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Videos uploaded by user “TheChemistryShack”
How to Purify Boric Acid (by Recrystallization)
 
04:24
In this video, I outline the process of recrystallization, using boric acid as an example. *This video is meant to be a guide to performing recrystallizations. I will have a more detailed video in the future that discusses the science behind recrystallization. Besides demonstrating recrystallization, boric acid is useful for other things. I am particularly interested in its use as a flame colorant. When dissolved in methanol and burned, it produces a GREEN FLAME! Link to the GREEN FIRE video here: https://www.youtube.com/watch?v=jMECHSflU5I Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 5851 TheChemistryShack
How to Dissolve US Nickels (H2SO4 method)
 
06:46
In this video, we will dissolve US nickels using sulfuric acid and hydrogen peroxide. US nickels consist of 75% copper and 25% nickel by mass. Because both of these metals are too unreactive to dissolve in H2SO4 alone, we need to add H2O2 to oxidize the metals and allow them to dissolve in the acid. This is quite a beautiful reaction, with a lovely blue-green solution being produced, but it can also provide you with a useful source of nickel metal. I am currently working on isolating the nickel metal from the solution, so keep an eye out for that video. DISCLAIMER: While defacing coins without fraudulent intent is fine, fraudulently defacing US coins is illegal. I am not responsible if you do anything illegal! This is more fully explained at the Tresury.gov page: https://www.treasury.gov/resource-center/faqs/Coins/Pages/edu_faq_coins_portraits.aspx Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 18131 TheChemistryShack
How to Make Aluminum Oxide (Al2O3)-IMPROVED VERSION
 
05:03
*REUPLOADED DUE TO AUDIO ISSUE* In this video, we will make aluminum oxide, a useful catalyst that I will use in upcoming videos. ***ANNOUNCEMENT*** Thank you guys so much for helping me reach 1,000 subscribers. I am extremely grateful to have the support of each and every one of you. To celebrate, I am planning on making a special video for the occasion. However, I want your input in deciding what kind of video you want this to be. I've listed a few ideas below, but feel free to suggest your own ideas. 1) List Video: something like "5 reactions you can do with home chemicals" 2) Pyrotechnics/explosions: thermite, booms, bangs, whatever! 3) Specific reaction; let me know if you guys have any specific reactions you'd like to see me perform! *About the Na2CO3 error; You should use 3.5 g of Na2CO3 per 1.00 gram of Al2O3 you want to make. The reason I didn't re-record this is because I am on vacation and I didn't bring my microphone. Subscribe to TheChemistryShack: https://www.youtube.com/user/TheChemistryShack Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Twitter: @TheChemShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@gmail.com
Views: 13982 TheChemistryShack
How to Make Ethene (Ethylene) - Catalytic Dehydration of Ethanol
 
05:03
In this video, I make ethene gas (also known as ethylene) by catalytic dehydration of ethanol. With the formula C2H4, ethene is the simplest alkene, a class of hydrocarbons containing carbon-carbon double bonds. Alkenes are very reactive and can be converted to various different molecules. As a few examples, they can be hydrogenated to form alkanes, halogenated to form halogenoalkanes, reacted with water to form alcohols, and polymerized to form polyalkenes. Ethene can be produced by dehydrating ethanol (removing a water molecule). I use an Aluminum oxide catalyst, which I showed how to make in a previous video, to catalyze the dehydration of ethanol. I also show how you can test the ethene produced by using iodine water. (Bromine water is typically used instead, but I didn't have any so I had to improvise.) How to Make Aluminum oxide: https://www.youtube.com/watch?v=tC5D5wRSr60 Subscribe to TheChemistryShack: https://www.youtube.com/user/TheChemistryShack Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Twitter: @TheChemShack Follow me on Google+ +TheChemistryShack
Views: 22367 TheChemistryShack
How to Make Aluminum Oxide (Al2O3)
 
05:03
**THIS VIDEO HAS A WEIRD AUDIO ISSUE** LINK TO FIXED VIDEO BELOW: https://www.youtube.com/watch?v=tC5D5wRSr60 In this video, we will make aluminum oxide, a useful catalyst that I will use in upcoming videos. ***ANNOUNCEMENT*** Thank you guys so much for helping me reach 1,000 subscribers. I am extremely grateful to have the support of each and every one of you. To celebrate, I am planning on making a special video for the occasion. However, I want your input in deciding what kind of video you want this to be. I've listed a few ideas below, but feel free to suggest your own ideas. 1) List Video: something like "5 reactions you can do with home chemicals" 2) Pyrotechnics/explosions: thermite, booms, bangs, whatever! 3) Specific reaction; let me know if you guys have any specific reactions you'd like to see me perform! Subscribe to TheChemistryShack: https://www.youtube.com/user/TheChemistryShack Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Twitter: @TheChemShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@gmail.com
Views: 46958 TheChemistryShack
Testing Silicon with Sodium Hydroxide [Full HD]
 
