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Solutions

Short Answer Type

1. Calculate the mass percentage of benzene (C₆H₆) and carbon tetrachloride (CCl₄) if 22 g of benzene is dissolved in 122 g of carbon tetrachloride.

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Long Answer Type

Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride.

897 Views

3. Calculate the molarity of each of the following solution (a) 30 g of Co(NO₃)₂.6H₂O in 4.3 L solution (b) 30 mL of 0.5 MH₂SO₄ diluted to 500 mL.

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4. Calculate the mass of urea (NH₂CONH₂) required in making 2.5 kg 0.25 of molal aqueous solution.

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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.

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Short Answer Type

6. H₂S, a toxic gas with rotten egg like smell, is used for the qualitative analysis. If the solubility of H₂S in water at S.T.P. is 0.195 m, calculate Henry's law constant.

It is given that the solubility of H₂S in water at STP is 0.195m, i.e., 0.195 mol of H₂S is dissolved in1000 g of water.

= $\frac{1000 g}{18 g {mol}^{- 1}} m o l e s o f w a t e r = 55.56 m o l = \frac{m o l e s o f H_{2} S}{m o l e s o f H_{2} S + m o l e s o f w a t e r} = \frac{0.195}{0.195 + 55.56} = 0.0035$

At STP pressure (P) = 0.987bar
According to henry's law p = k_Hx

$K_{H} = \frac{p}{x} = \frac{0.987}{0.0035} bar = 282 bar$

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7. Henry’s law constant for CO₂ in water is 1.67 x 10⁸ P_a at 298 K. Calculate the quantity of CO₂ in 500 mL of soda water when packed under 2.5 atm CO₂ pressure at 298 K.

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8. The vapour pressure of pure liquids A and B are 450 and 700 mm Hg at 350 K respectively. Find out the composition of the liquid mixture if total vapour pressure is 600 mm Hg. Also find the composition of the vapour phase.

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Long Answer Type

9. Vapour pressure of pure water at 298 K is 23.8 mm. 50 g of urea (NH₂CONH₂) is dissolved in 850 g of water. Calculate the vapour pressure of water for this solution and its relative lowering.

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