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**Q.****1. Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K _{2}SO_{4} in 2 liter of water at 25Â° C, assuming that it is completely dissociated.**

K

Total number of ions produced = 3

i =3

Given,

w = 25 mg = 0.025 g

V = 2 L

T = 25

Also, we know that:

R = 0.0821 L atm K

M = (2 Ã— 39) (1 Ã— 32) (4 Ã— 16) = 174 g mol

Appling the following relation,

**Q.****2. Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride.** **Ans. Benzene**

Let the total mass of the solution be 100 g and the mass of benzene be 30 g.

âˆ´ Mass of carbon tetrachloride = (100 âˆ’ 30)g = 70 g

Molar mass of benzene (C_{6}H_{6}) = (6 Ã— 12 + 6 Ã— 1) g mol^{âˆ’1} = 78 g mol^{âˆ’1}

âˆ´ Number of moles of C_{6}H_{6} = 30 /78 mol = 0.3846 mol

Molar mass of carbon tetrachloride (CCl_{4}) = 1 Ã— 12 + 4 Ã— 355 = 154 g mol^{âˆ’1}

âˆ´ Number of moles of CCl_{4} = 70/154 mol = 0.4545 mol

Thus, the mole fraction of C_{6}H_{6} is given as:

= 0.458**Q.****3. Calculate the molarity of each of the following solutions:****(a) 30 g of Co(NO _{3})_{2}. 6H_{2}O in 4.3 L of solution**

Molarity = Moles of solute/Volume of solution in litre

âˆ´ Moles of Co (NO

Therefore, molarity = 0.103 mol/4.3 L = 0.023 M

âˆ´ Number of moles present in 30 mL of 0.5 M H

Therefore, molarity = 0.015/0.5 L mol = 0.03 M

w

K

Î”T

We know that:

Therefore, observed molar mass of

CH_{2}FCOOH, (M_{2})_{obs} = 72.54 g mol

The calculated molar mass of CH_{2}FCOOH is:

(M_{2})_{cal} = 14 + 19 + 12 + 16 + 16 + 1

=78 g mol^{-1}

Therefore,

=1.0753

Let Î± be the degree of dissociation of CH_{2}FCOOH

Total = C(1 + Î±)

â‡’ i = 1 + Î±

â‡’ Î± = i - 1

= 1.0753 - 1

= 0.0753

Now, the value of K_{a} is given as:

Taking the volume of the solution as 500 mL, we have the concentration:

= 0.5 M

Therefore,

= 0.00307 (approximately)

= 3.07 Ã— 10^{-3}**Q.****5. Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density of 20% (mass/mass) aqueous KI is 1.202 g mL ^{-1}.**

20% (mass/mass) aqueous solution of KI means 20 g of KI is present in 100 g of solution.

That is,

20 g of KI is present in (100 âˆ’ 20) g of water = 80 g of water

Therefore,

Molality of the solution

= 1.506 m

= 1.51 m (approximately)

âˆ´ Volume of 100 g solution = Mass / Density

= 83.19 mL

= 83.19 Ã— 10

Therefore, molarity of the solution

= 1.45 M

**(c)** Moles of Kl = 20/166 = 0.12 mol

Moles of water = 80/18 = 4.44

Therefore, mole fraction of Kl

= 0.0263**Q.****6. H _{2}S, a toxic gas with rotten egg like smell, is used for the qualitative analysis. If the solubility of H_{2}S in water at STP is 0.195 m, calculate Henryâ€™s law constant.**

âˆ´ Mole fraction of H

At STP, pressure (p) = 0.987 bar

According to Henryâ€™s law:

p = K_{H}x

= 0.987 / 0.0035 Bar

= 282 bar**Q.****7. Henryâ€™s law constant for CO _{2} in water is 1.67 Ã— 10^{8} Pa at 298 K. Calculate the quantity of CO_{2} in 500 mL of soda water when packed under 2.5 atm CO_{2} pressure at 298 K.**

p

= 2.533125 Ã— 10

According to Henryâ€™s law:

= 0.00152

We can write,

[Since, is negligible as compared to ]

In 500 mL of soda water, the volume of water = 500 mL

[Neglecting the amount of soda present]

We can write:

