The Formula used to find the freezing point is "Delta T=Km"
"Delta T" is the change of temperature and what your are looking for.
"K" is the freezing constant of the solvent
"m" is the molality which is mols of solute over kg of solvent.
Based on the formula if you have 0.10m of each solvent you would think that it is the same. However, you also need to consider the number of mols of substance once the salt has disolved. NaCl will disassociate and then you will have more mols to account for in your molality calculation. This will give salt the lower freezing point.
If all of the "m"'s immediately preceded by a number in the question are intended to mean "molar" and 10 molar glucose actually exists, then the freezing points from lowest to highest are 10 molar glucose, 0.20 molar Na2SO4, 0.20 molar NaCl, and 0.10 molar BaCl2. Each mole of Na2SO4 provides 3 moles of ions after dissociation, each mole of NaCl provides 2 moles of ions after dissociation, and each mole of BaCl2 provides 3 moles of ions after dissociation. (Glucose does not ionize.) 10 > (0.20 X 3) > (0.20 X 2) > (0.10 X 3), and the largest concentration of dissolved units produces the greatest freezing point depression.
The glucose will C6H12O6 it has more particles when dissolved. Colligative properties depends only on the number of particles not the nature. Solutions will have a lower vapor pressure, higher boiling points and lower freezing points
0.5 m Na2CO3
1 m NaCI
3 m glycerol
2 m NH4NO3
1.5 m Ca(NO3)2
NaCl
Because NaCl --> Na+ + Cl-
0.1 0.1
0.1 + 0.1 = 0.2
NaCl forms 0.2m solute, therefore it has a lower F.P
it is increased with the increasing density
The freezing point is lowered.
you can shrink the spaces within the molecules of liquid by increasing the temperature (freezing it ) or adding pressure.
The problem with this question is that you did not provide any solutions, as stated, to calculate the freezing point for.
Increasing the amount of water
it is increased with the increasing density
When a material is melting, the temperature is likely to be increasing. That or the temperature is just above the material's melting/freezing point.
As water freezes salt is released increasing the percentage of salt in the ocean water, the higher the percentage of salt the lower the freezing temperature of the water. The cycle of water freezing -> salt being released -> more water freezing reaches equilibrium at witch point the temperature necessary to freeze more water is lower then the air temperature.
since freezing elastic object decreases its elastic limits, increasing temperature would increase elastic limits.
temperature below freezing point of water.
The freezing point is lowered.
The freezing point is lowered.
you can shrink the spaces within the molecules of liquid by increasing the temperature (freezing it ) or adding pressure.
The problem with this question is that you did not provide any solutions, as stated, to calculate the freezing point for.
It is the same thing. A melting point or freezing point is when a "material's" temperature stays the same. Then you can decide whether you want to freeze it or melt it by increasing or lowering the temperature.------Thats how my science teacher tought us.
Increasing the amount of water
Yes, due to higher no of solute particles the total kinetic energy will be higher, its proof is that such solutions freeze at lower temperature than a dilute solution (depression of freezing point).