why is calcium chloride soluble and isopropyl alcohol inslouble??
482786
Isopropyl alcohol is completely miscible with water, as it can hydrogen bond to water.\n\nCalcium chloride is soluble because water is polar and the attractive forces between the calcium ions and chloride ions can be overcome by water.
1183645
E.g. For cements. Calcium aluminates have very good step-wise hydratation properties.\n\nhttp://www.utexas.edu/research/cmrg/projects/CAC.html
560067
According to the solubility rules, it is insoluble.\n\nHere are the solubility rules\n1. All common compounds of Group I and ammonium ions are soluble. \n\n2. All nitrates, acetates, and chlorates are soluble. \n\n3. All binary compounds of the halogens (other than F) with metals are soluble, except those of Ag, Hg(I), and Pb. Pb halides are soluble in hot water.) \n\n4. All sulfates are soluble, except those of barium, strontium, calcium, lead, silver, and mercury (I). The latter three are slightly soluble. \n\n5. Except for rule 1, carbonates, hydroxides, oxides, silicates, and phosphates are insoluble. \n\n6.Sulfides are insoluble except for calcium, barium, strontium, magnesium, sodium, potassium, and ammonium.
82586
It has a cation or anion that isn't soluble. Stuff like NaCl won't work, because Na and Cl are always soluble. KBr has the same problem. But stuff like NaOH (the OH forms insoluble metal hydroxides) works well.\n\nBasically, you have to look at the solution and the precipitating agent and see if they'll form an insoluble compound.
583415
Apparently these pellets (for example, Damp Rid) are calcium chloride (see ref.), a well-known dehumidification and ice-melting compound. So you get a water solution of calcium chloride, which is sort of oily feeling to the touch. Other than being pretty corrosive to metals (like salt water) it's not particularly dangerous, but obviously it's not for internal consumption. Incidentally you can heat the solution and any half-dissolved wet pellets for reuse when dry.
825204
a. Insoluble, chloride salts are insoluble with Cu(I), Ag, Hg2, Pb cations.\nb. Insoluble, because of Cu presence, the only common soluble base is NaOH, KOH, NH4OH, Ba(OH)2, Ca(OH)2, Sr(OH)2.\nc. Soluble, because of Li presence\nd. Insoluble, sulphate salts are insoluble with Ba, Ca, Sr, Pb cations.\ne. Insoluble, all carbonate salts are insoluble in water, except when the cation is Na, K or NH4.\n\npeace\nvixklen
76820
I agree with the previous answer; magnesium nitrate is probably more soluble, at 125 g/100 mL water versus magnesium chloride's 54.2 g/100 mL.  Nitrate's ionic bond (not "bound") is weaker probably because of its higher electron density pulling away from that bond.  \n\nSolubility rules tell us that all nitrates are soluble, but silver, mercury, and lead chlorides are insoluble.
813208
Isopropyl alcohol does not occur naturally.\nIt is produced from propene by indirect hydration in a\ncomplex process known as "strong-acid process", or by\ndirect catalytic reduction of acetone.
762443
I thought this would be easier to answer than it was.  I did finally find it in a reference titled Cosmetics Additives - An Industrial Guide.\n\n\nIt states:\n\ndl-alpha tocopheryl acetate\n-insoluble in water.\n-freely soluble in alcohol.\n-miscible with acetone, ether, chloroform, vegetable oils, etc
423379
let me see if i can at least help you with part of your problem, solubility in chemistry is simple, basically the equation will always be:\n\n[Solubility equalibrium constant] = concentration of product divided by concentration of reagents (concentration of each reagents multiplying by each other).\n\nthe easiest way to understand this is to simplify things for you so as you know, a chemical equation always go like this:\n\nreagents <==> products\n\nJust know this from the above, the dynamic here is that when you have an excess of either the reagents or the product, the balance of the equation tend to shift in the opposite direction (ie excess concentration of product will cause more reagents to form and vice versa), in a chemical equation such as the one from above, the reaction can actually go either way, products or reagents can form.  What really matters is the equalibrium constant that I talked about in the first equation. This constant represent the concentration of the products and the reagents when they are in equailibrium or when they are balance, meaning that the rate at which products or reagent form stays the same and there are no change in the concentration of either the products or the reagents so the whole thing is static at the point.   Think about this, more concentration of products wouldn't form unless you have extra reagents to spare that can shift the balance.  When something is saturated it means that it can longer dissolve in a solvent (let's use water to simplify the explanation)so it just accumulates at the bottom, water molecules can only separate so many ions from each other (the reagents) and preventing them from forming a solid product since water itself has limited molecules (if you mix enough table salt in a glass of water, it'll get to the point where it'll accumulate at the bottom and won't dissolve).  If remember correctly, in a chemical equation, when there's different amount of reagents needed to form the product, there's a slight modification to the equation I gave you, for example:\n\n2 CaCO3 + 4 ZnO2 <----> 3 ZnCO3 + 3 CaO2\n\nthen  [equilibrium constant] = [Cao2]^3 x [ZnCO3]^3 divided by [CaCO3]^2 x [ZnO2]^2\n\nnote that you should balance the chemical equations first, I am just giving an example.\n\nhere's a summary of how to compare numbers, if you plug given concentrations of reagents and product into the equation and the number you get is larger than the real equilibrium constant, then the concentration of products is higher than it should be and the equation will shift towards forming more reagents (in the case of the solid product, it'll dissolve) and if there's more reagents, more solid product is gonna form.  Hope that helps. Remember the Chemistry textbook is still your best reference.
874373
funny question\n\nccl4 is insoluble in water since it cannot form hydrogen bond with water\nsicl4 is soluble in water since it hydrolyse in water to give SiO2\nand HCl
944444
Both calcium chloride and silver nitrate are soluble in water. If you swap the names you get silver chloride and calcium nitrate. Silver chloride is insoluble and calcium nitrate is soluble. So if you mix a solution of calcium chloride and a solution of silver nitrate, an insoluble precipitate of silver chloride will form and calcium nitrate will remain in solution. The balanced equation is \n\nCaCl2(aq) + 2AgNO3(aq) -----> 2AgCl(s) + Ca(NO3)2 (aq)
27502
Simplest reason is that acetic acid is more water soluble than isopentyl alcohol. That five carbon chain on the alcohol is nonpolar and reduces water solubility.
833323
The most obvious reason is because it evaporates so quickly.  The cooling that takes place during evaporation causes water from the atmosphere to condense on it's surface.  This would lead to "wet" crystals.\n\nAlso, upon filtering the purified organic crystals you would see "ice crystals" form on the filter paper as the diethyl ether evaporated.\n\nA practical reason is because it is not one of the better solvents for most organic materials that one would wish to purify by recrystallization.  Alcohols are better for polar materials and benzene, dichloromethane or a petroleum hydrocarbon are better for others.\n\nIn terms of student lab, the anesthetic effects of the ether must also be considered.
634640
The people above are all right, polystyrene is not soluble in Ethanol. However, that's not the issue here. Alcohol contains hydrogens bonded to oxygen, and therefore has some degree of intermolecular hydrogen bonding, which causes surface tension. However, water has a much greater degree of surface tension. Therefore, we can think of water as being slightly "thicker" than alcohol. Now, to understand why alcohol and not water would leech out, you need to understand the structure of a Styrofoam cup. It's made of many small spheres pressed together, and as such has very small spaces between the little balls. The alcohol is thinner, and can more easily go through these spaces.
40729
It's probably ethyl chloride. See link below for more info.
410578
Calcium chloride (CaCl2) I think.