu(0).
2°)
The green Fe(2+) tends to oxidize upon contact with air (or dissolved O2 from the air) to produce yellow/orange/red Fe(3+). What is observed into your open to the air tube.
Fe2(SO4)3 is slightly acidic when into solution and does form at least partially red rust and sulfuric acid.
Fe2(SO4)3 + 6H2O 2Fe(OH)3 + H2SO4...
Part of the red mud supposed to be cemented Cu(0) may thus be rust (iron (III) hydroxide).
3°) You of course know that inox metal often contains Fe/Cr/Ni by decreasing %.
All 3 metals are more reducing than Copper... (Cr>Fe>Ni)
In principle your inox spoon must have been coated by reduced copper while swirling to dissolve your CuSO4... meanwhile you have some Cr(3+) \ Fe(2+) \ Ni(2+) sulfates - all 3 in different shades of green - that did pass into solution.
PHZ
(PHILOU Zrealone from the Science Madness forum)
Mr Louis Thank You for watching the video.
I am really grateful to you for writing and binging into my notice. Thank you
First time in life I saw this reaction.Thanks a lot!!
Really......'cause reactions are all around us!!!
Same here
MIND BLOWING TEACHING GURUJI ........... RADHEY RADHEY ........... AWESOME TEACHING SIR ............ 🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻
Thank you for your compliments 😊
These video's are very helpful, thank you
Really amazing. U r doing such a great job
Thanks sir very Informative,
1. Sir can we increase the amount of water(solvent) to dissolve CuSO4 completely in water?
2. If CuSO4 is not completely dissolved in water then does it will affect reaction?
I don't think we need to add water but with time it will dissolve it self
U think too much
@@barkatalimunshi770 But what if the solution is saturated
1. Yes, you can increase the amount of water (solvent) to dissolve CuSO4 (copper sulfate) completely. The solubility of a compound, such as CuSO4, is often affected by temperature and the amount of solvent present. Generally, increasing the amount of solvent, in this case water, can help increase the amount of solute (CuSO4) that can dissolve.
Copper sulfate is relatively soluble in water. If you add more water to a given amount of CuSO4, it will provide more space for the CuSO4 molecules to spread out and interact with the water molecules. This can lead to more CuSO4 molecules dissolving in the water until the solution becomes saturated.
However, it's important to note that there's a limit to how much solute can dissolve in a given amount of solvent at a specific temperature. Once the solution becomes saturated, further addition of CuSO4 will not dissolve, and any excess CuSO4 will settle at the bottom of the container.
If you're trying to dissolve a larger amount of CuSO4 than seems to be dissolving in a certain volume of water, you might need to increase the amount of water, stir the solution to help facilitate the dissolving process, and potentially adjust the temperature (if the solubility is temperature-dependent). Just remember that even though you can increase the amount of water to increase the potential for dissolving, there is still a limit to how much CuSO4 can dissolve in a given volume of water.
2. Yes, the degree to which CuSO4 (copper sulfate) is dissolved in water can affect reactions that involve this compound. The solubility of CuSO4 in water determines the concentration of copper ions (Cu²⁺) and sulfate ions (SO₄²⁻) present in the solution. These ions play a crucial role in various chemical reactions.
If CuSO4 is not completely dissolved in water and there is undissolved solid present, it can impact reactions in a few ways:
Reaction Rate: Reactions involving dissolved ions can occur more readily than reactions involving solid particles. If CuSO4 is not fully dissolved, the reaction might proceed more slowly because the ions have limited contact with the other reactants.
Stoichiometry: The amount of CuSO4 available for reactions will be determined by the amount that has dissolved. If only a portion has dissolved, the stoichiometry of the reaction might be affected, leading to incomplete or unexpected products.
Equilibrium: For reactions that reach equilibrium, the concentration of dissolved species can impact the position of the equilibrium. If the concentration of copper or sulfate ions is lower due to incomplete dissolution, the equilibrium might shift, affecting the overall reaction outcome.