02:50
In this video, I test the silicon produced in my video from December 2014, titled "Silicon Synthesis (From Mg and Sand) [Full HD]". (See that video here: I test the silicon by examining its reaction with sodium hydroxide. Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 3381 TheChemistryShack
How to Make Tert-Butyl Chloride
 
07:20
In this video, I show you how to make tert-butyl chloride from tert-butyl alcohol and hydrochloric acid. Tert-butyl alcohol is a type of molecule known as an alkyl halide. The term "alkyl" means that each carbon atom is bonded to 4 atoms (4 single bonds). The term "halide" means that there is a carbon-halogen bond, in this case a carbon-chlorine bond. Alkyl halides are pretty useful molecules because the halgoen atom can be exchanged for other atoms, molecules, or ions, producing a variety of different compounts. *The IUPAC name for tert-butyl chloride is 2-chloro-2-methylpropane This reaction is fairly straightforward: just mix hydrochloric acid with tert-butyl alcohol. Despite the seemingly simple reaction, the mechanism is really interesting. I explain the mechanism in the video (with diagrams!), but the fact that makes it interesting is that this mechanism only works for tertiary alcohols. It is possible to make primary and secondary alkyl chlorides, but the reaction doesn't happen at room temperature and is a lot more complex to carry out. Huge thanks to James from masterorganicchemistry.com for letting me use his reaction mechanism diagrams! The link to that page is provided below: http://www.masterorganicchemistry.com/2015/02/27/making-alkyl-halides-from-alcohols/ Explanation of my issues with the graph: The graph's density values were way off from the density values I calculated, even after accounting for the uncertainty in my measuring equipment and calibrating my pipet and digital balance. I am currently using the analytical balances and pipets at my school to replicated the paper's procedure and see if the authors of the paper messed up (or if I just screwed something up without realizing it). Learn more about Nucleophilic Substitution: http://www.masterorganicchemistry.com/2015/02/27/making-alkyl-halides-from-alcohols/ Learn more about SN1 reactions: http://www.organic-chemistry.org/namedreactions/nucleophilic-substitution-sn1-sn2.shtm Original procedure: http://www.orgsyn.org/Content/pdfs/procedures/CV1P0144.pdf Subscribe: https://www.youtube.com/user/TheChemistryShack Follow me on Twitter: @TheChemShack
Views: 9808 TheChemistryShack
How to Make A Bromophenol Blue Solution (pH Indicator)
 
04:18
In this video, I make a bromophenol blue indicator solution using two simple ingredients: bromophenol blue powder and methanol. WARNING: Methanol is highly toxic and flammable, so be careful when working with it. Alternatively, you could use 95% ethanol for this experiment. All you need to do to make a bromophenol blue solution is dissolve 0.1 g of bromophenol blue powder in 100 mL of methanol, and stir for a few minutes. Bromophenol blue is a type of pH indicator, which means it changes color when the pH of a solution changes. In methanol, BB is a reddish-green color. However, when you add a few drops to a solution, it will change to either blue or yellow, depending on the pH: pH less than 3 = yellow pH greater than 4.6 = blue Because of its pH range, BB is great for distinguishing between dilute and concentrated acids. Conc acids with pH below 3 will be yellow, but dilute acids with pH above 4.6 will be blue. This is discussed at 2:14 in the video. However, it is not a great indicator if you have to distinguish between acidic and basic solutions, because ALL pH values above 4.6 will be blue. I demonstrate this at by adding a few drops of BB to a dilute acid (pH 5), water (pH 7), a dilute base (pH 11), and a concentrated base (pH 14), and they all turn the same shade of blue*. *The concentrated base is a significantly darker blue than the other three, and this has to do with BB's acid/base equilibrium. I don't have room to explain this fully in the description, but if you are curious send me a private message through youtube, or email me (you will se my email listed below). ***STAY TUNED FOR LIQUID CHLORINE VIDEO, COMING SOON*** LIQUID CHLORINE Reacting with Metals Trailer! The full liquid chlorine video will be out on Friday, February 5. Hope you enjoy! Subscribe to TheChemistryShack: https://www.youtube.com/user/TheChemistryShack Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@gmail.com Hustle by Kevin MacLeod is licensed under a Creative Commons Attribution license (https://creativecommons.org/licenses/by/4.0/) Source: http://incompetech.com/music/royalty-free/index.html?isrc=USUAN1100793 Artist: http://incompetech.com/
Views: 9752 TheChemistryShack
Making LIQUID CHLORINE and Reacting it With Metals
 