500 mL of water = 500 g of water

= 27.78 mol of water

Now,

Hence, quantity of CO_{2} in 500 mL of soda water = (0.042 Ã— 44)g

= 1.848 g**Q.****8. The vapour pressure of pure liquids A and B are 450 and 700 mm Hg respectively, at 350 K. Find out the composition of the liquid mixture if total vapour pressure is 600 mm Hg. Also find the composition of the vapour phase.****Ans. **It is given that:

from Rault's law, we have:

Therefore, total pressure

â‡’ 600 = (450 - 700) x_{A} + 700

â‡’ - 100 = -250x_{A}

â‡’ x_{A} = 0.4

Therefore, x_{B }= 1 - x_{A}

= 1 - 0.4

= 0.6

Now,

= 450 Ã— 0.4

= 180 mm of Hg

= 700 Ã— 0.6

= 420 mm of Hg

Now, in the vapour phase:

Mole fraction of liquid

And, mole fraction of liquid B = 1 âˆ’ 0.30 = 0.70**Q.****9. Vapour pressure of pure water at 298 K is 23.8 mm Hg. 50 g of urea (NH _{2}CONH_{2}) is dissolved in 850 g of water. Calculate the vapour pressure of water for this solution and its relative lowering.**

Weight of water taken, w

Weight of urea taken, w

Molecular weight of water, M

Molecular weight of urea, M

Now, we have to calculate vapour pressure of water in the solution. We take vapour

pressure as p

Now, from Raoultâ€™s law, we have:

Hence, the vapour pressure of water in the given solution is 23.4 mm of Hg and its relative lowering is 0.0173.**Q.****10. Boiling point of water at 750 mm Hg is 99.63Â°C. How much sucrose is to be added to 500 g of water such that it boils at 100Â°C. Molal elevation constant for water is 0.52 K kg mol ^{âˆ’1}.**

Î”T

= 0.37 K

Mass of water, w

Molar mass of sucrose (C

= 342 g mol

Molal elevation constant, K

We know that:

= 121.67 g (approximately)

Hence, 121.67 g of sucrose is to be added.**Note:** There is a slight variation in this answer and the one given in the NCERT textbook.**Q.****11. Determine the amount of CaCl _{2} (i = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27Â°C.**

Ï€ = 0.75 atm

V = 2.5 L

i = 2.47

T = 300 K

Here,

R = 0.0821 L atm K

M = 1 Ã— 40.2 Ã— 35.5

= 111 g mol

Therefore,

Hence, the required amount of CaCl_{2} is 3.42 g.**Q.****12. Vapour pressure of water at 293 K is 17.535 mm Hg. Calculate the vapour pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water.****Ans. **Vapour pressure of water, pÂ°_{1} = 17.535 mm of Hg

Mass of glucose, w_{2} = 25 g

Mass of water, w_{1} = 450 g

We know that,

Molar mass of glucose (C_{6}H_{12}O_{6}), M_{2} = 6 Ã— 12 + 12 Ã— 1 + 6 Ã— 16

= 180 g mol^{âˆ’1}

Molar mass of water, M_{1} = 18 g mol^{âˆ’1}

Then, number of moles of glucose,

= 0.139 mol

And, number of moles of water,

= 25 mol

We know that,

â‡’ p_{1} = 17.44 mm of Hg

Hence, the vapour pressure of water is 17.44 mm of Hg.**Q.****13. Define the term solution. How many types of solutions are formed? Write briefly about each type with an example.****Ans. **Homogeneous mixtures of two or more than two components are known as solutions.

There are three types of solutions.**(i) Gaseous solution: **The solution in which the solvent is a gas is called a gaseous solution. In these solutions, the solute may be liquid, solid, or gas.**Example:** a mixture of oxygen and nitrogen gas is a gaseous solution.**(ii) Liquid solution: **The solution in which the solvent is a liquid is known as a liquid solution. The solute in these solutions may be gas, liquid, or solid.**Example:** a solution of ethanol in water is a liquid solution.**(iii) Solid solution: **The solution in which the solvent is a solid is known as a solid solution. The solute may be gas, liquid or solid. For example, a solution of copper in gold is a solid solution.**Q.****14. Give an example of solid solution in which the solute is a gas.****Ans. **In case a solid solution is formed between two substances (one having very large particles and the other having very small particles), an interstitial solid solution will be formed.**Example:** a solution of hydrogen in palladium is a solid solution in which the solute is a gas.

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