This is a chemistry question. a supersaturated solution is one that ontains more solutes than usual. This kind of solution is always necessary for crystallization. Why?
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Precipitation, or crystallization, only occurs when the solution is already holding more solute than it can regularly hold. As a result, the hypercollisons of the molecules cause bonding between them to occur and for the solute to precipitate.
184013
Water of crystallisation is the water which combines with the salt during crystal formation and gets attached to it and results in some very interesting properties of the crystal..\n\nIt depends on the nature f the salt, the temparature, the time of crystallisation, the catalysts and other factors.\n\nTry searching on google to get more info on water of crystallisation.
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whey is a protein which when seperated from the curdor casein which form a solid , remains a liquid in suspension\nof itself there is no surface tension as that is born by the casein - whey has a freezng point lower that water because of it's fat content and it's viscosity by that very nature,\nthough variable is more dense that most liquids
410443
Precipitation:: Precipitation is the formation of a solid in a solution during a chemical reaction. When the chemical reaction occurs the solid formed is called the precipitate. This can occur when an insoluble substance, the precipitate, is formed in the solution due to a reaction or when the solution has been supersaturated by a compound. The formation of a precipitate is a sign of a chemical change. In most situations, the solid forms ("falls") out of the solute phase, and sinks to the bottom of the solution (though it will float if it is less dense than the solvent, or form a suspension).\n\nThis effect is useful in many industrial and scientific applications whereby a chemical reaction may produce a solid that can be collected from the solution by various methods (e.g. filtration, decanting, centrifuging). Precipitation from a solid solution is also a useful way to strengthen alloys.\n\nAn important stage of the precipitation process is the onset of nucleation. The creation of a hypothetical solid particle includes the formation of an interface, which requires some energy based on the relative surface energy of the solid and the solution. If this energy is not available, and no suitable nucleation surface is available, supersaturation occurs.\n\n\n\nAggregation::Particle aggregation in materials science is direct mutual attraction between particles (atoms or molecules) via van der Waals forces or chemical bonding.\n\n\n\nCoagulation::The transformation of liquid into jelly like semisolid mass.\n\n\nFlocculation::Flocculation refers to a process where a solute comes out of solution in the form of floc or "flakes." The term is also used to refer to the process by which fine particulates are caused to clump together into floc. The floc may then float to the top of the liquid, settle to the bottom of the liquid, or can be readily filtered from the liquid.
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WHOA !!! you have a contradictory question..emulsification is NOT the same as solubility. What do you want to do ? Emulsify or dissolve ?
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Tap water evaporates as it sits around.  The additives become more concentrated as the water evaporates but they don't dissipate.  Eventually they "precipitate" as salts and end up as solids in the container.
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Sounds like you've got too much time on your hands to me!  The ions in solution keep the water molecules farther apart from eachother on average than they would be in pure water.  Therefore the hydrogen bonds are weaker and the water will boil at a lower energy level.  At least that's what I'd guess.
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Yes definitely! This is for the simple reason:-Tap water is likely to contain dissolved salts, and other impurities. But distilled water contains only water, and hence better.
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wow, well put mrjeffy! I have one thing to add though. Because all acids and bases are electrolytes, you can use pH to determine what is and isn't an electrolyte in a solution. If it come out as acidic or basic, it is and electrolyte(the darker, the more basic or acidic). If it comes out neutral, like Distilled Water, it is not. Also don't forget that non-electrolytes will not completely dissolve into solution in water.
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Most solutes (sugar in this case) have limited solubility (ability to dissolve) in most solvents (water in this case). This solubility varies with temperature - the hotter the solution, the higher the solubility. As mentioned in an earlier answer, this means more energy must be added to dissolve more solute. On the other hand, if energy is taken out of a solution, the solute will usually  come out of the solution, depending on the concentration.\n\nThis physical law that governs this is the 2nd law of thermodyamics.
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This is a poorly worded question.  All chemicals have some solubility in water, however minute.\n\nOf these selections, I would go with A\n\nAdding a charge facilitates dissolution.\nMany covalent materials (oil) have low solubility \nMany large molecules are water soluble (Poly Ethylene Glycol)
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If by 'undissolved' you mean why are some salts insoluble in water, then I think we are in business.\n\nIn order for a salt to be soluble it has to be energetically favorable for the ions to separate. This requires a negative gibbs free energy. G = H - TS So you have to find the H and S values for the solid to aqueous solution and see if G will be negative for a given temperature.\n\nA method I recently learned to make insolube salts more soluble is to add other ions to the water...but you have to be careful to not add a common ion...or Le Chantliear will come into play.
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What about boiling points?  Or regular melting points?
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Supercooled state is usually reffered as \nsuper-cooled-liquid. ---\n\nGlass is an example of supercooledliquid or a supercooled state.\n\nGlass and other matters are apprently solids but referred as in supercooled state because of their irregular molecular distribution which is similar to liquids. Solids have a geometrical arrangement of molecules.
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solutes such as ions, greatly increase boiling point and reduce the freezing point thank you\n\nexplaination... have things to do with attraction between molecules and bonding..
555127
The lead compounds would be much more covalent in character, with a very high bond strength (aka lattice enthalpy). Where a compound is insoluble, this energy is too high for hydration enthalpies (the energy released when water surrounds an ion of either charge) to compensate for.
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A concentrated solution has more sugar and is more conductive.