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)Water

b)CaCl2
c)CaCl2
d)Water
e)CaCl2

a)CaCl2

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

To determine the freezing point, boiling point, and osmotic pressure, you need to consider the concentration of solute particles in the solution.

a) Highest Freezing Point:
The solution with the highest freezing point will have the highest concentration of solute particles. In this case, the solution of CaCl2 (m=0.01) in water would have the highest freezing point. This is because CaCl2 dissociates into three particles (1 Ca2+ ion and 2 Cl- ions) in water, compared to the other solutions which dissociate into one or two particles.

b) Lowest Freezing Point:
The solution with the lowest freezing point will have the lowest concentration of solute particles. In this case, pure water would have the lowest freezing point since it does not contain any solute particles.

c) Highest Boiling Point:
The solution with the highest boiling point will have the highest concentration of solute particles. In this case, the solution of CaCl2 (m=0.01) in water would also have the highest boiling point. Just like in the freezing point case, CaCl2 dissociates into three particles, increasing the concentration of solute particles.

d) Lowest Boiling Point:
The solution with the lowest boiling point will have the lowest concentration of solute particles. In this case, pure water would have the lowest boiling point since it does not contain any solute particles.

e) Highest Osmotic Pressure:
Osmotic pressure depends on the concentration of solute particles in a solution. The solution with the highest osmotic pressure will have the highest concentration of solute particles. In this case, the solution of NaCl (m=0.01) in water would have the highest osmotic pressure. This is because NaCl dissociates into two particles (1 Na+ ion and 1 Cl- ion) in water, compared to the other solutions which dissociate into one or three particles.

To summarize:
a) Highest Freezing Point: Solution of CaCl2 (m=0.01) in water
b) Lowest Freezing Point: Pure water
c) Highest Boiling Point: Solution of CaCl2 (m=0.01) in water
d) Lowest Boiling Point: Pure water
e) Highest Osmotic Pressure: Solution of NaCl (m=0.01) in water.

To determine the answers to these questions, we need to compare the properties of the given substances.

a) To find the solution with the highest freezing point, we need to consider the colligative property of freezing point depression. The freezing point of a solution is lower than that of the pure solvent due to the presence of solute particles. The greater the number of solute particles, the greater the depression of the freezing point.

In this case, we have a solution of C12H22O11 (m=0.01) in water, which means we have 0.01 moles of C12H22O11 in 1 kg of water. C12H22O11 is a larger molecule than NaCl or CaCl2, so it will have a higher number of solute particles per mole. Therefore, the solution of C12H22O11 will have the highest freezing point among the given options.

b) Conversely, the solution with the lowest freezing point will have the fewest solute particles. In this case, pure water contains no solute particles and will have the lowest freezing point.

c) To find the solution with the highest boiling point, we need to consider the colligative property of boiling point elevation. The boiling point of a solution is higher than that of the pure solvent due to the presence of solute particles. Again, the greater the number of solute particles, the greater the elevation of the boiling point.

Among the given options, the solution with CaCl2 (m=0.01) in water will have the highest boiling point since CaCl2 dissociates into three ions (Ca2+ and two Cl-) per formula unit, providing the highest number of solute particles.

d) Conversely, the solution with the lowest boiling point will have the fewest solute particles. In this case, pure water contains no solute particles and will have the lowest boiling point.

e) The osmotic pressure of a solution is directly proportional to the concentration of solute particles. In this case, since all solutions have the same concentration (m=0.01), the osmotic pressure will be the same for all the given options.

To summarize:
a) Solution of C12H22O11 (m=0.01) in water has the highest freezing point.
b) Pure water has the lowest freezing point.
c) Solution of CaCl2 (m=0.01) in water has the highest boiling point.
d) Pure water has the lowest boiling point.
e) All the solutions have the same osmotic pressure.