Salt retards and inhibats the formation of ice crystals within water that is to be frozen.Salt is heavier.?
89574
The chemical reaction from adding\nsalt lowers the temperature in which water freezes.\n\nThat is why they throw in onto the roads in areas of winter freezing.
75493
Salt lowers the freezing point of water, making the salt/ice combination colder than ice alone.  This makes the ice cream freezing process faster.
163597
By "salt," I'm assuming you are talking about rock salt. It lowers the necessary temperature for which the ice cream will freeze, allowing the ice cream to congeal (come together). This provides the texture that we all have come to know and love. People also use rock salt on snow to melt it. The lowering the freezing point of the water combined with the temperature of the snow remaining the same, causes the snow to melt.
323097
Ice has a lower density than water. When water freezes, the way in which the molecules rearrange to make a solid means that they are slightly further apart than in liquid water. Since density = mass/volume, and in ice there is slightly less mass in the same volume, ice is less dense.\n\nTherefore, because of Archimedes' buoyancy principle (the upward force on an object in liquid is equal to the mass of substance *displaced* by the object), ice floats. The ice displaces a volume of water equal to the volume of ice, but that volume of water has more mass than the same volume of ice, so the upward force is greater than the mass of ice. So the ice floats.
617322
Althouigh I am sure you mean Sodium Chloride when you say "Salt", just to be perfectly clear....there are multiple types of "salt".\nA salt is an ionic compound made up of a matal cation and a non-metal anion. Sodium Chloride ("table salt") is an example of a salt, so is Potassium Chloride and Ammonium Nitrate.\n\nWhen you dissolve a salt in water, the freezing point of the solution is lowered.  Likewise, when dissolving a salt, the boiling point of the solution is raised.\n\nBut you asked about a temperature change.\nWhen dissolving some salts, the dissolving process is endothermic...meaning that it requires enegry input to proceed.  When a endothermic process occurs, the temperature of the surroundings (this case, the water) drops.\nThere are also salts which give off energy when they are dissolved in water.  Processes which give off excess energy are called exothermic and can raise the temperature of the surroundings.\nThere are also a few (not too many) "ideal" salts which neither take in or give off energy when they dissolve.\n\nWhen the salt dissolves, if the "product" (the aqueous salt) has a lower enthalpy than the undissolved salt, the solution is said to be exothermic.  If the enthalpy increases, the solution is said to be endothermic.\n\nSalts like Potassium Chloride, Ammonium Nitrate, and several others (probably NaCl too, which you refered to) are endothermic when dissolved in water, and thus, when dissolved cause the temperature of the solution to decrease slighty.\n\nSalts like Sodium or Potassium Hydroxide are great examples of salts which are exothermic (give off energy) when they are dissolved in water.  When dissolving these salts in water, a notible increase in temperature can be observed.
663824
it lowers the freezing point of water, make it more dense, so it has to e colder for water to freeze
1154777
When any salt particularly NaCl is added to the ice, it lowers down the temperature. The FREE ENERGY of the ice is interfered by the energy due to the ions (Na+ and Cl-) of the salt added to it. The movement of water molecule is restricted to some extent in the ice in the presence of salts. The energy saved due to restriction of movement of water molecule is being utilised by the ice to remain at still lower termperature aganist the surrounding temperature. Thus addition of salt to ice reduces the ice temperature.
90401
The higher the salinity the more resistant something is to a cold temperature change. Meaning that it takes it longer to freeze. Frozen things are more dense, so something that takes longer to freeze is less dense.
68685
water with salt bcoz water bcoms lighter wen alt dissolves in it ans hence its density decreases allowing it to evaporate easily
587656
So anti-freeze and salt causes a freezing point depression in the water which means as you add solvent such as salt the freezing point is lowered (hence when you add salt to your windshield the ice melts).  There is a simple mathematic equation that will relate the change of Temp freezing to the amout of solvent added.  (ΔTf = Kfcm).  Kf is the freezing point constant of the solvent and cm is the molal concentration of the solvent. So as you can see from the equation the ΔTf will be greater as you increase cm so the effects of adding a solvent will depend on how much solvent you add.  \n\nSo a simple experiment would be to add increasing amounts of salt and antifreeze to constant volumes of water and determine the freezing temperatures of each one.  You should also want to calculate the molal concentration of each one and try to determine before hand what the freezing points should be (hypothesis).
284203
Ice lowers the melting point of water, so it causes the ice to turn to liquid water and break up.  If it's *really* cold, this doesn't help.
