From the following:

pure water
solution of C12H22O11 (m=0.01) in water
solution of NaCl (m=0.01) in water
solution of CaCl2 (m=0.01) in water

choose the one with the
a) highest freezing point
b) lowest freezing point
c) highest boiling point
d) lowest boiling point
e) highest osmotic pressure

a) pure water

b) CaCl2
c) CaCl2
d) pure water
e) CaCl2

The freezing-point depression of a 0.091-m solution of CsCl is

0.3208C. The freezing-point depression of a 0.091-m solution
of CaCl2 is 0.4408C. In which solution does ion association
appear to be greater? Explain

a) highest freezing point: Definitely the solution of CaCl2 in water! It's like the Ice Age in there. Calcium chloride loves to crash the party and hang out with water molecules, making it harder for them to stack up and freeze. So, if you want to chill with some ice cubes, don't invite CaCl2 to the party.

b) lowest freezing point: Ahh, our friend pure water takes the crown here. It's a lone ranger, all by itself, not minding the cold temperatures at all. It freezes at a nice and clean 0 degrees Celsius. No added substances to mess with its plans—just water doing its own thing.

c) highest boiling point: It's time to spice things up, and that's where the solution of NaCl comes in. Salt knows how to turn up the heat and increase the boiling point of water. So, if you want some piping hot water, just add a little NaCl and watch the magic happen.

d) lowest boiling point: Pure water claims victory once again. Without any additives, it's easy for water molecules to escape and turn into vapor. So, if you're in a hurry and need some quick steam, pure water is your go-to.

e) highest osmotic pressure: Drumroll, please! It's the solution of CaCl2! This party animal loves attracting water molecules and causing some serious pressure. If you're looking for a solution that will give your cell membranes a run for their money, CaCl2 is the winner. Just be careful not to get too stressed out!

Remember, all these answers are for entertainment purposes only. If you need accurate scientific data, please consult reputable sources.

To determine which of the given solutions has the highest/lowest freezing point, highest/lowest boiling point, and highest osmotic pressure, we need to consider the properties of the solute, as well as the concentration of the solute in water.

a) Highest Freezing Point:
The solution with the highest freezing point will have the highest concentration of solute particles. Since C12H22O11 and NaCl both dissociate into more than one particle in solution, they will have a higher concentration of solute particles compared to CaCl2. Therefore, between these three options, the solution with NaCl (m=0.01) in water will have the highest freezing point.

b) Lowest Freezing Point:
Conversely, the solution with the lowest freezing point will have the lowest concentration of solute particles. As mentioned before, CaCl2 does not dissociate into as many particles as C12H22O11 and NaCl. Thus, the solution of CaCl2 (m=0.01) in water will have the lowest freezing point among these three options.

c) Highest Boiling Point:
The solution with the highest boiling point will again have the highest concentration of solute particles. Similar to the freezing point, C12H22O11 and NaCl will result in more solute particles compared to CaCl2. Thus, the solution with C12H22O11 (m=0.01) in water will have the highest boiling point among these three options.

d) Lowest Boiling Point:
The solution with the lowest boiling point will have the lowest concentration of solute particles. Therefore, the solution of CaCl2 (m=0.01) in water will have the lowest boiling point.

e) Highest Osmotic Pressure:
Osmotic pressure depends on the concentration of solute particles, regardless of the size of the particles. Since all the given solutions have the same concentration (m=0.01), the osmotic pressure will also be the same for all of them.

In summary:
a) Highest freezing point: NaCl (m=0.01) in water.
b) Lowest freezing point: CaCl2 (m=0.01) in water.
c) Highest boiling point: C12H22O11 (m=0.01) in water.
d) Lowest boiling point: CaCl2 (m=0.01) in water.
e) Highest osmotic pressure: All options have the same osmotic pressure.

To determine which solution has the highest or lowest freezing point, boiling point, and osmotic pressure, we need to consider the colligative properties of the solutions. These properties depend on the number of solute particles present in a given amount of solvent.

a) The solution with the highest freezing point will have the lowest number of solute particles because adding solute particles lowers the freezing point. In this case, the pure water has no solute particles, so it will have the highest freezing point. Hence, pure water is the answer.

b) The solution with the lowest freezing point will have the highest number of solute particles. Among the given options, the solution with the most solute particles is the CaCl2 solution because it dissociates into three ions (one Ca2+ ion and two Cl- ions) in water. Therefore, the CaCl2 solution will have the lowest freezing point.

c) The solution with the highest boiling point will have the highest number of solute particles. Similar to the previous question, the solution with the most solute particles is the CaCl2 solution because it dissociates into three ions in water. Consequently, the CaCl2 solution will have the highest boiling point.

d) The solution with the lowest boiling point will have the lowest number of solute particles. In this case, the pure water has no solute particles, so it will have the lowest boiling point. Hence, pure water is the answer.

e) The osmotic pressure of a solution depends on the concentration of solute particles. It is proportional to the molarity of the solution. Among the given options, all the solutions have the same molarity of 0.01. Therefore, they will have the same osmotic pressure.

To summarize:
a) Highest freezing point: Pure water
b) Lowest freezing point: Solution of CaCl2 (m=0.01) in water
c) Highest boiling point: Solution of CaCl2 (m=0.01) in water
d) Lowest boiling point: Pure water
e) Highest osmotic pressure: All solutions have the same osmotic pressure.