how would u design an experiment showing:which is a better solvent, alcohol or water?
109122
Second answer has some misunderstood spellings.\n\nSolvent is the substance which dissolves.\n\nSolute is the substance which is dissolved and\n\nSolution is the end mixture aof the solvent and the solute.\n\nThere is always a reference for better solubility of a solvent with that of other.\n\nYou can say A is better solvent than B because it dissolves more substances.\nIn this respect you select a number of solutes and get try to dissolve in both solvents.\n\nYou can say A is better solvent for a substance S because A dissolves more quantity of S than solvent B\nIn this respect you take equal volumes of the solvents and two equal volumes of the solute one to dissolve in each solvent. The solvent which gets more amount dissolved is better solvent for the solute than the other one.\n\nIt is just possible that A is better solvent in terms of quantity of a substance dissolved and B is better solvent for another substance \nOR A is better solvent for one substance but B is better solvent in number of of substances it can dissolve.
878769
rubbing alcohol and cotton
485319
A classic, but great visual experiment is sucking a hard boiled egg into an erlenmyer flask. It is done by using the principles of the kinetic theory of matter.\nAnother cool project might be doing something with dry ice. Find a place that you can get dry ice and do fun stuff with it, like create smoke, put bubble solution in water and then drop in dry ice to make bubbles that, when you pop, let out white smoke.\n\nAnother idea might be to do some cool colorful reactions. Make some dye molecules or something.\n\nHope one of these ideas works for you.
641728
see how much weight each surface can hold up. I know u can keep a needle afloat in a cup of water. Although the experiment would depend on what kind of paper and how damp it was.
423221
Ethane is nonpolar.  Ethanol has a polar hydroxyl group which can form hydrogen bonds with water.
67994
Narrow it to surface tension. 1. Sprinkle on wax paper and drag drops using toothpick. 2. Overfill a shotglass. 3. (my favorite)  get a flashlight , small bowl of water and an eyedropper of common rubbing alchohol.  Shine the light on the surface of the bowl of water and from about 1/2 inch, drip in the alchohol.  It will appear to boil!
500934
Combine 19 parts of solvent with 1 part solute.  Boom, 5% solution.  \n\nIf you have an already diluted substance, just figure out the ratio and try to make it 1/20.  For example, if you have a 50% solution of NaCl and water, add two parts (2*50% is 100% or 1 part) of it to 18 parts water to make a 5% NaCl and H20 solution.
429768
To perform a solution-based separation, you need a solvent in which one or some of the solutes (in the mixture to be separated) is/are highly soluble, and in which the other components are highly insoluble.\n\nA simple example might be separating an ethanol/pentane mixture by using water.  Ethanol, being polar, will readily dissolve in water; but the nonpolar pentane will not.
363827
Depends on what you do or care about.  Do you want to know how much sugar to add when making wine to reach the desired alcohol content and/or "dryness"?  Do you want to know how much acetylene and oxygen to mix when welding?  Do you want to fill a scuba diving tank?  Do you want to know how much vinegar and baking soda to add when making sponge toffee so it is neither bitter nor sour?  \n\nThese are just a few examples for people who are not scientists at all.  Zillions of reasons more.
140226
ethanol and oil\nwater and chloroform
30706
test the reactions of different substances in water. like um put in sugar and salt and then say it dissolved. And put in oil and say it freakin stayed seperate or whatever it does
4591
sugars + yeast + water = ethanol ;I wouldn't drink it though unless you know what you are doing. There is always the possibility of methanol contamination that's the reason for distillation. IF YOU DRINK IT YOU COULD GO BLIND!!!
620413
Do the experiment.  You might learn something.
106576
You'd need 4 L of dehydrated alcohol and 1 L of water in order to get a 80% solution. Getting a dry solution of ethanol would be a challenge, though, so I would expect it to be closer to 75-77% in actuality (but theoretically 80)
512002
Yup, non-polar solvents.  If acetone, alkanes, or toluene don't work, then go with petroleum ether(hist. ligroin) that dissolves alot of things.
889419
1) Decide what solvent you want to use: water or organic?\n2) Decide how much solution you want: 1L?\n3) Check the solubility of phenol in the solvent you choose. And calculate how much phenol you'll need by weight to make a saturated solution\n4) Find out the relationship between solubility and temperature.\n5) I assume you want to make a saturated phenol solution at room temperature. If the solubility increases as temperature goes higher, add a bit more phenol than needed (from the calculation above) to the solvent. \n6) Heat the flask or beaker that contains the solvent and phenol until all phenol dissolves.\n7) Let the container cool down to room temperature.\n8) If no phenol crystalizes the solution is over-saturated. You may rub the side of the flask or beaker to help phenol crystalize.\n9) You have your saturated phenol solution!!
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Physical and chemical properties\nThe hydroxyl group generally makes the alcohol molecule polar. Those groups can form hydrogen bonds to one another and to other compounds. Two opposing solubility trends in alcohols are: the tendency of the polar OH to promote solubility in water, and of the carbon chain to resist it. Thus, methanol, ethanol, and propanol are miscible in water because the hydroxyl group wins out over the short carbon chain. Butanol, with a four-carbon chain, is moderately soluble because of a balance between the two trends. Alcohols of five or more carbons (Pentanol and higher) are effectively insoluble because of the hydrocarbon chain's dominance.\n\nBecause of hydrogen bonding, alcohols tend to have higher boiling points than comparable hydrocarbons and ethers. All simple alcohols are miscible in organic solvents. This hydrogen bonding means that alcohols can be used as protic solvents.\n\nThe lone pairs of electrons on the oxygen of the hydroxyl group also makes alcohols nucleophiles.\n\nAlcohols, like water, can show either acidic or basic properties at the O-H group. With a pKa of around 16-19 they are generally slightly weaker acids than water, but they are still able to react with strong bases such as sodium hydride or reactive metals such as sodium. The salts that result are called alkoxides, with the general formula RO- M+.\n\nMeanwhile the oxygen atom has lone pairs of nonbonded electrons that render it weakly basic in the presence of strong acids such as sulfuric acid. For example, with methanol: