For all the people that are looking for the natural qualities and advantages of mint for your health simply get a bunch of leaves you can even throw the stem in there boil it down extract the water dilute it with more water maybe add some honey when it cools down drinks up All you need is a pot a bunch of mints and a source of heat mission complete
Hey! I just found you're channel, way to go! I really am enjoying everything im seeing, so very well done . Im putting you up there with chemical force its actually refreshing to see the career and hobbie ive been addicted to as a very young child playing mad scientist by dumping a bit of everything that was in my aunt's bathroom closet onto the toilet bowl! Cleaners, antacids, aspirin, toothpaste, (for texture! ) and it pains me to say 😢 her medicine cabinet ! Where her prescriptions were, holy shit i didn't dump all of her meds down into the cauldron of herr professor dopeinstupid . And yes a really bad reaction had taken place when I added a final ingredient! Yes a little dab of draino crystals had started to fizz really loud like, and then came the fumes! Oh well kids got to love em!😅
It depends on the quality of the pump and the sealing of the connections. Good setups lower the boiling point to around 90°C others, more like to 130°C.
Hello I have a question. I have to do a qualitative analysis of salt as part of my university practical. The sample contains a mixture of different cations and anions which have to be detected. In the end of the video, you mentioned that large amounts of arsenic can give a false result. My sample contains arsenic , so I would like to know how to get a correct test for tin in the presence of arsenic. Your answer will be really helpful for me.
I request you to show as the COD measurement process according to APHA5220D. with reagent A and B making as well as the use of the spectrophotometer. is it possible?
Hey, could you help me with this reaction ASAP? I used this recipe: but no bromine was being formed do you know where I could be going wrong? Furthermore, the ferroin solution wasn't changing colour and no oscillations was being created and the H2SO4 was reacting quite a lot unlike yours. Solution a: 11g of KBrO3 100ml of distilled water Solution b) 2g of CH₂(COOH)₂ 75ml H2SO4(10%) 1g of NaBr Fill it to 100ml In 100 ml volumetric flask Solution 3) Ferroin (0.025 mol/L concentration) Mix Solution 1 and 2 in a 1:1 ratio. Add 25 ml of both in a beaker. Note: Bromine should be formed immediately so cover it with a watch glass. Then, add about 1.6 ml of Ferroin once the solution becomes colourless. The duration between colour changes should be about 2 minutes. At the end of the reaction, the solution should remain blue. Then, mix 10 ml of each solution and add ferroin via a pipette. Add everything to a petri dish. Your help would be greatly appreciated. I need your help ASAP
I used silver nitrate and sodium citrate to make silver citrate, which resulted in a clear solution which produced white crystals. Is the silver reduced here because of the heat and/or stoichiometry? I've made silver nanoparticles with a few different methods, but mostly with electrolysis, producing a range of concentrations up to completely opaque. At a certain concentration, it resembles anti-freeze. I didn't know about the infrared properties though, that's pretty interesting. Thanks!
The silver should be reduced in every combination, but the low concentrations and stirring lead to the formation of the round particles. The heat is just to increase the speed of the reaction. If the concentrations are higher, it's possible for one or both of the compound to crystalize on cooling or large crystals of silver are formed as a precipitate. Electrolysis to make silver nano particles sounds quite interesting. Are these spherical particles? I wonder how they form at the cathode and are removed. I would have guessed, that there would always be just crystals forming in electrolysis.
@@RaExpIn @RaExpIn I just followed some colloidal silver methods. I've used glucose and cinnamon extract as capping agents, using low current and strong stirring. I cut a silver round in half for the electrodes, and used a small timer and DPDT relay to alternate the anode and cathode a couple times a minute, so I could wear on both halves evenly and avoid contamination from other metals. For the citrate, I followed _"Synthesis and Antimicrobial Activity of Silver Citrate Complexes"_ I use the citrate as a deodorant.
For some reason I didn't get a notification, but I always coming back to your channel so I was able to discover this new upload before too long. Love to see it!
What is the middle beaker 3:47 in the video? Is it a total equilibrium, with the other 2 beakers favoring reactants on the right and products on the left?
It's a diluted solution of the iron thiocyanate complex as a comparison. To the left more thiocyanate solution was added and to the right more iron(III) solution. Both cause the equilibrium to shift to the right side of the equation.
