what is the effect of a chemical identity of the solute on the slope of the concentration vs. freezing point?
114166
theoretically the identity has nothing to do with what you're talking about. that's the definition of a colligative property.\nin reality it might make a little difference but you're probably safe to ignore it.
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.
887709
the more solute...the higher the solute concentration which lowers the water potential (concentration of water)
558840
When you dissolve a salt in water, the freezing point of the resulting solution is lower than the freezing point of the pure solvent (water).\nThe amount of the freezing point depressure depends on two factors, the concentration of the solute (salt) and the freezing point depression constant of the solvent.\n\nThe formula to calculate the freezing point depression in therms of the change in the original freezing point (delta T) is,\n(delta T) = k_f * m\nwhere k_f is the freezing point depression constant and m is the concentration of the solute in terms of molarity.\n\nIt is mathmatically possible for the concentration of the solute to be so greate at to create a change in the freezing point of water of more than 32 degrees F.\n\nThe freezing point depression constant of water is -1.86 degrees C per molality.  So mathmatically, if one had a solute concentration of about 9.57 molality or greater, the freezing point of water would be below 0 degree F.
239534
because the impurities have low melting points under the ice , u got a compound not a pure material
617450
Some molecules absorb visible light, e.g. due to conjugation and pi to pi antibonding transitions, with the highest intensity at a particular wavelength.  One can prepare standard solutions, with accurately devised known concentrations, the measured intensities of these solutions are correlated with these standard solutions, covering a particular dynamic range.  Assuming Beer's Law, the plot will resemble a linear curve, and a least fit regression line and its equation can be obtained; also by correcting for the blank if this is has not bee accounted for by the spectrometer.  The unknown pure solution, or a matrix derived alternative method if the solution is not pure that there are significant impurities in the unknown solution, will also be measured at this wavelength and it's intensity, often the y value, will be plugged into the regression equation to estimate the concentration.
199280
Salt causes the freezing point of water (and any other solvent for that matter) to be lowered. Thus, a salt solution freezes at a lower temperature than pure water. This phenomenon is called "freezing point depression." The extent to which the temperature is lowered is a function of the molality (moles of solute per kilogram of solution). That means that the more salt you add, the lower will be the freezing point.
959876
a) the hydration energy is greater because the temp decreases. When you go from a low potential energy substance to a high potential energy substance the temp of solution will decrease.\n\nb) the solubilty will increase because energy is on the reactant side of the equation. (the reaction is endothermic and requires energy to occur)
721022
Well, I do not know that syllabus.  You will need to sift useful answers.\n\nI would use:\n\ndifferent solubility in solvents\ndifferent boiling points\nrecrystallise one out of a mixed solution\n\nYou might be at too junior a level to know about ion exchange resins, and other chromatography techniques.
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!
613215
Simply put, the salt lowers the freezing point of water.\n\nHow does it do this?  From kinetic molecular theory, the temperature of an object is proportional to the random motion of the molecules of the object.  As water cools down the molecules move slower and stick closer together until the intermolecular forces are stong enough to lock the molecules into a crystal structure (overcome random motion) and water freezes.  The salt lowers these intermolecular forces by interacting with the water molecules: there is some salt-water interaction and thus less water-water interaction.  Thus, a lower temperature is required to lock in the crystal structure (lower melting point) and the ice melts.\n\nThis works to about -30 or -40 C IIRC.
131090
In general, a colligative property is a property that only relies on the number of molecules present, not the type of molecule. Basically, it's another way of saying that the property relies on concentration rather than composition. The formula for how much a certain solute will change the freezing point is:\n\nChange in temperature = -kf x m\n\nWhere kf = molal freezing point constant for the solvent\n           m = molality of solution (mol solute/kg solvent)\n\nAs you can see, the equation depends on the concentration of the solution, m, not the actual type of molecules that make up the concentration.