Precipitation Reactions: In some reactions, if the concentration of dissolved ions exceeds their solubility product, a solid precipitate can form. If not all of the CuSO4 is dissolved, the potential for such precipitation reactions might change.
To optimize reactions involving CuSO4, it's generally preferred to work with fully dissolved solutions. This ensures that the concentrations of the relevant ions are accurately controlled and that the reaction kinetics are not hindered by undissolved solids. If complete dissolution is not achieved, the reaction conditions might need to be adjusted or further steps taken to promote dissolution, such as increasing the amount of solvent, stirring, or adjusting the temperature.
Thank you sir.. this really helped me with my practicals 🙏🏻
Most welcome!
Jis din India ki ratta mar education policy badlegi us din aapke million main subscriber honge
Thanks🙏
Thank you so much sir
i was so confused when I saw the reaction I was confused but this helped me a lot
I mean this ain't confusing if u wana really get confused look at mole concept😢
hi sir, pls can u confirm whether copper is reddish brown or pink in colour. bcaz in the net its reddish brown but in this video it is pink .i was astonished good vids sir keep it up
Yes
I meant Reddish brown...but in some textbooks you will find pink
Very informative
Thank you sir
It was uploaded 3 yrs ago and now I'm watching it in 2024
Hey, you should avoid using a metal spool Bcs it interferes with the reaction!
Very true
*Wonderful Presentation Sir*
Thanks Sir. Your vedios are always sir unparrallel, knowledge imparting and really helpful. Allah bless you sir.
🙏
Sir please post a video of rice pulling in old copper coins and mention that what are the chemicals needed for that and make it has an experiment
I am unaware of this process. Sorry
Thank you sir it's pleasure to see this. , Hope you get 1 million soon , loving from KSA , Riyadh
Thanks🙏
Yes
what a respect! THE COPPER SULPHATE SOLUTION However,nice video
So easy and helpful experiment. Thank you
Sir U are saying that "See the deposition of pink colour in the iron nail" but exactly it's brown in colour.....
Thanks for correction
Not worry in Science when you tube is available.
Wow
hope you reach till 1m likes and views
This helpful for my study thank you 😊😊😊😊😊😊😊
What is the nature of cu deposited is t hard flaky,soft
soft
Thank you , for such a helpful video sir .
Sir please tell me how to make @ anti iron gel.
I don't know. Thanks for watching the video
sir the copper deposition is totally pure copper or not ?????
Yes pure copper
Sir is the solution acidic in nature or basic in nature
Neutral
Very nice sir... Thank you...
Sir we want double displacement reaction pls 😭🙏
Its there please check precipitation reaction in chemistry play list
@@MakeMeScientific sure sir
I have one doubt citric acid+bakingsoda+sulphuricacid+magnesiumhydroxide all two neutralization in one test tube then what is our final product in the end can you creat a video on it please
When you mix citric acid, baking soda, sulfuric acid, and magnesium hydroxide in a test tube, a series of chemical reactions will occur. Let's break down the reactions step by step:
Citric acid (a weak acid) reacts with baking soda (sodium bicarbonate, a base):
Citric acid + Baking soda → Sodium citrate + Carbon dioxide + Water
The produced carbon dioxide gas will likely bubble out of the solution.
Magnesium hydroxide (a base) reacts with sulfuric acid (a strong acid):
Magnesium hydroxide + Sulfuric acid → Magnesium sulfate + Water
The final products of these reactions would be sodium citrate, magnesium sulfate, water, and carbon dioxide gas. However, since the reactions involve various substances and conditions, the exact outcome could depend on the quantities and concentrations of the reactants, the temperature, and other factors.
Please note that mixing strong acids and bases like sulfuric acid and magnesium hydroxide can be potentially hazardous, as they can react vigorously and release heat. It's important to handle such chemicals with care and avoid creating mixtures that could lead to dangerous reactions.
Sir I have a doubt if amount of iron is same that of cuso4 then same amount of copper that of the iron is formed or iron completely displace cu and cu becomes the nail?
