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If 22 g of benzene is dissolved in 122 g of carbon tetrachloride then the mass percentage of benzene (C6H6) and carbon tetrachloride (CCl4) are respectively:
1. 86.32 %; 13.68 %
2. 13.68 %; 86.32 %
3. 84.72 %; 15.28 %
4. 15.28 %; 84.72 %
Q1:
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Subtopic:  Concentration Terms & Henry's Law |
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The mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride is:

1. 0.528
2. 0.618
3. 0.458
4. 0.338
Q2:
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The molarity of 30 g Co(NO3)2. 6H2O in 4.3 L of solution is:

1. 0.053 M
2. 0.043 M
3. 0.023 M
4. 0.063 M

Q3:
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What mass of urea (NH₂CONH₂) is needed to prepare 2.5 kg of a 0.25 molal solution?
1. 39 g 2. 37 g
3. 41 g 4. 35 g
Q4:
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Calculate the molarity of the KI solution, provided its density is 1.202 g mL-1 and it consists of a 20% (mass/mass) concentration.

1. 1.25 M
2. 1.95 M
3. 1.45 M
4. 2.15 M
Q5:
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The solubility of H2S in water at STP is 0.195 m, The value of Henry’s law constant will be:
1. 274 atm 2. 285 atm
3. 295 atm 4. 278 atm
Q6:
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Henry’s law constant for CO2 in water is 1.67 × 108 Pa at 298 K. The quantity of CO2 in 500 mL of soda water when packed under 2.5 atm CO2 pressure at 298 K is:
1. 1.24 g 2. 1.45 g
3. 1.65 g 4. 1.85 g
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The vapour pressure of pure liquids A and B are 450 and 700 mm Hg respectively, at 350 K.  If the total vapour pressure is 600 mm Hg then the composition of the vapour phase are:

1. XA=0.30; XB=0.70
2. XA=0.40; XB=0.60
3. XA=0.20; XB=0.90
4. XA=0.50; XB=0.50
 

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Subtopic:  Raoult's Law |
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Vapour pressure of pure water at 298 K is 23.8 mm Hg. 50 g of urea (NH2CONH2) is dissolved in 850 g of water.
The vapour pressure of water (in mm Hg) for this solution is : 
1. 23.40 2. 0.23 
3. 12.87 4. 40.14
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Subtopic:  Raoult's Law |
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If the boiling point of water at 750 mm Hg is 99.63°C, what quantity of sucrose is needed to be dissolved in 500 g of water to achieve a boiling point of 100°C?
(Molal elevation constant for water is 0.52 K kg mol−1 )

1. 128.17 g
2. 121.67 g
3. 125.57 g
4. 116.27 g
Q10:
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Subtopic:  Elevation of Boiling Point |
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