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.
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
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
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.
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.