423379
let me see if i can at least help you with part of your problem, solubility in chemistry is simple, basically the equation will always be:\n\n[Solubility equalibrium constant] = concentration of product divided by concentration of reagents (concentration of each reagents multiplying by each other).\n\nthe easiest way to understand this is to simplify things for you so as you know, a chemical equation always go like this:\n\nreagents <==> products\n\nJust know this from the above, the dynamic here is that when you have an excess of either the reagents or the product, the balance of the equation tend to shift in the opposite direction (ie excess concentration of product will cause more reagents to form and vice versa), in a chemical equation such as the one from above, the reaction can actually go either way, products or reagents can form.  What really matters is the equalibrium constant that I talked about in the first equation. This constant represent the concentration of the products and the reagents when they are in equailibrium or when they are balance, meaning that the rate at which products or reagent form stays the same and there are no change in the concentration of either the products or the reagents so the whole thing is static at the point.   Think about this, more concentration of products wouldn't form unless you have extra reagents to spare that can shift the balance.  When something is saturated it means that it can longer dissolve in a solvent (let's use water to simplify the explanation)so it just accumulates at the bottom, water molecules can only separate so many ions from each other (the reagents) and preventing them from forming a solid product since water itself has limited molecules (if you mix enough table salt in a glass of water, it'll get to the point where it'll accumulate at the bottom and won't dissolve).  If remember correctly, in a chemical equation, when there's different amount of reagents needed to form the product, there's a slight modification to the equation I gave you, for example:\n\n2 CaCO3 + 4 ZnO2 <----> 3 ZnCO3 + 3 CaO2\n\nthen  [equilibrium constant] = [Cao2]^3 x [ZnCO3]^3 divided by [CaCO3]^2 x [ZnO2]^2\n\nnote that you should balance the chemical equations first, I am just giving an example.\n\nhere's a summary of how to compare numbers, if you plug given concentrations of reagents and product into the equation and the number you get is larger than the real equilibrium constant, then the concentration of products is higher than it should be and the equation will shift towards forming more reagents (in the case of the solid product, it'll dissolve) and if there's more reagents, more solid product is gonna form.  Hope that helps. Remember the Chemistry textbook is still your best reference.
240715
The answer to this problem lies in colligative properties.  The salt ice solution will have a lower freezing point because by adding the salt, the solution is going through freezing point depression, which means that the solute is spreading apart the molecules of the solvent, thus requiring a lower temperature to freeze.
905977
While it lowers the mp of water as stated earlier (a colligative property), more importantly, the dissolving process (measured by heat of solvation) is endothermic.  It takes energy to separate the ions in the salt (solute).  That energy comes from the solvent (water).\n\nTherefore, the solution cools.  (BTW, the salt goes into the cooling or refrigerant bath, not the edible product itself).\n\nIf you start with ice water(0 C), then you end up cooler than zero.  At those temps, the fatty emulsion of protein and water (aka cream) (as well as sugar and flavoring) solidifies.\n\nYum, yum and enjoy.
205901
I don't have to resources in front of me to really compute the answer, but this should give you the answer.\n\n1) you know the freezing point of water is zero degrees Celsius.\n\n2) find the moles of NiSO per kg of water (molality)\n\n3) use the following dimensional analysis (with 'X' being the previous answer): (X mol./kg)*(1.86 degree decrease/1 mole NiSO added) = Y\n\n4)Since there is 100% dissociation, the answer should be  0 - 2*Y (vant Hoff factor).\n\nThis means your answer will be a negative (below zero) number with Celcius as the temperature units
735542
This a  difficult question to answer since the solubilty of these three liquids changes with changing temperature.  Water and acetic acid and miscible at all tempertures and chloroform and acetic acid are miscible at all tempertatures.  However, water and chloroform are only partially soluble in each other and their solubilty changes with changing temperatures.  \n\nPlease also refer to the reference that I have indicated below.  It discussed a point in the ternary system diagram called the Plait Point.  It is an example of a critical point, where the composition of the two phases is equal. At this point, the relative volumes of the two phases are equal and the boundary vanishes as the system becomes homogeneous.\n\nPlease refer to this document for more answers, sorry I could not have been more help.