04:50
In this video, I will make liquid chlorine and react it with steel wool, magnesium, and lithium. Chlorine boils at -34 Celsius, so condensing chlorine gas requires a special setup. I first set up a chlorine gas generator, and then used a bath of dry ice in acetone to condense the chlorine into a liquid. Once I had the liquid chlorine, I reacted it with steel wool, magnesium, and lithium. Watch the video to find out what happens! Subscribe to TheChemistryShack: https://www.youtube.com/user/TheChemi... Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemi... Follow me on Twitter: @TheChemShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@gmail.com
Views: 9422 TheChemistryShack
How to Make Chloroform
 
06:44
In this video, I react bleach and acetone via the haloform reaction to synthesize chloroform. Chloroform is a very useful solvent and reagent, and I'll be using it in upcoming videos. This reaction is aptly named the "Haloform Reaction" because it produces a Haloform (a methane molecule where 3 of the hydrogen atoms have been replaced by a halogen). This reaction doesn't give great yields, but the reactants are so cheap that it is definitely an economically viable way to produce chloroform. Disposing of chloroform: Chloroform hydrolyzes in basic conditions, so just let the chloroform sit in the bleach bottles for a couple of weeks, allowing the basic conditions to break down the chloroform. After a couple of weeks, there will be only a tiny amount of chloroform left, and you can flush this down the drain with excess water. Link to UC235 video (he explains the mechanism of the reaction): https://www.youtube.com/watch?v=XYbnNufX5-c Subscribe to TheChemistryShack: https://www.youtube.com/user/TheChemistryShack Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Twitter: @TheChemShack Follow me on Google+ +TheChemistryShack
Views: 391596 TheChemistryShack
How to Purify 70% Ethyl Rubbing Alcohol
 
05:45
See my write-up of this experiment on sciencemadness: http://www.sciencemadness.org/talk/viewthread.php?tid=63320#pid416043 In this video, I'll show you how to purify 70% ethyl rubbing alcohol from the pharmacy into nearly anhydrous reagent grade ethanol. The purification process involves 3 main steps (and an optional one): 1) Simple distillation This concentrates the ethanol to about 85% and leaves behind higher-boiling impurities like MIBK and Denatonium benozate 2) Drying The ethanol is dried using MgSO4 and filtered. Other appropriate drying agents like K2CO3 and molecular sieves could be used. 2a) Fractional distillation *OPTIONAL* This is to remove the acetone. Discard the acetone distillate that comes over at 56 C and stop the distillation once the temp rises above 56 C. 3)Final simple distillation Finally, we distill off the ethanol from any MgSO4 that may have dissolved in it. This distillation is nto necessary if you used molecular sieves. ***WARNING***** This ethanol is intended to be used as a lab solvent or reagent ONLY. IT IS NOT intended for topical or ingestion purposes. Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 13173 TheChemistryShack
Reaction of SiCl4 and Water (Hydrolysis)
 
02:11
In this video, I use some of the SiCl4 that I made in my last video (link below) to illustrate its reaction with water. SiCl4 video: https://www.youtube.com/watch?v=ojUebnfzzz0 This reaction is an example of a hydrolysis reaction. "Hydrolysis" is really just a fancy way of saying "water tearing stuff apart". Indeed, a hydrolysis reaction is one in which water molecules break apart other molecules. In this case, water is breaking apart the Si-Cl bonds in SiCl4. The reaction is as follows: SiCl4 + 4H2O ---- 4HCl + H4SiO4 (sorry, youtube wouldn't let me add arrows for some reason :( The reaction is quite exothermic and even boils the water!! As a side note, Nile Red also has an excellent video on this reaction: https://www.youtube.com/watch?v=wU77anzCzxg He discusses the reaction of SiCl4 with water at 7:14 After performing the reaction, I do a pH test to show that HCl has indeed been made. Check out Shiva Chemist: https://www.youtube.com/user/Shivachemist Subscribe to TheChemistryShack: https://www.youtube.com/user/TheChemistryShack Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@gmail.com Hyperfun by Kevin MacLeod is licensed under a Creative Commons Attribution license (https://creativecommons.org/licenses/by/4.0/) Source: http://incompetech.com/music/royalty-free/index.html?isrc=USUAN1400038 Artist: http://incompetech.com/
Views: 5418 TheChemistryShack
Beautiful Purple Copper Complex
 
05:03
In this video, I make a copper complex with a gorgeous purple color. The process is simple and only involves two chemicals: copper sulfate and sodium dichloroisocyanurate. Watch the video to see how the complex is made, and watch me fail at art :P
Views: 5324 TheChemistryShack
Magnesium/Sulfur Flash Powder
 
