what are azeotropic mixtures?
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A liquid mixture of two or more substances that retains the same composition in the vapour state as in the liquid state when distilled or evaporated under some conditions
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Solid,liquid and gas.
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a)mixture..they are together but they are not bonded\nb)mixture\nc)compound\nd) compound...the molecules are chemically bonded
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e.g. of formula: Magnesium+oxygen=magnesium oxide\ne.g. of Mixture: Air\ne.g. of Compound: Magnesium oxide
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mixture is combining substances, solution is dissolving a substance in another
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None. They are two different compounds.\n\nIt looks like you want to compare a specific property of the alcohols. Please specify!
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substances that have crystallization water trapped inside their molecules :D
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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.
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a. Silver nitrate\nb. isopropanol? methanol?\nc. Potassium chloride\nd. Benzene\ne. Carbon monoxide\nf. Sodium hydroxide
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Its a mixture of hydrocarbons. It doesn not have a name because it is not composed of one compound.
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Air is is mainly nitrogen  and oxygen with a mixture of other gases.\nmilk is proteins, fats, lactose, and various vitamins and minerals.\nBronze is various alloys of copper and tin and some bronze will contain other metals too.\nSugar is a sweet cystalline or powder derived from sucrose and lactose obtained mainly from sugar cane and sugar beets.\nSo in all technicality the answer would be E. no of the above.
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the last guy to answer was correct.  alcohol and water create what is called an azeotropic mixture after you get to 95% alcohol and 5% water.  you can do something like add trace amounts of benzene to the mix and that will make it so you can have a higher alcohol percentages, but I wouldn't recommend drinking that (I only assume that because you are using proof as the unit of measurement).  anyway, you can distill your alcohol to 190 proof but not 200 without introducing something else.
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Types of distillation include simple distillation (described here), fractional distillation (different volatile 'fractions' are collected as they are produced), and destructive distillation (usually, a material is heated so that it decomposes into compounds for collection
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A mixture is a physical combination of two or more pure substances in relative amounts. It is called an impure substance when it contains a substance that is much greater than the amount of other substances in a mixture. \n\nHope this helps,\nUltimeaciax
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blueb_24' s answer to the first part of you question is great. \n\nMechanical mixtures are very simple mixtures that can be separated mechanically (soap is definitely not one). Some mechanical mixtures found in everyday life: \n- M&M's (various colours)\n- Mixed vegies\n- Bag of marbles\n- Box of bolts and nuts\n\nSolutions are more complex and can only be seperated by means of their physical properties, such as boiling point. Some everyday solutions include:\n- Coffee\n- Detergent\n- Salt water\n- Vinager\n\n4.a  Solid solutions: \n- Sand - suspension mixture of solid particles\n- Muddy water - solid particles suspended in water\n- Smoke - solid mixed in gas\n\nb) a liquid solution that does not contain water:\n- Motor oil - a mixture of heavy hydrocarbons\n- Vegetable oil - mixture of plant oils\n\nc) a solution of gases\n- Air - air is a mixture of many gases\n- LP gas (liquid petroleum gas)- mixture containing mainly propane or butane (depending on application)
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A substance has its own unique set of properties which are different from other substances.  A mixture is a combination of different substances that keep their own properties when mixed.  Mixtures do not have their own unique set of properties.
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LIQUID-VAPOR EQUILIBRIUM IN BINARY SYSTEMS\nApparatus\nBoiling apparatus with heating mantle and variac (S), 1/100o thermometer (S),\nrefractometer (L), glass beads or boiling chips (S), weighing bottles (D), small\nstoppered vials (D), 250 ml n-hexane (S) and 250 ml absolute ethanol (S).\nOther binary systems which may be investigated are (1) cyclohexane (S)-\nethanol (S); (2) ethyl acetate (S)-ethanol (S); (3) Methanol (S)-ethyl acetate (S);\n(4) isopropanol (S)-n-hexane (S); (5) isopropanol (S)-cyclohexane (S); (6)\nisopropanol (S)-ethylacetate (S); (7) Acetone (S)-cyclohexane (S); (8) Acetone\n(S)- hexane (S); and (9) cyclohexane (S)-2-propanol (S), (10) 1 Propanol-water.\nCONSULT YOUR LAB INSTRUCTOR TO FIND OUT WHICH SYSTEM YOU\nARE TO INVESTIGATE.\nCAUTION: The ORGANIC LIQUIDS are TOXIC and FLAMMABLE! Use all\nnecessary precautions to avoid accidents!\nCAUTION: DISPOSE OF THESE ORGANIC LIQUIDS by placing in the\nWaste Containers provided. DO NOT POUR DOWN THE DRAIN!\n\nAssemble the apparatus with care; consult instructor if you are at\nall doubtful how to put the pieces together. A 3-way stopcock (shown in Figure\n2) is provided as a means of withdrawing samples of distillate and residue at the\nappropriate time. Best procedure is to withdraw distillate first, then the residue.\n\nProcedure\nClean the apparatus by rinsing with a few milliliters of pure n-hexane. Make sure\nvials are clean and DRY and have labels for marking. Add glass beads to flask\n(carefully).\nThere are three particularly important requirements in this experiment.\n• Make sure that the condensed distillate and the liquid residue samples are\ncollected under equilibrium conditions\n• Read the equilibrium temperature accurately\n• Analyze the compositions accurately\nPlace the thermometer in a position near the top and center of the three legs of\nthe first insert as seen in Figure 3. The hole in the second insert should be\nplaced pointed towards the condenser\nPlace 50 ml n-hexane in a flask. Adjust the variac (not more than 100 -110 volts)\nso that liquid boils "reversibly" (very moderate boiling with only very tiny bubbles\nformed) and so that distillate comes over at a rate which will fill the sample tube\nonce every two or three minutes.\nDraw off the first fraction (containing impurities) which comes over and discard\n(use waste container). When a constant boiling mixture is obtained, record the\nboiling point and withdraw samples from distillate and residue into marked vials.\nAdd 1 ml ethanol to the distillate in the flask, obtain equilibrium-boiling, record the\nboiling point, and again withdraw samples of distillate and residue for analysis.\nBoiling points and refractive indices of the distillate and residue are then\ndetermined after successive additions of 0.2, 0.5, 1, 2, 5 and 5 ml of ethanol. The\nrefractive indices are used to obtain the mole fractions of ethanol in these\nsolutions.\nClean the apparatus by rinsing with a few milliliters of ethanol, and repeat the\nprocess starting with 50 ml of ethanol in the flask. Now, however, boiling points\nare to be determined after successive additions of 0.5, 1, 2, 5, 15 and 20 ml of nhexane\nto the flask.\nIn order to construct a plot of refractive index versus mole percent ethanol, the\nrefractive indices are determined for the pure hexane and ethanol and for a\nseries of solutions containing accurately known weights of hexane and ethanol.\nMixtures about 5 ml in volume containing approximately 1 volume of ethanol to 1,\n3, and 6 volumes of hexane are convenient. To obtain a decent standardization\ncurve of refractive index versus mole fraction, a series of 6 to 8 solutions\ncontaining accurately known weights of n-hexane and ethanol must be prepared\nand their refractive indices measured. Only a few milliliters of each of these\nsolutions are required, so do not waste chemicals when preparing them. The\nrequired data for the vapor pressures of the organic liquids are availab