379604
Rock salt and table salt ar two different ionic compounds.  Roack salt, calcium chloride, contains 3 ions: one calcium and 2 chloride ions.  Table salt has only 2 ions: one sodium and one chloride.\nSo who cares?  Well, the more ions (rock salt!) that are added to the ice (to make ice cream), the lower the freezing point of the ice will be.  Rock salt (3 ions) make the ice colder than the table salt (2 ions).  This is the only way the fatty moleculse of the cream can freeze into ice cream.  With table salt the ice just isn't cold enough.  The size of the salt crystals is not relevant.
1096429
Ice requires a crystalline lattice structure. The salt ions (Na+ and Cl-) physically interfere with the formation of that lattice structure by standing in the way of water molecules. A lower temperature is therefore necessary to form ice and so water that contains ionic salt can drop to lower temperatures before forming ice. The same general effect applies to boiling water. Because the salt prevents molecules from escaping into the atmosphere as gas, the boiling point is raised.\n\nNote: I assume you meant 0 degrees Celsius. The Fahrenheit scale is somewhat different, since water freezes at 32 degrees Fahrenheit. But don't let these numbers cause you to believe something different is going on in the salt/water/ice mixture. The Celsius scale is set such that water freezes at 0 degrees (absent salt). This doesn't mean that at 0 Celsius and below there is no temperature or energy. Just the same, below 0 degrees Fahrenheit compounds still have energy and temperature. Scientists tend to use another scale which more accurately depicts true temperature, which is the Kelvin scale. In the Kelvin scale, absolute zero- the temperature at which all molecules and atoms stop moving- is really 0. But 0 Kelvin is much lower than either 0 Celsius or 0 Fahrenheit. To convert from Celsius to Kelvin, just add 273 degrees (or subtract 273 from Kelvin to Celsius). So 0 Celsius is actually 273 degrees Kelvin.  \n\nIn any case, if you were looking for an answer that has to do with the chemical properties of the salt/ice/water mixture, and why, for example, salt tends to lower the freezing point (or raises the boiling point), my first answer is right.  Any solute you add to a solvent will change the colligative properties of the solvent.  It interferes with the organization of water molecules such that they have a harder time aligning into a crystalline ice pattern, and therefore a lower temperature is required for ice to form. Note also that whenever you have an ice/water mixture, the entire mixture maintains the same temperature until all of the water has turned to ice. That is, in pure water that contains ice, the water will stay at 0 degrees Celsius until all the water has turned to ice, and then the ice will gradually drop in temperature. The salt just lowers that freezing point, but the same applies, just that the salt/water/ice mixture remains at that lower freezing point until all water as frozen, then it drops further in temperature.
562622
Let a chemistry student explain it.  \nThis here is something called a colligative property. A colligative property is a property that is affected by how many particles are involved.  \n\nNow, it just so happens that freezing point lowering is a colligative property.  That means that if you have stuff floating around in water, it needs to be colder in order for that water to freeze.  We put salt on icy sidewalks because when salt particles are in the water, the temperature has to be a lot lower in order for the ice to stay frozen.  That means that the ice is a lot less likely to stay frozen, so it melts.  \nI hope I helped!
858544
Because water expands when it freezes..\nTherefore ice is of larger volume than the water it originated from\ntherefore it is less dense..
348819
fresh water\nany substance in water increases boiling temp\nthe particles of this substance "get in the way" of the water's gas molecules and makes it "more difficult" for the water to evaporate.\nso really, the myth that adding salt to water when making pasta makes it boil faster it enitrely wrong\nit actually makes it longer, but not by much time (a few extra mins)\nsimilarly, This is why we salt our roads\n the salt dissolves the ice and doesn't let it freeze again because it decreases freezing pt by, again, "getting in the way" of the water forming its 6-sided ring (solid state)\na lower temp (slow down the molucles EVEN MORE) is needed to freeze it
469334
Because salt consists of sodium and chloride ions, and as You know, ions have charge, so You know there will be an interaction(attraction) between water molecules and the ions. You might also know that in ice, water molecules are in a definite distance from each other, they are in a crystal structure. Well, because of the interaction, that structure "opens up", and the water molecules get closer to each other, so the structure move from solid to liquid, as the interaction between them becomes weaker.\nI hope i was understandable. \nSalt lowers the boiling point and increases the freezing point of water. You can see it Yourself by putting salt into water, it'll boil sooner than without it.