03:28
In this video I show you how to make a flash powder using magnesium and sulfur powders. These powders react very quickly and explosively, generating a flash (hence the name "flash powder"). WARNING: This reaction involves a highly explosive mixture (duh!). Do not make large quantities ( over 5 grams) of this mixture. Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 6236 TheChemistryShack
How To Make Silicon Tetrachloride (SiCl4)
 
09:47
WARNING!!!! DO NOT REPEAT THIS EXPERIMENT UNDER ANY CIRCUMSTANCES! CHLORINE AND SILICON TETRACHLORIDE ARE EXTREMELY TOXIC! In this video, we synthesize silicon tetrachloride from silicon powder and chlorine gas. I've been promising to make this video for quite a while, and it's finally here. The setup and procedure is from WACKER"S experimental kit; link here: http://www.chemiedidaktik.uni-wuppertal.de/disido_cy/en/exp/m_fact01.htm (My setup varied slightly from this setup; the main difference is that I didn't use primary absorption bottles-everything else is pretty much the same). Silicon tetrachloride (SiCl4) is a pretty interesting molecule, as it exhibits the nonmetal characteristics of silicon. As you may recall from chemistry class, silicon is a metalloid, which means it can act as a metal AND a nonmetal. In compounds like SiO2, silicon acts as a metal and forms ionic bonds*, whereas in compounds like SiCl4 silicon forms covalent bonds. It is also one of the few compounds of silicon that is LIQUID at room temperature!!! *The bonds aren't actually ionic; this is an oversimplification. See the annotation at 0:45 for clarification. Synthesizing silicon tetrachloride is actually fairly simple. All that needs to be done is to heat silicon while passing a stream of chlorine over it, and condense the SiCl4 vapors. However, because of the toxicity and reactivity of both chlorine and SiCl4, the apparatus is fairly complex and takes a while to set up. In this video, I demonstrate the production of silicon tetrachloride and talk about the molecule itself and the chemistry behind its synthesis. I must once again stress that this is for educational purposes only and should not be repeated! In my next video, we will be looking at the reaction of SiCl4 with water, so stay tuned for that. Subscribe to TheChemistryShack: https://www.youtube.com/user/TheChemistryShack Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@gmail.com
Views: 4649 TheChemistryShack
DIY Bunsen Burner Fuel Source (Propane)
 
03:05
In this video, I show you how to make a cheap propane fuel source for a bunsen burner. The only cost, other than the propane itself (which is about $5 for a decent-sized tank) is a brass torch fitting and vinyl tubing, both of which add up to about $15.
Views: 12346 TheChemistryShack
Make GREEN FIRE (Using Boric Acid)
 
04:22
In this video, I show you how to make GREEN FIRE! All you need is methanol, some recrystallized boric acid, and an ignition source, and you can make a vibrant green flame! Of course, this experiment is dangerous for obvious reasons. Methanol is highly flammable AND very poisonous. While I do recommend that you try this experiment yourself, make sure you know what you are doing. I will not be held responsible for any injuries you cause to yourself or others. Link to video of exploding methanol bottle: https://www.youtube.com/watch?v=IYbqBAeMNhY The music is Mozart's Oboe Concerto in C major, K.314. Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 4939 TheChemistryShack
Aluminum Powder + HCl: Effect of Surface Area on Reaction Rate
 
02:24
In this video, I demonstrate the effect of surface area on reaction rate by reacting aluminum powder with HCl. Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 1656 TheChemistryShack
DIY Vacuum FIltration (for under $10!)
 
04:42
In this video I show you how to perform a vacuum filtration with parts costing less than $10.
Views: 13214 TheChemistryShack
Awesome Hydrogen and Oxygen Experiments!
 
03:25
In this video I isolate elemental hydrogen and oxygen and do a few interesting experiments with them WARNING! This reaction uses CORROSIVE acids, FLAME, HIGH TEMPERATURES, EXPLOSIVE gases, and ecologically harmful MnO2. Do not repeat under any circumstances. I am not responsible for any harm that may come to you should you choose to duplicate this procedure! Note on MnO2 (manganese dioxide): This compound is toxic to aquatic life and SHOULD NOT BE FLUSHED DOWN THE DRAIN UNDER ANY CIRCUMSTANCES WHATSOEVER!!! Instead, dilute the MnO2 waste from the flask and store it in an appropriate container. You can reuse this in the future to generate more oxygen from H2O2.
Views: 10406 TheChemistryShack
Cleaning Potassium Permanganate stains (the cheap and easy way)
 
01:17
A cheaper and safer way to remove potassium permanganate stains.
Views: 12104 TheChemistryShack
Amazing Chemistry Magic Trick!
 
