how do solvents work?what happens?the cause and effect of solvents?
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A solvent is a liquid that dissolves a solid, liquid, or gaseous solute, resulting in a solution. The most common solvent in everyday life is water. The term organic solvent refers to most other solvents that are organic compounds and contain carbon atoms. Solvents usually have a low boiling point and evaporate easily or can be removed by distillation, thereby leaving the dissolved substance behind. Solvents should therefore not react chemically with the dissolved compounds — they have to be inert. Solvents can also be used to extract soluble compounds from a mixture, the most common example is the brewing of coffee or tea with hot water. Solvents are usually clear and colorless liquids and most of them have a characteristic odor. The concentration of a solution is the amount of compound that is dissolved in a certain volume of solvent. The solubility is the maximal amount of compound that is soluble in a certain volume of solvent at a specified temperature.\n\nThe link below will have resources on specific solvents and their behavior.
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Solution is the mixture of a solvent and a solute ,where the solute dissolves in the solvent.
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If you mean to ask what the difference between a solution and a suspension is, then a solution is when the solute is dissolved into the solvent completely, and a suspension is when energy must be constantly applied to the mixture in order to keep it mixed up (like shaking, stirring, etc.)\n\nHope this helps...
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How Anesthesia Works\nhttp://health.howstuffworks.com/anesthesia.htm
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Non-Polar Solvents:\n> Hexane -( CH3-CH2-CH2-CH2-CH2-CH3 )\n>Benzene  (C6H6 )\n>Toluene  (C6H5-CH3 )\n>Diethyl ether  (CH3CH2-O-CH2-CH3 )\n>Chloroform  (CHCl3 )\n>Ethyl acetate  (CH3-C(=O)-O-CH2-CH3)\n> Dichloromethane  (CH2Cl2 )\n\nPolar Aprotic Solvents:\n>1,4-Dioxane  (&#92;-CH2-CH2-O-CH2-CH2-O-&#92; )\n>Tetrahydrofuran (THF) ( /-CH2-CH2-O-CH2-CH2-&#92; )\n>Acetone  (CH3-C(=O)-CH3 )\n>Acetonitrile  ((MeCN) CH3-C≡N )\n>Dimethylformamide (DMF)>> ( H-C(=O)N(CH3)2 )\n>Dimethyl sulfoxide (DMSO) >>> (CH3-S(=O)-CH3 )\n\nPolar Protic Solvents:\n>Acetic acid  (CH3-C(=O)OH )\n>n-Butanol  {CH3-CH2-CH2-CH2-OH }\n>Isopropanol  {CH3-CH(-OH)-CH3}\n> n-Propanol  {CH3-CH2-CH2-OH }\n>Ethanol  {CH3-CH2-OH }\n>Methanol  {CH3-OH }\n>Formic acid  {H-C(=O)OH }\n>Water  {H-O-H }
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First, you dissolve your compound in the solvent in which is is most soluable (perhaps THF or methylene chloride).  Then you very carefully use a pipette to layer the solvent in which it is not soluable on top (perhaps diethyl ether or pentane).  You need to add the second solvent slowly and carefully.  Let the solvent run down the side of the container.  Obviously the top solvent needs to be less dense than the bottom one.  You then let the container sit undisturbed on the bench or in the freezer away from any vibrations until crystals form.  As the upper solvent diffuses into the lower solvent, you compound will become less soluable until it falls out.  The first solution should be as close to saturated as possible.
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because in osmosis/ diffusion, solvent / solute moves across a barier to balance the concentration. since the water is saltier than normal, either water has to come out of the cells to dilute it, or salt has to go into the cells to make them more concentrated. either one is bad for cells, but in terms of osmosis, it is the water that does the moving, leaving the cells dehydrated.
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I agree with the first poster on C and E, but I'm not sure if A is also.  A solute dissolving in a solvent seems like a chemical process to me, but I don't remember for sure.
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I would have to guess that it involves the neutralization reaction of more than 2 substances.\n\nJust a guess
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Couldn't you evaporate the solvent? I think it's water or ethanol.
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CO2 makes the bubbles.\n\nAt the time of preparation CO2 is dissolved in the drink (water being the solvent) at a high prssure.\nSolubility of CO2 increases at high pressure so more gas is present as the dissolved gas.\n\nWhen the bottle is opened the extra pressure is released and so the excess dissolved gas (under pressure) becomes surplus at normal pressure and so the gas (CO2) escapes in the form of bubbles.
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depends if the mixture is bonded by a physical or chem bond....there is magnetic separation,distillation,fractional distillation,evaporation,crystallization...etc...why dont u look up a chemistry book
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dont ask us your homework online, you actually need to learn the stuff.\n\nappended:\n\nliquids are gasses, but something a gasses become liquids when they are pressurized enough to where gravity is able to overcome the kinetic (heat) energy of the mollicules.this causes  seperate from lighter gasses, and sink to the bottom. at low pressures or gravity, liquids become gasses, and vice versa.
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It takes energy not only to break up the solid solute into its individual particles, but also to force the solvent molecules apart.  Now, if the solute can offer the solvent some very attractive forces (like sodium ions and chloride ions do from table salt) the whole process will work. The energy required to break up chalk is just too great.
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chemical reaction\n\nall substance give off some heat during change\n\nlook up kinetics on the web
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In short: Any solution will boil at a higher temperature than the pure solvent. \nBoiling point elevation is a colligative property. Use the formula provided by emilyrose. The addition of salt to water causes vapor pressure reduction of the water. This is because the addition of a non-volatile solute causes a reduction in the surface area available to water molecules, reducing the likelihood of evaporation. This vapor pressure lowering is described by Raoults Law (see link).\nInterestingly, if you have a salt solution, and you heat it till it boils, as the water evaporates, the boiling temperature of the solution will continuously increase, because its molality increases. Please see the link below for a more detailed discussion.
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if i recall correctly you are mixing two (or more) substances together, generally liquid, and solids form and precipitate out of solution.  (basically some solid chunks form from the mixture of the liquid)