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Osmotic Pressure and Osmotic Potential

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Calculate the vapour pressure of an aqueous solution containning 100 g of an antifreeze, ethylene glycol ( molar mass 62 g / mol) , in 500g of water( molar mass18g/ mol) at 100^°

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Q. Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to

4

kg of water to prevent it from freezing at

- 6^{o} C

K_{f}

1.86

K kg/mol and molar mass of ethylene glycol =

62

^{- 1}

Q. The molarity of an aqueous solution of glycol is

12 M

. The density of the solution is

1.392 g/mL

. Find the mole fraction of glycol.
(Given, molar mass of glycol

= 62 g/mol

)

Q. The boiling point of pure water is

100^{\circ}

C. Calculate the boiling point of an aqueous solution containing

0.6 g

of urea (molar mass =

60 {g mol}^{- 1}

100 g

K_{b}

0.52 {K kg mol}^{- 1}

.

Q. An antifreeze mixture consists of

40

% ethylene glycol

(C_{2} H_{6} O_{2})

by weight in aqueous solution. If the density of this solution is

1.05

g/mL, what is the molar concentration?

Q. The freezing point of a solution

50 c m^{3}

of ethylene glycol in

50 g

water is found to be

{- 34}^{\circ} C

. Assuming ideal behaviour, calculate the density of ethylene glycol

(K_{f} f o r H_{2} O = 1.86 K k g m o l^{- 1}

Molar mass of Ethylene glycol = 62 g m o l^{- 1}

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