how would the freezing and boiling points of distilled water and seawatercompare?
364087
sea water = S\ndistilled water = D\nfreezin point = fp\nboiling point = bp\n\nS fp < D fp ~ 0 deg C < 100 deg C ~ D bp < S bp\n\nRemember freezing point depression and boiling point elevation.  If you have problems remember which drops just remember that they salt the roads in winter to help the roads not freeze.
658781
Freezing and Boiling points of Water are:\n\n 0 and 100 degrees Celsius\n32 and 212 degrees Fahrenheit\n\nFrom the equation of a straight line,\n\nF = mC + A\n\nwhere m is the gradient and A is a constant\n\nm = (212-32)/(100-0) = 1.8\n\nF = 1.8C + A\n\nwhen x=0, F=32\n\n32 = 1.8(0) + A\n\nA = 32\n\nTherefore the final equation is:\n\nF = 1.8C + 32\n\nor\n\nC = (F - 32)/1.8
488884
There are two different "environmental conditions" which would affect the water: very low pressure and very low temperature.\nThe first thing to happen is that the water would "boil" (that is start to turn into a vapor).  This would be described as a "vacuum distillation."  This process (which removes heat from the liquid water), combined with the already low temperature would remove enough heat for the water to freeze.\nIf the container was allowed to remain exposed, the solid water would slowly continue to "sublime" (turn into a vapor under reduced pressure) until some sort of equilibrium was reached.\nNo.  I do not believe that this experiment has been tried, or if tried, the results released to the general public.
432890
Pure =32 degrees F\nSalt = depends on the salt concentration, ocean water is -40 degrees F
30770
Excellent question.  Food for thought for both of us.  Let's see- changing the pH of water could allow for greater or less solubility of minerals.  With more minerals in solution, the rate of evaporation increases while the boiling/freezing point lowers, as intermolecular attraction is decreased.  The opposite would then be true with less minerals in solution.
91256
28.8 DEGREES FARENHEIT. IT'S NEAR THE BOTTOM OF MY ANSWER.\n\nYou must know the salinity to answer accurately. Ocean water has different amounts of salt dissolved in it in different locations and currents. If you know the salinity you can use this automatic calculator to determine the freezing point. http://www.csgnetwork.com/h2ofreezecalc.html\n\nIf you don't know that, a good rule of thumb is 28.8 degrees farenheit.
777060
Tap water. Dissolved salt raises the boiling point, so salt water  takes longer to boil.
484846
1. The freezing point of water and gasoline can be compared in terms of their intermolecular forces. The stronger the intermolecular forces of a substance, the higher the freezing point (as more energy is required to overcome those forces). Water has a low molecular weight and so has weak dispersion forces. Gasoline consists of long chained hydrocarbons with high molecular weights and so would have much stronger dispersion forces than water. Even though water has strong hydrogen bonding, the overall intermolecular forces in gasoline would be much stronger and so it would have a lower freezing point, that is, less than 0 degrees celsius. \n\n2. Freezing and melting are opposite processes. So if water freezes at 0 degrees celsius, then it must melt at 0 degrees celsius.
684151
The freezing point of pure water is 0°C, but that melting point can be lowered by the adding any solvent such as a salt. Depending on the amount of salt the freezing temperature of a saline solution can range from below 0°C to -21.1°C. The frozen solution is a mixture of separate NaCl·2H2O crystals and ice crystals, not a homogeneous mixture of salt and water. This heterogeneous mixture is called a eutectic mixture. \nThe use of ordinary salt on sidewalks is effective because it requires a colder temperature to freeze water and it is a cheaper alternative to other solvents or methods of ice removal.
53261
salt's chemical composition breaks down bonds at an intermolecular level and lowers the freezing point of water...which is normally 32 degrees Fahrenheit. When the freezing point goes down...it melts
49074
It causes the water to boil at a higher temperature.\n\nAs soon as any of the salt dissolves in the water, the boiling point of the water will begin to rise -- by about one half degree Celsius for every 58 grams of salt\ndissolved per kilogram of water. In fact, any non-volatile soluble substance will raise the boiling point of water. That is why antifreeze(ethylene glycol)provides boiling protection in winter as it simultaneously provides freezing\nprotection in the summer.\n\nhere's a good site with more info:\nhttp://www.freesciencefairproject.com/projects/effect_salt_boiling_water.html
199763
What context are you describing (or is that what you are asking)?\n\nHot water will freeze slower than cold water.  In order to freeze the water temperature must be dropped to freezing temperature, and the farther away you are from freezing, the longer it will take to 'bleed' the temperature away by any known method.\n\nI am not aware of any condition where hot water will freeze faster than cold water, assuming the water in both situations is exactly the same (i.e., not water made of different material, or with another chemical in aqueous solution), so if someone can give this example, I would be very curious to see it.\n\nPerhaps there is a situation where you can heat a liquid to convert it into gas, and then from gas directly to solid (frost formation is an example of this).  I am not sure, but this might be one approach to try getting water to go to a solid state faster when the water temperature is initially higher.  The key is you are bypassing the liquid state.\n\nAddendum:\nActually now that I think about it, I have an aswer.  If you have supercooled water, i.e. water that is below freezing, it could stay in that metastable state indefintely.  So here is a case where hot water would cool faster.  The hot water will cool down to freezing and will freeze, while the supercooled water may never turn solid.\n\nAddendum:\nWow, this link that someone below posted is interesting:\nhttp://math.ucr.edu/home/baez/physics/General/hot_water.html\n\nI was going to say that it is impossible, since water at a higher temperature would have to pass through all lower temperatures, but this article pretty much explains it (in that, well, we just don't know).  It has been observed, but there is no explanation that can be agreed upon.\n\nTo be completely pedantic, I note that most of the explanations point to what I would consider to be "experimenter's errors" in the set up of the experiments (if more dissolved gas is in hotter water, than the two water mixtures are certainly not the same, so this is an invalid experiment... if there is a 'hot top', then the experimenter did not start with a homogenious mixture, and that has to be mentioned in the experiment... if the surrounding environment is not the same, then the ambient conditions are changing which not an assumption in a traditional experiment, but rather a source of error... if evaporation is allowed than some quantifiable mass of the water is not turning solid, so this again is invalid).  The only explantation that doesn't result from a poorly set up experiment is supercooling.
432980
Look in the index of an introductory chemistry text for "colligative properties", "freezing point depression", or "boiling point elevation".  Simply put, the water molecules prefer to orient themselves around the sodium and chloride ions instead of each other.  This lowers the freezing point (more energy has to be removed from the system to slow down the molecules enough to be in the solid state.  This effect also accounts for the boiling point elevation (salty water boils at a higher temp) and for the same reason.
748490
If you are asking how to separate a mixture of water and salt, then you need to distill the water.  Distillation separates materials by adding increasing amounts heat in order to boil off the materials at theri respective boiling points.  The material that boil at a lower temperature would be removed first.  As you increase the tempreature, higher boiling temperature materials are separated.\n\nSince the water boils and the salt does not, all you need to do is heat the mixture up until it boils.  The water will vaporize and can be captured in another container, leaving the salt behind in the original container.
908737
compared to what?\nIt would be buoyant compared to sea water, which is heavier due to the high number of minerals dissolved in the water.\nIt would not be buoyant compared to distilled water, which would be lighter because it has no minerals dissolved in it.
838271
What about boiling points?  Or regular melting points?
316108
It depends on the purity of the water and the pressure of the system.  Pure water in normal atmospheric pressure boils at 212 F.