01:34
A magic trick, chemistry style! An explanation is below, so if you want to try and guess how everything worked, you can see if you are correct or not. ..... ..... ..... The water is actual pure distilled water--no tricks there 1) Turning into "grape juice"--The first beaker had a very small amount of potassium permanganate on the bottom (KMnO4). Even a small amount of this powder creates a very intense purple-pink solution. 2)Turning into "Muddy water"-- I then poured the KMnO4 solution into a dilute solution of sodium metabisulfite. The metabisulfite reduces, or gives electrons, to the permanganate, reducing it to brown manganese dioxide (MnO2). 3) "Purifying" the "muddy water" -- I simply let the MnO2 react with the metabisulfite further to fully reduce it to colorless Mn2+ ions. The permanganate wasn't instantly converted to Mn2+ because the metabisulfite solution was dilute, and this low concentration slowed down the reaction. This beaker also had a few drops of phenolphthalein in it, which is important for the next step. 4) Turning it into "Pink Lemonade"--The 4th beaker contained a few drops of NaOH solution. When the phenolphthalein from beaker #3 is in a basic solution (like NaOH), it turns pink. 5) Turning it into "vodka"--The 5th beaker had just enough vinegar to neutralize the NaOH and make the solution slightly acidic. Phenolphthalein turns clear in acidic conditions. 6)Turning it into "lemonade"--The 6th beaker contained a small amount of potassium dichromate (K2Cr2O7) powder. This dissolves to give a yellow solution. 7) Turning it into "limeade"--The last beaker had a metabisulfite solution in it. This reduced the yellow dichromate to a lower oxidation state, which has a green color in solution. Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 16070 TheChemistryShack
Silicon Synthesis (From Mg and Sand) [Full HD]
 
09:44
Merry Christmas, Everyone! As a present from me to you, I have a Christmas-themed video for you guys! Because what says "Merry Christmas" better than a powdered, black, semiconducting metalloid?? In this video, I synthesize silicon (Si). Silicon is a metalloid used in semiconductors and computer chips. It also makes up 28% of the earth's mass, and is found in sand and quartz. It has a wide range of interesting physical and chemical properties, and in a later video I will be reacting it with chlorine to make silicon tetrachloride (SiCl4). SiCl4 is an interesting chemical and I will tell you more about its properties in the upcoming video. Anyway, back to the silicon synthesis. The standard method of synthesizing silicon is a thermite reaction, either with sand (silicon dioxide; SiO2) and aluminum or sand and magnesium. However, I could not perform a thermite reaction for several reasons, mainly the lack of a container to contain the molten silicon resulting from the thermite. So I decided to use a modified version of Nile Red's Magnesium Silicide Synthesis (link below) to make silicon. Link to the video: https://www.youtube.com/watch?v=KXCBnznxxIk In his synthesis, he heats silicon dioxide and magnesium together, with the magnesium being in excess. Two reactions occur, shown below: Reaction 1: 2Mg + SiO2 = 2MgO + Si Reaction 2: Si + 2Mg = Mg2Si In the first reaction, the magnesium combusts by stripping the oxygen from the SiO2 and forms silicon. The Silicon produced then reacts with the remaining hot magnesium to produce magnesium silicide. It is for this reason that the magnesium is in excess. Now I figured that by instead making silicon dioxide the excess reagent, we could prevent the second reaction from occurring (or at least make it occur to a lesser extent) and end up with some elemental silicon. So that's what I did! I reacted magnesium powder with a 20% excess of silicon dioxide (impure; I should have washed it with water and HCl). The product of the reaction, once washed, was a dark black powder, which is a good sign that the reaction actually worked and that we made actual silicon. Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com Merry Christmas and a Happy New Year!
Views: 27072 TheChemistryShack
Tour of "The Chemistry Shack 2.0"
 
03:21
A tour of THE CHEMISTRY SHACK 2.0! The shack has changed a lot since last year, so I wanted to catch you guys up on all of the renovations. Hope you enjoy! Future videos (probably in order?): Purifying 70% ethyl alcohol Synthesis of SiCl4 Dissolving US Nickels (2 methods) Extracting Nickel metal from US nickels (I'm still working on this and haven't had success yet, but I'll keep trying :P) Extracting CaCO3 from antacid tablets Generating anhydrous ammonia gas Generating anhydrous HCl gas Cheap sources of liquid nitrogen Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 1794 TheChemistryShack
Choosing the Right Gloves
 
05:06
Specific gloves need to be chosen for specific categories of chemicals. This video lists the different types of gloves and what they can protect against, according to the Flinn Scientific Glove Selection Guide
Views: 5826 TheChemistryShack
How to Purify Hydrochloric acid (sort of)
 
