Chapter 2 : Solutions

Q. Heptane and octane form an ideal solution. At

373 K

, the vapour pressures of the two liquid components are

105.2 k P a

and

46.8 k P a

respectively. What will be the vapour pressure of a mixture of

26.0 g

of heptane and

35 g

of octane?

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Q. What role does the molecular interaction play in a solution of alcohol and water?

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Q. Concentrated nitric acid used in laboratory work is

68

% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is

1.504 g m L^{- 1}

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Q. Define the term solution. How many types of solutions are formed? Write briefly about each type with an example.

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Q. A solution of glucose in water is labelled as

10

% w/v, what would be the molality and mole fraction of each component in the solution? If the density of the solution is

1.2 g m L^{- 1}

, then what shall be the molarity of the solution?

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Q. The partial pressure of ethane over a solution containing

6.56 \times 10^{- 3} g

of ethane is

1

bar. If the solution contains

5.00 \times 10^{- 2} g

of ethane, then what shall be the partial pressure of the gas?

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Q. A

5

% solution (by mass) of cane sugar in water has freezing point of

271 K

. Calculate the freezing point of

5

% glucose in water if freezing point of pure water is

273.15 K

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Q. Calculate the mass of a non-volatile solute (molar mass

40 g m o l^{- 1}

) which should be dissolved in

114 g

octane to reduce its vapour pressure to

80

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Q. What is meant by positive and negative deviations from Raoult's law and how is the sign of

Δ_{m i x} H

related to positive and negative deviations from Raoult's law?

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Q. Two elements

A

and

B

form compounds having formula

A B_{2}

and

A B_{4}

. When dissolved in

20 g

of benzene

(C_{6} H_{6}), 1 g

A B_{2}

lowers the freezing point by

2.3 K

whereas

1.0 g

A B_{4}

lowers it by

1.3 K

. The molar depression constant for benzene is

5.1 K k g m o l^{- 1}

. Calculate atomic masses of

A

and

B

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Q. How many mL of

0.1 M H C l

are required to react completely with

1 g

mixture of

N a_{2} C O_{3}

and

N a H C O_{3}

containing equimolar amounts of both?

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Q. The vapour pressure of water is

12.3 k P a

300 K

. Calculate the vapour pressure of

1

molal solution of a non-volatile solute in it.

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Q. A solution is obtained by mixing

300 g

25

% solution and

400 g

40

% solution by mass. Calculate the mass percentage of the resulting solution

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Q. Define the following terms:
(i) Mole fraction

(ii) Molality

(iii) Molarity

(iv) Mass percentage.

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Q. State Henry's law and mention some important applications?

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Q. A solution containing

30 g m

of non-volatile solute exactly in

90 g m

of water has a vapour pressure of

2.8 k P a

298 K

. Further,

18 g m

of water is then added to the solution and the new vapour pressure becomes

2.9 k P a

298 K

Calculate: (i) molar mass of the solute (ii) vapour pressure of water at

298 K

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Q. Give an example of a solid solution in which the solute is a gas.

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Q. An antifreeze solution is prepared from

222.6 g

of ethylene glycol

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

and

200 g

of water. Calculate the molality of the solution. If the density of the solution is

1.072 g m L^{- 1}

, then what shall be the molarity of the solution?

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Q. Why do gases always tend to be less soluble in liquids as the temperature is raised?

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Q. A sample of drinking water was found to be severely contaminated with chloroform

(C H C l_{3})

supposed to be a carcinogen. The level of contamination was

15 p p m

(by mass):

(i) express this in percent by mass

(ii) determine the molality of chloroform in the water sample.

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