hermanntrude

A vacuum pump can remove most of the air from inside of beaker, although it is impossible to create a perfect vacuum. Here is a company who sells pumps specfically for chemistry labs, I don't have any experience with the company they simply came up in my search.

 

If you use a vacuum pump to remove the air from inside a container the pressure inside drops.

our policy on homework (or coursework) help, even if it isnt in the homework help forum, is to NOT directly answer it. Give the poster clues or references and links so that they can figure it out for themselves.

decomposition of H2O2?

i'm gonna need more. Which chalcogen? sulfur? and how is its name sunny?

copper sulfate changes colour depending on how hydrated it is. [ce]CuSO4.5H2O[/ce] is blue, as you know, but copper sulfate with less water associated can be greenish, and completely anhydrous copper sulfate is a white powder, which slowly turns greenish blue as it absorbs water from the atmosphere.

Of course... it could be impure, too

sapphyrin

 

Your first mistake was mentioning it in IRC a while back.

 

I am a polycyclic aromatic molecule with a rather sunny name, consisting solely of carbon and a chalcogen. What am I?

solely carbon and a chalcogen? no hydrogen?

i'm like a porphyrin, but with an extra pyrrole unit per ring. I am unbelievably difficult to make.

do you have access to an nmr machine? that'd be pretty conclusive...

otherwise you could try this

seeing as UC said anyone can post one here's another:

 

This metalorganic compound is pretty unsavoury. if it was a person you'd say he was a real ass.

 

The molcular structure of this compound looks quite similar to what its name suggests but this is purely coincidental.

arsole?

Seeing as batteries are chemical, I've moved this to Chemistry for you. Perhaps one of our resident chemistry experts will know the answer.

<runs away and hides>

 

next one, this element sounds like it steals the letter L

nickel!

______________________________________

next:

A non-toxic element, surrounded in the periodic table by toxic elements, the active ingredient of pepto-bismol.

I made a plastic which was purple once. It was a star-polymer based on porphyrins. it's in "macromolecules"

certainly it's a fairly simple one. perhaps you could build a machine with an analytical chemist inside it, a food tube, water tube, evacuation tubes and an air supply and a depository station for you to send in samples... then you'd have a machine for doing it all. Fairly cheap, too

the first few experiments would be to determine whether it was organic or inorganic, aqueous or non-aqueous. After that, depending on the results, the tests would be different.

If it turned out to be organic, NMR, IR and melting-point or boiling point information would be useful. Perhaps a mass-spectrum too.

If it was an inorganic substance dissolved in water I'd probably give it to an inorganic chemist and tell them to do it for me :0)

i

 

do you know that water we drink consist of very small amount D2O(heavy water) and T2O ,and salt to taste ................

it should also contain small quantities of HOD, TOD and HOT! (or DOH, TOH and DOT!)

every week or two we get someone asking how to make ethanol or methanol gel. try the search function

I'd like to remind members that since this topic is based around some very dangerous materials, perhaps it'd be wise only to respond if you actually know what you're talking about and have tried the experiment you're reccommending for yourself in a controlled environment without burning your face off.

didn't you already ask this question and then abandon the thread?

if the answer is at all possible or feasible, it's in this thread.

guess how I found it

answer: (highlight this line to see it):use the search function!!!!

wine is often sold in bags, but the bag is a strong one and placed inside a box... probably for this reason.

check all your math and if your answer still comes out as 3, simply write an explanation of why that might be and leave it at that.

You can get a very high mark in a lab without getting perfect experimental results. Instructors are usually looking more for an understanding of what you're doing than a perfect execution of the method.

that synthesis seems to have worked but as you can see it's extremely dangerous. Anyone reading this thread should think LONG and HARD before attempting to recreate the reaction. Note that the guy who did the reaction was badly hurt and could easily have been blinded or permanently scarred.

Even without the extremely silly idea of pouring water onto hot sodium, the rest of the reaction could use a bit more attention to safety.

To be honest i'm not totally comfortable with this link being on our site for the safety of some of our more confident and less-skilled members.

well you chose the most difficult groups to isolate. Groups I and II are just not very stable as the elements. The one nearly everyone seems to want is sodium but I see you already have some of that. Please be VERY careful with it. Also remember that any water you drop that sodium into will become a solution of sodium hydroxide which is also very hazardous.

The other group I elements are essential impossible to make at home, and even if you could do it I'd suggest that you shouldn't try, because the dangers are far too great.

Some of the group II elements might be possible (perhaps calcium?) but i'm not up on the techniques.

If you want some magnesium, simply buy or find an old metallic pencil-sharpener.

No?

pretty lousy synthesis if you can't purify the sodium... anyway, what proof do you have that you/they made sodium? it reacts with water? so would hot powdered magnesium... so would a lot of things.

I'm not saying you/they didn't make sodium... i'm saying you/they haven't proven it, and the burden of proof is on you or them.

I also have concerns about your reaction vessel... what was the pan made of? how can you be sure it wasn't involved in the reaction?

the pH scale is really only applicable to aqueous solutions, since it is the negative logarithm of the concentration of hydronium ions.

Now while there will be a few hydroxonium ions in any solution, no matter how dry, unless there is a VERY significant impurity in the non-organic solution, the concentration of hydronium ions will be very very low indeed, which, in an aqueous solution would translate to a high pH (perhaps 13 or 14), which would also mean that the hyoxide ion concentration would be very high, which would mean the solution was basic and probably highly corrosive. This isn't true of our non-aqueous solution, though, since there may be no hydroxide ions at all or, more likely, exactly the same amount as there are hydronium ions, meaning the solution is actually neutral.

Remember that in an aqueous solution, pH and pOH are tied together via PKw (PKw is the legative logarithm of the equilibrium constant for the auto-ionization of water ([ce]2H2O <=> H3O+ + OH- [/ce]). pH + pOH = pKw = 14), but this doesnt work in a non-aqueous solution because any water that is present is an impurity and therefore part of a mixture rather than a pure aqueous solution.

P4o10?