00:02
Hi there.
00:02
In this question, we want to know which of these aqueous solutions, so that means water is the solvent, would have the highest freezing point.
00:18
Well, we know that freezing point depression is a colligative property.
00:23
The more solute particles there are in a solution, the more it lowers the freezing point.
00:28
So if we're looking for the highest freezing point, we are looking for the the one that is lowered the least.
00:41
Or in other words, the one with the smallest change in freezing temperature.
00:51
Yes, that's the one that would lower it the least.
00:53
Well, to answer this question then, we need the equation for how the change in freezing temperature is calculated.
01:01
It's calculated by taking the freezing point constant for the solvent, in this case water, multiplying times the molality of the solution and then multiplying times i, which is the vantahoff factor.
01:22
The vantahoff factor is the number of particles the solute produces when it dissolves.
01:40
So ionic substances, for example, are going to dissociate or break into ions.
01:45
Counting up those ions would give us i, the vantahoff factor.
01:49
If it's a molecular substance, molecular substances do not break apart in water.
01:53
So for example, one molecule of sugar would just give us one particle.
01:58
It's not going to break apart.
02:00
Alright, so let's figure out for each of these.
02:03
For letter a, we have a 1 .0 molar solution of sodium nitrate.
02:10
So sodium nitrate is nano3.
02:13
When it's placed into water, we get a sodium ion and we get a nitrate ion...