That’s definitely the VERY OLD fashioned way! Except the product is nowhere near pure, containing oxygen (metabolism is not 100% efficient!), water vapor, nitrogen, and whatever your digestion and/or metabolism created from your last few meals. Even acetone perhaps!
I always like videos where you guys screw something up best. It reminds us that academia is a human pursuit, and you always seem to treat failure as an opportunity for humor and learning.
Professor Poliakoff's idea of "let's add some visual flare" is so awesome. Though things didn't work out, the idea that he thought, "Hey, let's make some colors happen" makes me, as a viewer, grateful to him for caring about us!
I love watching chemistry not go as planned just as much as watching it work out. Because then, it really gets the ol' gears working and makes you think more. Cool stuff.
So glad you posted this. We just had one of these donated to our high school chemistry program with a load of older glassware and had no idea what it was for.
Steve Read and yet there’s a shortage affecting North America, i can no longer get diet dr. Pepper, and several different brands of pop are disappearing from store shelves.
Weak acids like H2CO3 don't displace sulphate and nitrate from metals very well. It might have worked better with copper and lead acetates, or salts of some even weaker acid. Succinates, perhaps.
The reason why the first tests with the transition metals didn't work is because the anions were all those of strong acids, and thus, poor conjugate bases. In order for gaseous or dissolved carbon dioxide to form carbonate or bicarbonate ions in solution, the presence of hydroxide ions in the water is necessary. Since the anions of the salts used don't pull protons off of water molecules very well, hydroxide ions will be rare. Additionally, transition metal cations are actually relatively strong Lewis acids (hence why they form precipitates with carbonate/bicarbonate and hydroxide ions), and so their solutions will have a relatively low pH, decreasing, even further, the concentration of hydroxide ions in solution.
stinooke At the same time, you're also removing electrons from water to form oxygen gas. While pH/pOH values for areas surrounding the electrodes shift due to the influx of electrons at the cathode (lowering pOH) and the loss of electrons at the anode (lowering pH), the overall acidity/basicity of the solution will remain unchanged.
Liter is not an SI unit. It is an acceptable unit, but strictly speaking there is no SI unit for volume, because cubic decimeter is after all, just meters. Sort of like SI seconds. Hours are not SI units, hours are just bunches of seconds.
What a great teacher and person! Professor Poliakoff with all his experience and knowledge is humble enough to say in the video that he might be wrong. This is the best colorful solution! :)
Destin just achieved greatness in my book. It wasn't the tour of the ISS, it wasn't fist bumping Obama, it was being blessed enough to touch the professors spectacular hair.
Used to love Kipps apparatus. We had one at school and also in the first laboratory I worked in a histology lab. Also had them in several schools I worked in later, we also used one for generating hydrogen sulphide.
I absolutely love the professor's honesty and modesty of admitting he got the chemistry wrong. Not one bit of ego or shamefulness, sending a clear message that all humans are prone to error, no matter how experienced or educated they are. That's what being a scientist is all about! You have my sincere admiration, Prof' Poliakoff. You're setting a wonderful example of scientific integrity. :-)
I love old tech and methods. You can learn a lot from obsolete things like this, Not to mention how interesting and cool it is. Thanks for sharing this with us!
The carbonate (CO3-2) has to be free in order to react with Cu2+. CO2 + H2O-> H2CO3-> H+ + HCO3-. The second deprotonation is too weak to produce substantial amounts for carbonate. If it was in a strong base, it might work. However, there you would have precipitation of hydroxides.
Seeing the Kipp's apparatus brought back memories of Chemistry lessons in the 1960s including one where the apparatus had a bung in the side of the bottom vessel, presumably to enable it to be drained easily. The bung was, of course, pushed firmly in place, or should have been. During one lesson it came loose and acid flooded out across the bench and down the front of one of the pupils. Our Chemistry master at the time was a large, enthusiastic individual. He picked up the pupil, threw him in the large sink at the end of the bench and turned on the water tap full blast. I seem to remember him also grabbing a Winchester of ammonia too and adding that to the sink to neutralise the acid but that may just be my fanciful imagination. Happy days.
You would be better just buying a nice "science-looking" bong… Chances are that you'll get a used Kipp's apparatus which was used for toxic gases (its main use…). A brand new Kipp's apparatus can cost many thousands dollars! You really don't want some arsine, sulfane or cyanides in your weed…
Bonus: Now you can precipitate hydrochloric acid, and pickle your metal pipes so they're nice and shiny! :D Just make sure to remove the chemicals when you're done. Inhaling hydrochloric acid probably wouldn't be fun.
Chris SSDD actually curious about that... lol... would the acid and calcium chips cost more than say lighting some candles/gas stoves? or do growers have a better way to make CO2?
A perfect example of the fact that science is no less exciting when things don't work the way you expected them to compared to when everything works as expected.
The college I study at has a network of gas lines of many types, there are lines of purified Oxigen, Helium, Argon, 'synthetic air' (guess it's air with standart concentration of it's components) etc. There are old labs, however, that date back to the 1930's, and are not provided with these gas lines. on the second or third class when I entered college, we got to use this device. I found the way it works to be very clever. Can't remember if on the same lab, or a nearby one, there's an extended periodic table as well.
