What is the apparent solubility of magnesium sulfate in distilled water?
828232
As I've answered elsewhere, the solubility of the Group 2 sulphates decreases as you go down the group. MgSO4 is reasonably soluble, therefore, but BaSO4 is pretty insoluble.
982289
low solubility; im sure
516306
Until the concentration of salt is large enough to form a saturated solution, ie. one in which no more solute will dissolve, the volume of the solvent (water) will not change.  20g of salt is not nearly enough to form a saturated solution, so the water level will remain at 500ml.
46964
It determines the number of ligands the ion can be surrounded with, both in the crystal and in solution. (Electronic configuration dictates the likely geometry.)\n\nThere is no direct correlation. Stability of the salt depends among other factors from the ionic character of the salt - some of the badly soluble sulfides have bonds with covalent character.\n\nThe energy gain from dissolving the salt (allowing free movement of formerly ordered crystals) has to be greater than the energy required to leave the crystal. Usually the ionic ligands in the salt crystal are replaced by water molecules.
751720
chromium (II) sulfate fo sho
36586
Ag+ + SO4(2-) ---> Ag2SO4\nYeah, it's double replacement, and according to my solubility rules, AgSO4 is insoluble.
655901
You really need to give a little more information about what you are attempting to convert.  However, in very general terms you remove the sulfate, usually by making a solution containing your material basic.  You then form the hydrochloride salt by adjusting the pH back to the acid side via the addition of hydrochloric acid.\n\nPlease note, this process applies to the salt conversion of materials that are basic in nature and water soluable as their salt form.
568319
in water the solubility is -6.26440763228718
64690
NA2SO4,KOH,AGCL,CA(NO3)2 ARE SOLUBLE.AND HG2BR2 AND CDS IS INSOLUBLE.
438725
Magnesium Sulfate\n\nMgSO4\n\nMg(OH)2 + H2SO4 -> MgSO4 + 2HOH\n\nHOH = H20\nJust in case...
429367
It doesn't form into anything. You said it yourself, it's soluble. The hydroxide part of the milk of magnesia (magnesium hydroxide) and the hydrogen of the sulfuric acid combine to form water, but then you're left with Mg+2 and HSO4- ions. It's just a clear liquid.
568138
I think it should be lower, coz i checked my data book and there is no value of solubility for copper sulphate, salt is 3.03*10 squared.
513514
Crystallization of solution of CuSO4.
702225
there are 5 ways to prepair MgSo4 \n\n-neutralisation between acid and alkali(but this is espcially for sodium and potassium salt)\n\n-Acid and metal (magnesium and sulphuric acid)\n\n-Acid and metal oxide (magnesium oxide and sulphuric acid)\n\n-Acid and metal hydroxide (magnesium hydroxide and sulphuric acid)\n\n-Acid and metal carbonate (magnesium carbonate and sulphuric acid)\n\nthese methods are especially for soluble salts...
799105
Assume you have the salt AxBy and the molar solubility is s.\n\nThen\n\nAxBy <=> xA^(+y) +yB(^-x)\ns mole/lt\ngive... .. .. ..xs .. .. .. ..ys\n\nKsp=([A(+y)]^x) *[B(-x)]^y =(xs)^x * (ys)^y=>\nKsp= (x^x)*(y^y)*s^(x+y)\n\ne.g. for Fe3(PO4)2 tou have x=3, y=2, so\nKsp=(3^3)*(2^2)*s^(3+2)= 36s^5
969567
You can evaporate, or distill off the water.  Then you'll get the CuSO4, along with any non-volatile impurities that may be present.  Or you can do a recrystalization.  You boil the solution until the CuSO4 just starts to crystalize out.  Then you let the solution cool.  As it cools, the solubility of the salt decreases, and more & more of it crystalizes.  When cooling, you may end up with a super-saturated solution, instead of crystals being formed.  In that case, scratching the inside of the beaker with a glass rod will initiate the crystalization process.  With recrystalization, the product is also purified.
1079987
No safe way to do it.  Distillation perhaps, but that's not safe as sulphate fumes are not that good for you.  \n\nGrab the stock bottle and make up a fresh solution.