How do i separate sulphur and sand, and what method do i use?
551708
heat it up, the sulphur will burn off.\n\nor mix with water and filter out the sand, then evaporate the water to get the sulphur.
458134
hope this helps you out. molding clay is what i would use.
225104
Lots of regular gravel and sand of different sized granuels. They use finer material thedeeper in the leech pit you go until you will eventually get clean water out the other side. (Hopefully)
327571
I would think the best way to do this is to dry the sample and then turn it into a powder.  You could then perform an extraction of the metals possibly with Conc. HCL or HNO3.  There may be an organic solvent that could do this extraction but many of these solvents are not compatible with the plastics in AAS autosamplers.  Preparing the blanks would be the same as any other AAS standards.  Prepare an acid solution to match that of your sample and determine if and how much of each metal is present in your acid.  It is also good just for reference to run a blank of the water you are using.  When preparing the standards for the individual metals read some of the literature to determine the best method (ashing temp, atomization temps. etc.).  In many cases better results are obtained with the use of a matrix modifier.  I would read some literature and there should be many examples of this type of work.
163000
there is really no way of controlling the sulphur. is it the smell that you are trying to control, or the amount of these emmissions that are escaping?
402174
You can Use Dean and Stark Apparatus To Separate them \n\nAlso one Source i m providing you which involve the separation using PTC\n\nRefer it \n\nhttp://www.ptcorganics.com/Top10PTC.pdf
903862
Sorry Voyager. Copper is not so reactive a metal that it will react with sulphuric acid.\nYou need either solid copper (II) carbonate or solid copper (II) oxide for the salt.\nSince it is a sulphate, sulphuric acid is used together with the solid.\nHeat the acid so that the reaction can proceed at a faster rate. Add solid till no more will react (no bubbles of gas produced, and the solid remains insoluble). This is to ensure that all the acid is used up. Filter to remove unreacted solid and heat the filtrate, which is the copper (II) sulphate solution, till saturated (approximately 1/3 to half the original volume left would be a good gauge). Let the hot saturated copper (II) sulphate solution cool and after some days, when the excess water evaporates off, you should get hydrated copper (II) sulphate crystals.\nDo not heat till dryness as this will evaporate off the water of crystallization needed for the blue copper (II) sulphate crystals to form. Without the water of crystallization, you would get anhydrous copper (II) sulphate powder (white) and not the blue crystals.\n\nHope this helps :)
757083
Look at USES\n\nhttp://en.wikipedia.org/wiki/Sulfur_dioxide
1027323
Well it looks like in the first experiment the mass of sulfur was doubled to obtain the sulfur dioxide. So divide 0.842g by 2 to get the original amount of sulfur used. It would be 0.421 g of sulfur.
718889
You can use something called a sand bath or a water bath (for the wax not you!) You can also keep it in a crucible and in a microfurnace. Your lab should have these facilities.
72719
This sounds so excessive! What a crazy teacher you must have. :)\n\nAlright - well...\nThe gravel is the easy part. Use the screen as a sift and hopefully the screen will be fine enough that none of the gravel will get through. \n\nNow the plan of action is dump the powder and salt in the water. [Which I guess will be done in Cup #1.] You'll filter out the powder. The salt will dissolve in the water, and you will evaporate the water later. The question is how to do this with what you have.\n\nI'm thinking the craft sticks are to hold up the funnel. Arrange them over the top of the cup [Cup #2] so that they make a triangle and see if it'll hold up the funnel. \n\nPut a filter paper in the funnel. Pour the mixture in and the powder will collect in the funnel. When you're done, take out that first filter paper and set it aside. Then set up your funnel in Cup #3 with the second piece of paper and filter the mixture a second time just to make sure you got all of the powder.\n\nI was trying to think of what the syringe could possibly be for, and the only thing I can think of is to take the salt-water out of Cup #3 and into the evaporation dishes.\n\nNo idea what the magnifying glass is for.\n\nBut the basic idea is that you sift out the gravel, mix the powder&salt in water, fliter out the powder, then dissolve the water.
516829
Preparative HPLC should do the trick.  Try a search at these to see if an exact procedure might be on the web.\n\n\nhttp://www.scienceresearch.com/search/\n\nhttp://www.scirus.com/srsapp/
1070616
mix concetrated sulphuric acid to the sodium acetate, the reaction will produce acetic acid and sodium sulphate.\n\nif you take all the water out of the sodium acetate, you will end up with 100% pure acetic acid.\n\nH2SO4 + CH2COONa => CH3COOH + Na2SO4\n(unbalanced equation)
1097636
You need a solution of gold sulfate or gold chloride to do it, but it has to be extremely pure, made with distilled/deionized water.  Remember to have your ring on the anion (the negative) and your gold source on the cation.
94062
I wanted to help you but I just wonder where the sulfur atom in SO2 comes from? Sulfuric acid, maybe, somewhere in your process? Or is it SeO2? These have to be clarified first to get a reliable answer.
653331
As said before you can do the classic baking soda and vinagar, but a more dramatic reaction between sulfuric acid and sugar. Mix concentrated sulfuric acid and sugar in a well ventilated glass beaker or container and the acid will dehydrate the sugar leaving a stack of pure carbon
971882
Easy!\nStir the mixture into water. Sand sinks. Styrofoam floats.\nScoop the Styrofoam off the water surface with a strainer.\nPour off the water.