In which of the following solution will CaF2 be most soluble?
410572
according to the common ion effect, placing CaF2 in either solution will decrease its solubility.  However when having to choose between the two, it will be most soluble in Ca(NO3)2.  This is because Ksp=[Ca+][F-]^2  The fluorine component is squared making it a bigger factor in lowering the solubility.
942442
According to a book I read some time back, "Mellor's Modern Inorganic Chemistry," fluorine is stored in copper lined cylinders.  The F reacts with the Cu, forming a layer of CuF2, which prevents further attack.  Here's a good document on everything you ever wanted to know about handling fluorine:\nhttp://www.llnl.gov/es_and_h/hsm/doc_14.06/doc14-06.html\nI couldn't find anything on cost.
1135506
Dilute the stock solution.\n\nBe careful, though. Trifluoroacetic is very noxious stuff. My undergrad organic teacher said that he handled inorganic acids for years, with no problem. First day he handled trifluoroacetic, he burned himself.
459648
Themes > Science > Chemistry > Miscellenous > Help file Index > Precipitation Equilibrium > Ksp and Ion Concentration \n\nThe solubility product constant can be used to compute the equilibrium concentration of ions in solution in the same way that you use other equilibrium constant expressions to compute equilibrium concentrations. \n\nUse the Initial, Change, Equilibrium method to compute the concentrations: write the equilibrium expression, the initial amounts of each thing in the expression, how much they change by, then the equilibrium amounts. From that, you can compute the concentrations of all species. \n\nExample: BaF2 has a Ksp of 1.8*10-7. What is the concentration of barium in a saturated solution of BaF2? \n\nSolution:. First, write the balanced equation and the solubility constant expression: \n\nBaF2(s) < = > Ba+2(aq) + 2F-(aq) \nKsp = [Ba+2][F-]2\nWe start with no barium or fluoride ions in solution. If we set the amount of barium ions formed to x, then the number of flouride ions formed is just 2x \n\n [Ba+2] (M) [F-] (M) \nInitial 0 0 \nChange +x +2x \nEquilibrium x 2x \n\n\nNow plug in the equilibrium values shown above and solve for x \nKsp = [Ba+2][F-]2 \nKsp = (x)(2x)2 \nx = 3.6*10-3\nSince we defined the concentration of Ba+2 to be x, we've solved the problem \n[Ba+2] = 3.6*10-3 \n\nInformation provided by: http://learn.chem.vt.edu\n \n**try to visit the site below..** You can calculate the Ksp based on the above example..I'm sure the answer is in your books and notes..have fun learning..
962805
Insoluble amines can be made soluble by adding acid to the solution.  This forms the ammonium salt which is ionic and soluble.  Therefore the answer would be b, HCl.\n\nA similar strategy can also be used by adding base to carboxylic acids and phenols with low solubility.
889156
The answer is BrF3.\n\nand the balance equation is \n\nBr2  +  3F2  --->  2BrF3\n\nhow? get the moles of each using this formula:\nn = PV/RT\n\nyou'll get:\nmol Br2 = 0.041mol\nmol F2 = 0.123 mol\nmol pdt = 0.082 mol\n\nbase from this, you'll found that ratio of Br:F is 1:3. Hence, the product is BrF3. you'll also found that ratio of Br2:F2:pdt is 1:3:2 which also agrees with our balance equation above.
64690
NA2SO4,KOH,AGCL,CA(NO3)2 ARE SOLUBLE.AND HG2BR2 AND CDS IS INSOLUBLE.
962405
I think SO2, because the charge is -2.\n\nBy the way,I don't kno the cahrge of ClF3, sorry
436191
Uh, the rest of the question isn't appearing. But it's an equilibrium solubility problem. Write a reaction:\n\nMgF2 --> Mg+2 + 2F-\n\nKsp = 5.52e-9\n\nFill in the values on the ICE table (I don't know them, the numbers are missing), and set an equation up.\n\nKsp = [F-]^2 * [Mg+2]\n\nSolve with the numbers from the ICE table. Remember that those concentrations in the above equation are the equilibrated concentrations, not the initial.\n\n\nHope this helped.
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.
117753
Okay you have a choice between Potassium oxalate (K2C2O4 ) and Sodium Iodide (NaI). \n\nPotassium oxalate is highly soluble (30g/100g) and sodium iodide is even more soluble(184 g/100 ml).\n\nWithout knowing the reactants it is almost impossible to predict a product, especially with two choices. Given those two products, I would expect it to be K2C2O4, but that is just a guess. What was in the solution?
749219
a) Ag2S\nb) SnCl4\nc) Na3N\nd) SrI2\n\nDo us a favor and pay attention during class. That way you'd know how to do these.
1092099
to determine whether an acid or a base is soluble in say the universal polar solvent water, u should be knowing whether the substance is strong or weak\nnow bases like NaOH, CsOH, RbOH, Mg(OH)2 are strong bases and in solution they give us the cations and anions(mostly the hydroxyl grp)\nbases like Be(OH)2, Fe(OH)2 or 3, Cu(OH)2 or any of their oxides are weak and hence in solution they do not undergo complete dissociation and most of these are insoluble\nso in case ur not in a lab, the only way is to identify their degree of weakness
1172979
Lead II Nitride\n\nCa(BrO2)2
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.
911120
2BF3 + 3Li2SO3 → B2(SO3)3 + 6LiF\n3CaCO3 + 2H3PO4 → Ca3(PO4)2 + 3H2CO3\n8Ag2S → 16Ag+S8
864248
I understand that the compound in question is soluble in both pet. ether and ethanol. The reason why pet. ether is preferred must be to do with the volatility of pet. ether. \n\nYou can easily evaporate pet. ether, which is why this is preferred over ethanol. \n\nThanks.