04:08
Link to TheHomeScientist's video: https://www.youtube.com/watch?v=jv1Ms6Subg4 Link to videos explaining suck back (back flow): https://www.youtube.com/watch?v=kqQSpRus-t0 https://www.youtube.com/watch?v=YGjd7xxTuZw
Views: 6112 TheChemistryShack
LIQUID CHLORINE Reacting with Metals (Trailer)
 
00:45
LIQUID CHLORINE Reacting with Metals Trailer! The full liquid chlorine video will be out on Friday, February 5. Hope you enjoy! Subscribe to TheChemistryShack: https://www.youtube.com/user/TheChemi... Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemi... Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@gmail.com
Views: 890 TheChemistryShack
Titration of Cheap Potassium Hydroxide
 
04:18
In this video I determine the purity of super-cheap tech. grade potassium hydroxide ($6.95/2 pounds) form Dudadiesel.com via acid-base titration using phenolphthalein as an indicator. Link to the website: http://www.dudadiesel.com Difference between tech. grade and food grade: Technical grade chemicals usually contain many impurities and the exact amount of impurities has not been calculated by the seller. Food grade is essentially the same, but food grade chemicals are tested to make sure they have low levels of toxic substances such as lead and arsenic. My calculations from the 1st and 2nd titrations that I performed but didn't film (the ones where I got a light pink): 1st titration: A) Pre-titration calculations 5.44 g KOH in 100 mL water Assuming 90% purity gives us: 5.44 g impure KOH *9g actual KOH/10 g impure KOH = 4.896 g KOH/100 mL Conversion to M: 4.896 g KOH/100 mL * 1000 mL/L * 1 mol/56.11 g = 0.873 mol/L 1 mL vinegar placed in a flask (measured with Mohr pipet) 1 mL * 0.874 mol/1000 mL = 0.000874 mol H+ Determining amount of KOH that should be needed 0.000874 mol of KOH needed to neut. 0.000874 mol of vinegar 0.873 mol/1000 mL = 0.000874 mol/x mL x = 0.99 mL of KOH solution should be needed B) Titration results 1.0 mL of KOH used 2nd titration: A) Titration facts: 1 mL vinegar 0.9 mL of same KOH solution from previous titration used Calculating the Purity Average vol of KOH solution used: 0.9 mL + 1 mL/2 = 0.95 mL moles acid: 0.000874 That means that there are 0.000874 moles of OH- in 0.95 mL of solution Conversion to M: 0.000874 mol/0.95 mL = x mol/1000 mL x = 0.919 mol KOH/L Calculating total moles of KOH: 0.919 mol/1000 mL = x mol/100 mL = 0.0919 mol/100 mL Calculating total grams of KOH: 0.0919 mol * 56.11g/mol = 5.156 g KOH 5.44 grams of impure KOH were weighed out to start, so that means there are 5.156 g of actual KOH in 5.44 g of impure KOH Final conversion: calculation mass/mass % purity: 5.156 g actual KOH/5.44 g impure KOH = x g actual KOH/100 g impure KOH x = 94.78% pure
Views: 8352 TheChemistryShack
Announcement: Silicon Tetrachloride Video Coming Soon
 
01:19
SiCl4 video is up! Link here: https://www.youtube.com/watch?v=ojUebnfzzz0&feature=gp-n-y&google_comment_id=z13tgxjjswmpvvj2z23zwrfazky1exxjn04 Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 353 TheChemistryShack
How to Make Lithium Sulfide (Li2S) and Hydrogen Sulfide (H2S)
 
04:02
In this video, I show you how to make lithium sulfide from easily accessible chemicals. You can use this salt to generate hydrogen sulfide, a useful yet smelly gas. Even if you don't use the final product, the reaction is still fun to watch! Get sulfur-- www.dudadiesel.com Get lithium- https://www.youtube.com/watch?v=BliWUHSOalU
Views: 2524 TheChemistryShack
How to Make Up Molar Solutions (Without Volumetric Flask)
 
