what are the basic steps involved in two solvent crystalization?
139382
First, you dissolve your compound in the solvent in which is is most soluable (perhaps THF or methylene chloride).  Then you very carefully use a pipette to layer the solvent in which it is not soluable on top (perhaps diethyl ether or pentane).  You need to add the second solvent slowly and carefully.  Let the solvent run down the side of the container.  Obviously the top solvent needs to be less dense than the bottom one.  You then let the container sit undisturbed on the bench or in the freezer away from any vibrations until crystals form.  As the upper solvent diffuses into the lower solvent, you compound will become less soluable until it falls out.  The first solution should be as close to saturated as possible.
904363
(NH4)2CO3+MgSO4->(NH4)2SO4+MgCO3
813911
HBr ---> H(+) + Br(-)\nH2SO3 ---> H(+) + HSO3(-)\nCH3-COOH ---> H(+) + CH3-COO(-)
298301
Hmm. This is exactly what I've been doing for the past few weeks. I'm assuming these are aqueous solutions of the three, right?\n\nWell, both magnesium and strontium form precipitates with hydroxides, so you could add some sodium hydroxide and centrifuge it down. To the liquid remaining, add some kind of sulfate, like potassium sulfate, because barium precipitates with sulfates, forming BaSO4.\n\nTo the solid containing strontium and magnesium, add ammonia to make the solution basic, then add sodium carbonate. The magnesium should complex with the carbonate and fall out, forming Mg4(CO3)3(OH)2. Then, whatever's left is strontium.
621890
CaCl2+ 2NaHCO3 + 2H2O------> 2NaCl + 2H2CO3 + Ca(OH)2 \n\n\nyou have to add water molecules on left hand side         \n                                                                                  \nwill this help you?
263822
I've used it as a process in which a compound is dissolved in their recrystalization solvent (found in the Merck index) then filtered. The new filtered solution is allowed to cool and the compounds recrystallize creating more pure crystals. \nLook up types of organic purifications.
781203
2H3PO4(aq) + 3Mn(OH)2(s)  --> Mn3(PO4)2(s) + 6H2O(l)
748872
Cu2+ (aq)  +  Zn (s) -->  Cu (s) + Zn2+ (aq)
131699
Heat the crystals. If it  has water of crystallisation then it will eventually leave the substance. Collect any vapours using a liebig condenser then determine if that is water. Problem is, if you heat it, will it decompose?
622135
Can you collect the vapors that came off the sugar, then mix the black residue with those vapors to reconstitute sugar.\n\nDissolve the sugar in water to make a solution, and then evaporate the water to reform sugar crystals -- no chemical reaction, just a change of state.\n\nChar the sugar (sucrose) with heat, and you are dehydrating it, according to the equation:\n\nC6H12O6 =====> 6 C(solid) + 6 H2O (vapor)\n\nCan you mix water vapor (or liquid water) with the carbon to reconstitute the sugar?  No! Therefore, you have a chemical reaction!
857082
1.  Split up the elements and give them their original charges\n\nAg +\nNO3 -\nK +\nBr -\n\n2.  Combine an element with an element that they were not with, putting them side by side will help\n\nAg + with Br -\nNO3 - with K +\n\n3. So now you have 2 new compounds\n\nAgBr & KNO3-\n\n4.  Their should be a chart in your book that tells you which compound would be the precipitate but i don't think their is a precipitate for this reaction'\n\nso both will dissolve in a solution
429768
To perform a solution-based separation, you need a solvent in which one or some of the solutes (in the mixture to be separated) is/are highly soluble, and in which the other components are highly insoluble.\n\nA simple example might be separating an ethanol/pentane mixture by using water.  Ethanol, being polar, will readily dissolve in water; but the nonpolar pentane will not.
290781
MgSO4(s) + 2HCL(aq) ---> H2SO4(aq) + MgCl2 (aq)
608403
NaOH (aq) + HCl (aq) --> NaCl (aq) + H2O (l)
905525
In general smaller particles have more surface area so the solvent can solvate and pull molecules away from the bulk crystal more efficiently.  \n\nThe key to solubility is solvent access to the solid material. \nOn a surface of a particle only the outermost part can be solvated so if there is a lot of surface area in one sample compared to another, the large surface area to volume ratio particles will dissolve more efficiently.
903593
Crystal Energy et Active H\n\nSouriez à la vie et la vie vous sourira. ^---^
582636
Try dissolving sugar in water then freezing it this is a solid solution. The solute is the sugar and the water is the solvent