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Freezing Point Depression
- Thread starter s2thindi
- Start date
- Joined
- Oct 16, 2007
- Messages
- 4,197
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For simplicity, I will ignore the charges on the ions
Before mixing:
2 Ca
4 Cl
------
6 ions total (i = 6)
Immediately after mixed:
2 Ca
4 Cl
3 Ag
3 NO2
------
12 ions total (i = 12)
The Ag and Cl react to become insoluable. Only soluable material affects bp elevation and mp depression. So we ignore all the AgCl in the solution. In other words: i = 0 for AgCl.
After 3 Ag and 3 Cl are taken out:
2 Ca
1 Cl
3 NO2
-------
6 ions total
The number of ions is the same before and after. So nothing changes.
Hope that helps.
Before mixing:
2 Ca
4 Cl
------
6 ions total (i = 6)
Immediately after mixed:
2 Ca
4 Cl
3 Ag
3 NO2
------
12 ions total (i = 12)
The Ag and Cl react to become insoluable. Only soluable material affects bp elevation and mp depression. So we ignore all the AgCl in the solution. In other words: i = 0 for AgCl.
After 3 Ag and 3 Cl are taken out:
2 Ca
1 Cl
3 NO2
-------
6 ions total
The number of ions is the same before and after. So nothing changes.
Hope that helps.
- Joined
- Oct 16, 2007
- Messages
- 4,197
- Reaction score
- 36
Sort of. Association is when solutes come together so that there are less particles in solution. Acetic acid in benzene, for instance, tend to clump together because it is polar and the solvent is nonpolar.
But that's not what is exactly going on here. The salt is precipitating out and is not dissolved at all. Remember, colligative properties only apply to dissolved particles.
In a sense, you are right. They are "clumping up" so much that their van hoff factor becomes 0. So if this way makes sense to you, than go for it.
But that's not what is exactly going on here. The salt is precipitating out and is not dissolved at all. Remember, colligative properties only apply to dissolved particles.
In a sense, you are right. They are "clumping up" so much that their van hoff factor becomes 0. So if this way makes sense to you, than go for it.
