We left the solution to evaporate over a period of several weeks in another experiment, and a very crumbly white precipitate eventually formed. We may have formed a solution of tricalcium aluminate as well, seeing as the precipitate did resemble one of the mineral phases in Portland Cement, which is a variety of cement which uses calcium aluminates.
This is or is nearly the mixture added to finely ground sand and Portland cement to leaven concrete before it is steam cured into AAC blocks (aircrete). they ad the aluminum in a powder form, though.
Thank you for sharing this experiment. Also thank you for wearing that shirt. XD I ordered some calcium hydroxide in the mail, and i'm using a similar method to test if it is indeed CaOH2. This video was insightful for me in preparing my experiment. Good work.
In my experiment I started with a piece of aluminum bar. I filed away a small, flat area to remove the oxide layer and expose the aluminum metal. Then I placed a small ammount of Calcium Hydroxide onto the surface. Then carefully hydrated the powder by dropping water onto it with a syringe. Once wet the slurry began to bubble. After 10 minutes I wiped away the slurry, and rinsed the aluminum bar with warm water. I scrubbed the area with wet paper towel to remove any residue. When viewed under magnification I could see a thin layer of hard white material. So for my purposes I've verified that this chemical is probably Calcium Hydroxide. Next i am doing the CO2/limewater test.
thanks for seeing the experiment, i havent actually touched cal hydrox yet. but ive got some on the way, i wonder if it sets aluminium sulfate any good, or is it a non cementer because aluminium hydroxide its too water insoluable.
So basically that is a 10% solution - a double replacement reaction would not occur because you have used an elemental not a salt. There would be a slight evolution of hydrogen. Good principles and practices of chemistry demonstrated…👍
I am doing this experiment right now -tiny bubbles forming on the aluminium in my test tube. I am as lost as you guys are and learned as much you do, from wikipedia But I am just happy I AM getting aluminium to react for the first time! Do tell me If you guys have found something more about this reaction!
If you do it the same as us you should form a compound like a primitive concrete at the end. We think the actual compound is tricalcium aluminate (Ca3Al2O6), but we're not sure. If you find anything interesting about this we'd love to hear!
Al(s) + Ca(OH)₂(aq) → Al(OH)₃(aq) + Ca²⁺(aq) E° = E°(reduction) - E°(oxidation) = -1.55 V - (-2.87 V) = 1.32 V Also produce H₂(g) cause electrolysis of water start at 1.23 V.
Elementary aluminum is not (3+) - it can have different oxidation states, tricalcium aluminate requires a lot of energy to be formed and it reacts instantly with water to form calcium hydroxide. I understand the experimental nature of this but you should have at least used ionic aluminum if thats what you figure and write down. Give a disclaimer if you don't know what you're doing (which is totally fine) to prevent misinforming ppl (less fine). Also dropping something like that into a strong basic solution seems like a good way to jet some of the suspension into your eyes, that one unlucky time. Which would be unfortunate if you're not wearing any goggles. happy experimenting ;)
We left the solution to evaporate over a period of several weeks in another experiment, and a very crumbly white precipitate eventually formed. We may have formed a solution of tricalcium aluminate as well, seeing as the precipitate did resemble one of the mineral phases in Portland Cement, which is a variety of cement which uses calcium aluminates.
Has its temperature been rising?
This is or is nearly the mixture added to finely ground sand and Portland cement to leaven concrete before it is steam cured into AAC blocks (aircrete). they ad the aluminum in a powder form, though.
Thank you for sharing this experiment. Also thank you for wearing that shirt. XD I ordered some calcium hydroxide in the mail, and i'm using a similar method to test if it is indeed CaOH2. This video was insightful for me in preparing my experiment. Good work.
Thank you, and good luck with your research!
In my experiment I started with a piece of aluminum bar. I filed away a small, flat area to remove the oxide layer and expose the aluminum metal. Then I placed a small ammount of Calcium Hydroxide onto the surface. Then carefully hydrated the powder by dropping water onto it with a syringe. Once wet the slurry began to bubble.
After 10 minutes I wiped away the slurry, and rinsed the aluminum bar with warm water. I scrubbed the area with wet paper towel to remove any residue. When viewed under magnification I could see a thin layer of hard white material. So for my purposes I've verified that this chemical is probably Calcium Hydroxide. Next i am doing the CO2/limewater test.
thanks for seeing the experiment, i havent actually touched cal hydrox yet. but ive got some on the way, i wonder if it sets aluminium sulfate any good, or is it a non cementer because aluminium hydroxide its too water insoluable.
instead of crumpling the foil into a pill shape, would more surface area = better reaction? just a theory, great video!
Just found your channel - Great content! Subscribed - _with_ notifications, lol.
Please keep making videos :-)
That lab coat tho
So basically that is a 10% solution - a double replacement reaction would not occur because you have used an elemental not a salt. There would be a slight evolution of hydrogen. Good principles and practices of chemistry demonstrated…👍
شكرا 🌼
I am doing this experiment right now -tiny bubbles forming on the aluminium in my test tube.
I am as lost as you guys are and learned as much you do, from wikipedia
But I am just happy I AM getting aluminium to react for the first time!
Do tell me If you guys have found something more about this reaction!
If you do it the same as us you should form a compound like a primitive concrete at the end. We think the actual compound is tricalcium aluminate (Ca3Al2O6), but we're not sure. If you find anything interesting about this we'd love to hear!
Al(s) + Ca(OH)₂(aq) → Al(OH)₃(aq) + Ca²⁺(aq)
E° = E°(reduction) - E°(oxidation)
= -1.55 V - (-2.87 V)
= 1.32 V
Also produce H₂(g) cause electrolysis of water start at 1.23 V.
hey dudes so what what the final result besides the calcium powder at the end as leftovers what was actully formed?
We think its tricalcium aluminate (Ca3Al2O6), but we haven't confirmed that. We'll probably revisit this. It formed a primitive concrete.
you have a high chance of disaster making nitro glycerine, but its kinda the same thing as this i think.
Good job guys.
Elementary aluminum is not (3+) - it can have different oxidation states, tricalcium aluminate requires a lot of energy to be formed and it reacts instantly with water to form calcium hydroxide. I understand the experimental nature of this but you should have at least used ionic aluminum if thats what you figure and write down. Give a disclaimer if you don't know what you're doing (which is totally fine) to prevent misinforming ppl (less fine). Also dropping something like that into a strong basic solution seems like a good way to jet some of the suspension into your eyes, that one unlucky time. Which would be unfortunate if you're not wearing any goggles.
happy experimenting ;)
Sooty flame. You didn't burn solution
According to my knowledge it is impossible to make 1 mol solution of Calcium hydroxide.
Because it's not soluble? Yeah, I think he means suspension, not solution.
Love the shirt!!!
Bro. That shirt. I want it. 🤣
self-heating bag
Who is watching in 2022😂
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Matthew Petrick not me
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this the ingredients for concrete...