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From the following:

pure water

solution of C6 H12 O6 (x = 0.01) in water

solution of NaCl (x = 0.01) in water

solution of CaCl2 (x = 0.01) in water

Choose the one with the following:

a) highest freezing point

b) lowest freezing point

c) highest boiling point

d) lowest boiling point

e) highest osmotic pressure

Short Answer

Expert verified
  1. Highest freezing point = pure water
  2. Lowest freezing point = CaCl2
  3. Highest boiling point = CaCl2
  4. Lowest boiling point = pure water
  5. Highest osmotic pressure = pure water.

Step by step solution

01

Step 1:

The colligative properties of a solution depend on the concentration of

Solute particles

02

Step 2:

The concentration of solutes for every solution is given as 0.01

So the colligative properties will depend on the van’t Hoff factor

Higher the van’t Hoff factor greater the elevation in boiling point and

Depression in freezing point whereas higher the molar mass of the solute

lower the osmotic pressure.

03

Step 3:

Highest van’ Hoff factor is of CaCl2 so highest boiling point is of CaCl2

The lowestvan’t Hoff factor is of pure water so the lowest boiling point is of pure

water.

04

Step 4:

The highest van’ Hoff factor is of CaCl2 so highest depression in freezing point

is of CaCl2 so the lowest freezing point is ofCaCl2

The lowest van’t Hoff factor is of pure water so the lowest depression in

freezing point is of pure water so the highest freezing point is of pure water,

05

Step 5:

When the concentration of solute particles isthe same then the osmotic

pressure is inversely proportional to the molar mass. lower the molar mass

, higher the osmotic pressure. Pure water has the lowest molar mass so it will

have the highest osmotic pressure.

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