Quantity does not matter because after certain amount of time copper is over deposited on the surface of iron nail so ion nail items from inside cannot come out for the reaction
Sir I Have A Question,
Can We Add Something (metal or non metal compound) to speed up the deposition of copper on iron nail and formation of ferrous sulphate as it took the whole night to deposit.
It's a fast reaction but to get more amount of iron I waited for whole night. Still i will get back
@@MakeMeScientific Ok Sir,
Understood it well now.
Thanks a lot
I have a question that why does at last the iron sulphate turned green after the decomposition of copper on the nail ?
The color of iron sulphate formed is green that's why
Thank you sir 👍 for doing lots for us
NICE VIDEO
Excuse me but is there a way to increase the structure of the copper and make it a large monocrystal? Or tell me what is the main factor that can make a large monocrystal of the copper please
kindly refer to
www.ecowatch.com/solar/monocrystalline-vs-polycrystalline
Fe2S+H2SO4 ka bhi experiment kijiye
Ok will try asap
I have a question. You said iron sulphate is green in color, then why after keeping it overnight it color changed to yellowish ?
On heating, ferrous sulphate crystals lose water and anhydrous ferrous sulphate (FeSO4) is formed. So their colour changes from light green to white
@@MakeMeScientific but u didn't heat it right ?
What chemical can make iron metail (Nail) brittle and easy to brake
Carbon
It's really so helpful
Sir what is the procedure in CuSO4 + Fe nail?
It's a single displacement reaction. Please check theory for more details
Cool 🤩🤩
my name is Hirishikesh iam studying 7std in this video my science book also there the chapter name is physical and chemical change
Good luck with your studies 👍
U are a scientist
Awesome 😊🙏🙏🙏🙏🙏🙏🙏🙏🙏
Thanks you for the video
Sir nice video sir can you make video on potassium iodide
Its there please check chemistry playlist
7:35 Sir ye copper pink nhi Brown dekh rhi ha.
Yes actually dark pink ya brown dono sahi he
Nice sir
sir this is the really same colour of rust so sir can u plz tell me is this rust
No this is different from rust although the colour of yours the same rust is iron oxide where is this is copper
What copper sulphate are always in blue colour
Yes
But, Sir why its fully not Green Why the upper part is only green??
The entire solution turns green after about an hour. This observation was after 10 mins
👍👍👍
Which chemical used to Anti iron
Hydroxy(thio)pyrone and hydroxy(thio)pyridinone
Sar hydrogen hydride ko kaise regional head duplicate
Very very helpful
Nice vdo
Can u pls explain what is mixactive metal
I am unaware sorry
You know gohil sir from rajkot
Sorry I dont know..
How much time is required for this reaction?
About 2 mins
Do we need not add acid?
No
Thanks sir❤️❤️❤️❤️❤️
What is the name of anti iron chemical liquid
Hydroxy thio pyrone
What are the reactants in this
Please see chemical reaction show in the video
Thank u so much sir 😊😊
What the iron nail colour
is faded
As copper is displaced by iron and iron turns into iron sulphate which is green
I saw this experiment because I like to see a nice green solution 😁
Sir please tell me anti_iorn chemical reaction to coper
I am unaware sorry
Sir how can I make a Anti Iran in copr coin
Hydroxy(thio)pyrone and hydroxy(thio)pyridinone
Great 👍
7th wala like karo
Thanks
I read in text book dil h2so4 is adding. Why
It's not required
Thanks sir
Thank you
thanks a lot
Nice
Cu ka pink colour nahi dikha experiment mai
Dark pink or brown
Sir iron nail brown kyu hogyi?
due to deposition of copper on its surface
Omggg
Dhruva sarja
Who is from 7th grade
I'm from 7th
I am from 9th
I am from 7th
,✍️✍️✍️✍️✍️✍️
Anyone from 8th standard ???
Yes!!
Hi sir
hello
Sir you have repeated this topic twice.
Thanks. But i dark green color was not visible in previous video. So again repeated
Yes sir
Sir apka no. milega
Email kijye
kunal619connecting@gmail.com
Me
Thank you
Nice
Thanks