Could someone tell me what two common substances are insoluble in water?
919136
Most fatty substances such as oils ,butter etcc.. However it does not mean that they cannot remain suspended as particles in the water. Such would be called an immulsion.
38135
Well, I can give you three nonflammable liquids that are mutually immiscible...\n\nwater\ncarbon tetrachloride\nmercury\n\nMost things that are immiscible with water tend to be nonhalogenated solvents and therefore flammable.
2508
Weak acids and organic acids in water.\n\nBut remember the solution depends on what the solvent is.  In water, the seven strong acids essentially completely ionize...i.e. can be considered completely ionized.
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
830186
Polar substances like ionic compounds and salts are water soluble, non-polar substances like fat and oil are insoluble.
80429
The CRC Handbook of Chemistry and Physics has all kinds of good information like that (although it is pricey).\n\nOr, search the web for the specific liquid of interest.
345145
O2 is the least soluble in water, followed by Br2.\n\nthe problem is that both LiCl and methanol dissolve completely in water. LiCl since it is an ionic compound, and methanol since it forms hydrogen bonding with water. Therefore any order for LiCl and methanol would be correct I presume.
921966
Br2 is extremely soluble in CCl4 - much more soluble than in water.\nLook up "partition".
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
864649
Solute is anything tht is disolved in the liquid. If there was no solute, all you'd have is distilled water.
985052
Tap water.\nSoap breaks down the surface tension.
781072
useful substances enter and waste products exit of course.\nuseful substances include glucose, oxygen, amino acids, etc.\nwaste products would be carbon dioxide, urea, etc.
486005
Anything that dissociates well in water. Any strong acids or bases are good, so are salts of those since they exists as ions in solutions. Weak acids and bases are weak electrolytes, since they don't dissociate as well. The most common is probably table salt, NaCl. Potassium by itself is just a metal the reacts violently with water and is not a good electrolyte, but potassium compounds are, as are sodium compounds. \n\nNote: Remember, just because something dissolves well doesn't mean that it is necessarily a strong electrolyte., it must also dissociate into ions. Sugar dissolves in water, but since it doesn't separate into ions it is not an electrolyte.
135415
That's a difficult question to answer because magnesium hydroxide is practically insoluble in water with a ksp value of like 1.8 x 10^-11 so very little magnesium hydroxide is dissolved in water.  But if you were to compare the solubility of magnesium hydroxide at 25C with 80C my guess is that it would be more soluble at a higher temperature but only by an almost insignificant amount.  \n\nIn short, Mg(OH)2 is pretty much insoluble in water so my direct answer after all the reasoning would probably be: no, Mg(OH)2 does not fit the pattern due to its extremely low solubility.
41331
Hg2Br2, BaSO4, AgCl, PbCl2, Al(OH)3, are insoluble\nKBr is soluble.\nYou can refer to this link for details on solubility of salts.\nhttp://chemed.chem.purdue.edu/genchem/topicreview/bp/ch18/soluble.html
607804
The easiest way to prepare an insoluble salt is to produce it from two aqueous solutions each containing an ion present in the salt!\n\nSo, you'll just mix two solutions, and the insoluble salt appears! Of course, if you intend to prepare a certain amount/ mass of the salt, you may need to carry out some calculations to determine the necessary concentrations/ volumes of the 2 initial solutions. \n\nYou'll also get another product in the reaction, but it should be soluble and will not contaminate the desired product (the insoluble salt).  \n\nYou may refer to this website to gain a better understanding...\nhttp://www.wpbschoolhouse.btinternet.co.uk/page01/AqueousChem/AqueousChem.htm#salts [Refer to point (4)]
444550
The difference in solubility of the components allows for separation.  I don't remember the specifics, but that is the reason.  Water will not have a big enough difference.