@@blackhatguy6955 Whether you call a fermented alcoholic drink beer or wine depends entirely on where the sugars come from. If they come from fruit (not just grapes, but any other fruit), then it is typically called wine. Beer is made from malted grain - most often barley, but also wheat or even rice. The grain is soaked in water and allowed to germinate - the enzymes in the sprout convert most of the starches into sugars. This is then dried to stop it growing any further, ground up and soaked in water to extract the sugars, producing a "malt extract" full of glucose, maltose, all sorts of vitamins, minerals and some residual protein. This is what makes beer relatively nutritious, and the soluble protein stabilises foam, giving your beer a "head".
It is actually very interesting to see how various chemistry apparatus works and what they are used for. I really hope to see more videos like this in the future. Thanks for the video.
I'd always thought about what I'd do if I were placed in a situation where I couldn't obtain any pressurized tanks, like what apparatus I would use. This is brilliant!!
What old chemistry? We used this Kipp apparatus in high school and then on first year in university chemistry classes. It wasn't so long ago. 20 years is not long time ago :)
Aww thanks so much for uploading this. Last week I found a Kipp's Apparatus in my 'new' lab and I wanted to try it, but I couldn't wrap my head around how it worked. Now I get it :)
Chemical equilibrium. The reaction of sulfate salts with CO2 lead to the precipitation of metal carbonates and the formation of sulfuric acid derivatives, such as bisulfate. The problem with this is two-fold. Firstly, sulfuric acid is a stronger acid than carbonic acid (the source of carbonate ions in aqueous equilibria). So if you take CO2 and water, which generates carbonic acid in solution, the carbonic acid cannot generate sulfuric acid because sulfuric acid would be much stronger. The second problem is transition metal sulfate solutions are slightly acidic in their own right, and that works against the formation of carbonic acid in the first place.
Often used a Kipp's generator as a source of hydrogen sulphide back in the early 1950's when doing "wet" chemistry for routine qualitative analysis in a chemical laboratory in a manufacturing company - it was standard equipment in those days.
Seriously if you guys and Breaking Bad was around when I was in school, I would have been so much more into Chemistry. (Not that I want to make drugs) I've just learned how interesting it all is
Believe it or not I tried the reaction of carbon dioxide gas (bubbled through) with copper sulfate solution when I was a child of 13 years old (I'm now a retired chemistry teacher). I got the same result as you did. I tried to figure what the predicted products might be. Of course, the answer I got was dilute sulfuric acid and solid copper carbonate. I already knew that these substances react to form carbon dioxide and copper sulfate solution. I guessed that this is why you don't get copper carbonate precipitated. The same sort of thing would happen with copper nitrate or copper chloride solution. In each case the strong acid that might be produced (during the equilibrium reactions) would instantly react with the copper carbonate so no precipitate would survive, even if it did form. My guess is that it is all to do with the relative strengths of the acids involved. Carbonic acid is simple too weak an acid to have any visible effect in the equilibrium reaction. In other words, the equilibrium is always well over to the left, so no precipitate is ever seen. Presumably, this is predictable by examining the solubility characteristics of copper carbonate under varying hydrogen ion concentrations. Once the pH drops below 7, any possibility of copper carbonate formation would become zero.
***** Yeah, just please try using less monotonic music in the background. I barely stand the same tone for more than 10 secs. ;) Keep up the good work!
Oh wow we did this in school. Admittedly less elaborately, but we did end up bubbling carbon dioxide through limewater from the base ingredients of calcium carbonate and hydrochloric acid. I didn't really understand it though so this video helped.
Es posible que no hayan resultado debido al pH. Para generar los carbonatos deben asegurarse de que el pH sea básico. El CO2 es ácido por lo que acidificaba las soluciones y no se observaba precipitación. Excelente video! El aparato de Kipp es genial.
If you put a pressure relief valve on it instead of a tap you could use it in a green house to stimulate plant growth. Of course you need to get the valve to trigger at the right pressure to keep the acid levels in the middle chamber just right.
My explanation for why the first three precipitate tests did not work is because carbon dioxide predominately exists as carbonic acid in neutral solution. If you want to form the carbonate anion to form the precipitate, you need to have a basic medium (that's why the calcium hydroxide test worked so nicely). When you write out the chemical equation for carbonic acid reacting with copper sulfate, you'll find out that it would quickly make the solution acidic IF the precipitate is formed. This cannot be the case since the acid would then react with the carbonate formed, reforming the copper salt and carbon dioxide. The problem is that most colored metal carbonates also have highly insoluble hydroxides, so it will be hard to find a colorful precipitate proof that the gas is carbon dioxide. My suggestion is to bubble the carbon dioxide into a weakly basic solution with phenolphthalein. This will slowly result in the disappearance of the pink color due to the carbonic acid reacting with the base.
The copper salt solution did not precipitate due to the acid conditions with CO2. Copper carbonate does only precipitate in alcaline or at least neutral conditions (as basic copper carbonate). Thanks a lot to the Periodic Video Team for all your videos! Johanna
Still used at Universidad de Concepción for biochem and chemistry students. Funny enough, the career takes 6 years because we take 13 courses of chemistry and a lot of biochem and clynical chemistry with the necessary enzyme knowlesge of course.
10 лет назад
When the title said "How to make Carbon Dioxide" "The Old-Fashioned Way"... I thought like... "just breathe" wouldn't that work?
It's always fun to watch the team put together interesting experiments~ Kudos to all the Dr and Professors~ Would love to see more crazy and fun experiments :D
The test my dear professor was to douse a flame with the carbon dioxide gas. Allow you exhaust tube to be placed over a flame, and the heavy C02 will extinguish the flame.
No precipitate formed because Co2 has to purge out all the air in the tubing before a reaction will happen. Also you made the solution's way to dilute.