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********Titration with 5% vineagr showed this to be a 1.03 M solution, when it should have been 1.01 M. Using a volumetric flask would give you much more accurate results, but this small error of 0.02 M is acceptable for my needs.*************** In this video, I show you how to make up a molar solution without spending any money on expensive volumetric flasks. Note: This procedure won't yield EXTREMELY accurate results. Volumetric flasks are calibrated to a very precise volume (Ex: 250.000 mL) and are only off by 0.5 mL at the most, whereas graduated cylinders can be off by as much as 2-5 mL. However, for my purposes this small error is permissible. Also, since this is a basic solution, I can titrate it with 5% vinegar and verify its conc. If you need a solution of a very precise conc., go ahead and use a volumetric flask. Explanation of the Stoichiometry: 1) We want to end up with a solution described as (moles of solute per liter of solution). Steps: 1) Determine the desired molarity of your solution: I want a 1 M solution, or 1 mol KOH/L 2) Convert to grams/L: This is just a simple moles-grams conversion. The formula weight of KOH is 56.11 g/mol. Thus the conversion is: 1 mol KOH/L *56.11 g/mol = 56.11g/L (1 M conversions are pretty easy :) 3) Use proportions to adjust for a change in volume. You might not want to make a 1 liter solution of every chemical you have. That's okay, you can scale the volume up or down while maintaining the same molarity. 56.11g/1000 mL = x g/200 mL desired Cross multiply: 1000x = 11222 g x= 11.222 g of KOH
Views: 3458 TheChemistryShack
Potassium Permanganate (KMnO4) vs. Food Coloring
 
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How well does KMnO4 maintain its color when diluted? And how does it compare to food coloring? Explanation of the dilution equation: M1V1 = M2V2 M1 = initial concentration V1 = initial volume M2 = final conc. V2 = final volume example: M1 = 1000 ppm V1 = 1 g (since I used mass instead of volume) M2 = 100 ppm (this is the conc. I want to end up with) V2 = ? (how much will the final solution weigh? 1000 ppm * 1 g = (M2) * 100 ppm Divide each side by 100 ppm and we get: 10 g = M2
Views: 3864 TheChemistryShack
Sour Patch Kids vs. Sulfuric Acid
 
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Leftover candy + Strong acid = Well... you tell me!
Views: 1111 TheChemistryShack
Tour of the Chemistry Shack
 
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This is just a quick tour of my makeshift lab (or at least what it was like when I started chemistry). I go through and show you all of my boxes and shelves full of chemicals and equipment. Currently, everything is much more organized, as I store my equipment is closed plastic boxes and my chemicals in designated cabinets, where they are isolated by type. My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email wwswillsmith77@aol.com Here is a brief outline of all the components of my lab (as organized way back when): Box #1: Burners, torches, and hot plates. My various butane and propane torches, all of which serve different purposes (ignition, sustained heating, torching the crap out of things), as well as my alcohol burners, butane gas burner (My hottest burner, reaching up to 2500 Celsius), and Bunsen Burner (although it is technically a Tirril burner). I also have 1 hot plate/magnetic stirrer combination, but it is currently not working :( Box #2 Excess glassware. I keep a large variety of glassware around because you never know what kind of apparatus you will need. This particular box contained some beakers, Erlenmeyer flasks, and specialized storage containers (like my 1 all-glass bottle for storing strong acids). The long, plastic-wrapped thingy on the right side of the box is my uncut 24 in. glass tubing). Box #3 More glassware!!!! Test tubes and stoppers, bottles, jars, and other items like vials and spoons (which are a great alternative to more expensive scoopulas!). Box #4 Weigh boats (essentially just fancy plastic bowls), tubing, adhesives (tapes, glues, epxoys, etc..), and distilled water. I use distilled water instead of tap water because tap water often contains contaminating ions that are fine to drink, but would tamper with experiments, especially quantitative analyses. Box #5 Spoons, scoops, stirring rods, spatulas, thermometers, glass tubes, syringes, and pipets. If you are wondering why I have both syringes AND pipets, I used syringes before I could afford pipets. I don't really prefer one over the other, although graduated pipets tend to be much more accurate and precise than syringes. Box #6 Larger hardware, like scissors, X-acto knives, test tube and beaker tongs, pliers, etc... AND THE HAMMER!!!!!! Box #7 Stuff that I couldn't find a place for, including my sheet of copper that is too big to store with my other metals and a bunch of electrical equipment. Box #8 Safety equipment!! Gloves, goggles, face shield, respirator, and plastic bags for spill control. Box #9 "Glassware." Essentially just wine bottles that I never used because well---DUH! Box #10 (Against back wall) Crucibles, watch glasses, plastic pipets, my 2 digital balances, Kjeldahl distillation bulb (I think that's how you spell it), and some other miscellaneous stuff. Box #11 Ring stand accessories. Various clamps and such. If you want to learn more about different types of clamps and/or other ring stand accessories, tell me in the comments. Box #12 Filtration equipment. Basically just a bunch of different types of funnels and filter paper. Chemicals: See my video entitled "Lab Update (and how to store chemicals" for more info on how I organize my chemicals.
Views: 1444 TheChemistryShack
Aluminum Sculpture VS. Hydrochloric Acid (HCl) [Full HD]
 
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In this video, I destroy a Halloween-themed aluminum sculpture using concentrated 10 Molar Hydrochloric acid (HCl). This video was supposed to be the 2015 Halloween special, but I decided to go ahead and upload it; I'll surely think of something better when it comes time for Halloween though. Here are the links for the channels I mentioned in the video: HunChem: https://www.youtube.com/user/TheHunChem TheBackyardScientist: https://www.youtube.com/user/TheBackyardScientist ExplosionsAndFire: https://www.youtube.com/user/ExplosionsAndFire Did you like the salsa music in the background? Here is the name of the song (All rights to the Music go to Simona Cavuoto): "Pobre Diabla" by Simona Cavuoto Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 561 TheChemistryShack
How to: Dehydrate Salts
 
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In this video, I show you how to dehydrate salt hydrates while simultaneously determining their formula. I wasn't able to explain the related calculations because "brackets aren't allowed in video descriptions", even though I didn't use any brackets. Link to NurdRage's video: https://www.youtube.com/watch?v=XJFfS_YbbYI
Views: 687 TheChemistryShack
Lab Update (and how to organize chemicals)
 
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Just a brief lab update in which I explain my new system for organizing chemicals safely.
Views: 2227 TheChemistryShack
Chemistry Magic Trick/Brianteaser
 
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A little more involved than my previous magic trick, as you guys get to try and figure out how I did it!
Views: 444 TheChemistryShack
How to Remove Rust from Ring Stand Clamps
 
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In this video I test and easy method of removing rust from ring stand clamps--all you need is some salt and vinegar!
Views: 894 TheChemistryShack
70 Subscriber Special: Part I [HD]
 
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Thank you guys so much for subscribing! It really means a lot!!
Views: 357 TheChemistryShack
Why You Should Take the Flinn Scientific Safety Course
 
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The Flinn Scientific Safety course contains a wealth of extremely useful safety information. "Death by Test Tube Brush" Explanation: Here is the scenario: You clean a test tube with a brush that doesn't have bristles on the very end. Therefore, the metal scrapes the bottom of the test tube. This weakens the structural integrity of the glass and makes it more likely to crack. The next day, you add aluminum to the tube and drip on several mL of sulfuric acid. To speed up the reaction, you heat the test tube over a Bunsen. The test tube cracks, spraying boiling-hot sulfuric acid all over you.
Views: 756 TheChemistryShack
Inexpensive Safety Equipmment
 
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In this video I cover some cheap yet very effective ways of protecting yourself in the lab.
Views: 867 TheChemistryShack
Ice Bucket Challenge-Lab Safety Style!
 
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You finally get to see me dump a bucket of ice water on my head--while learning about lab safety and spill control. It's the best of both worlds! NOTE: NO CHEMISTRY NERDS WERE HARMED IN THE MAKING OF THIS VIDEO, AND MORE IMPORTANTLY, NO REAL SULFURIC ACID WAS WASTED.
Views: 497 TheChemistryShack
A Tour of Matter
 
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A tour of the 4 different types of matter that can be found on earth. NOTE: Throughout the video, i pronounce the word "heterogeneous" in different ways. The correct pronunciation, according to dictionary.com, is "het-er-uh-JEE-nee-us)
Views: 257 TheChemistryShack
Happy Mole Day! Here are some treats to Celebrate! [HD]
 
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Happy Mole Day! In this video, I show you some tasty mole-themed treats that you can easily make at home, and all of them are listed below. If you are unfamiliar with, or would like to learn more about the mole, check out the video by Science Hideout that I have linked below: Video by Science Hideout: https://www.youtube.com/watch?v=TAsgg9Rd_ws&list=UUqdaflk0TuFIIlWA-2xG22A I tried to incorporate the word mole and the number 6.0221 everywhere I could in the recipes. #1 Chocolate MOLEshake Mix together 6.0221 scoops of chocolate ice cream, 6.0221 half-cups of milk, and 1 mole of table sugar (342.34 grams). Blend well. DO NOT DRINK THIS!!! IT TASTES TERRIBLE!!! Barely any of the sugar dissolved, and made the drink grainy. It was basically like drinking a way-too-sweet drink with sand in it. #2 Pound cake a la MOLE 6.0221 pieces of pound cake, 6.0221 scoops vanilla ice cream, and 6.0221 drops of chocolate sauce. #3 Coca MOLa, MOLo Yellow, MOLEntain Dew Measure out 60.221 mL of the soft drink of your choice, and add to it precisely 6.0221 grains of sugar. Contact me: My Channel Home Page: https://www.youtube.com/user/TheChemistryShack Follow me on Google+ +TheChemistryShack My email: wwswillsmith77@aol.com
Views: 773 TheChemistryShack