CUET Chemistry MCQs Unit II Solutions

Question : When a solute is present in trace quantities the following expression is used

a) Gram per million

b) Milligram percent

c) Microgram percent

d) Parts per million

Answer : D

Question : Which of the following concentration terms is/are independent of temperature?

a) Molality only

b) Molality and mole fraction

c) Molarity and mole fraction

d) Molality and normality

Answer : B

Question : Which of the following concentration unit is independent of temperature ?

a) Normality

b) Molarity

c) Formality

d) Molality

Answer : D

Question : An aqueous solution of glucose is 10% in strength. The volume in which 1 g mole of it is dissolved, will be

a) 9 litre

b) 1.8 litre

c) 8 litre

d) 0.9 litre

Answer : B

Question : An aqueous solution of hydrochloric acid

a) Obeys Raoult’s law

b) Shows negative deviation from Raoult’s law

c) Shows positive deviation from Raoult’s law

d) Obeys Henry’s law at all compositions

Answer : B

Question. Dilute one litre 1 molar H₂SO₄ solution by 5 litre water, the normality of that solution is:

a. 0.2 N

b. 5 N

c. 10 N

d. 0.33 N

Answer : D

Question : At a particular temperature, the vapour pressures of two liquids A and B are respectively 120 and 180 mm of mercury. If 2 moles of A and 3 moles of B are mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be (in mm of mercury)

a) 156

b) 145

c) 150

d) 108

Answer : A

Question. Which solution will show the maximum vapour pressure at 300 K ?

a. 1 M C₁₂ H₂₂ O₁₁

b. 1 M CH₃ COOH

c. 1 M NaCl₃

d. 1 M NaCl

Answer : A

Question : 10 Which observation(s) reflect(s) colligative properties?

(i) A 0.5 m NaBr solution has a higher vapour pressure than a 0.5 m BaCl₂ solution at the same temperature

(ii) Pure water freezes at the higher temperature than pure methanol

(iii) a 0.1 m NaOH solution freezes at a lower temperature than pure water

Choose the correct answer from the codes given below

a) (i), (ii) and (iii)

b) (i) and (ii)

c) (ii) and (iii)      

d) (i) and (iii)

Answer : D

Question. The azeotropic mixture of water (b.p. 100°C) and HCl (b.p.85°C) boils at 108.5°C. When this mixture is distilled it is possible to obtain?

a. Pure HCl

b. Pure water

c. Pure water as well as pure HCl

d. Neither HCl nor H₂O in their pure states

Answer : D

Question : The colligative property is not represented by :

a) elevation in boiling point

b) osmotic pressure

c) optical activity

d) relative lowering of vapour pressure

Answer : C

Question. What volume of 0.8 M solution contains 0.1 mole of the solute?

a. 100 ml

b. 125 ml

c. 500 ml

d. 62.5

Answer : B

Question : The vapour pressure of pure benzene at a certain temperature is 0.850 bar. A non-volatile, nonelectrolyte solid weighing 0.5 g is added to 39.0 g of benzene (molar mass 78 g/mol). The vapour pressure of the solution then is 0.845 bar. What is the molecular mass of the solid substance? 

a) 58  

b) 180

c) 170

d) 145.

Answer : C

Question. A solution of Al₂ (SO₄)₃ {d = 1.253gm/ml} contain 22% salt by weight. The molarity, normality and molality of the solution is:

a. 0.805 M, 4.83 N, 0.825 M

b. 0.825 M, 48.3 N, 0.805 M

c. 4.83 M, 4.83 N, 4.83 M

d. None

Answer : A

Question : The term homogenous mixtures signifies that

a) its composition is uniform throughout the mixture.

b) its properties are uniform throughout the mixture.

c) both composition and properties are uniform throughout the mixture.

d) neither composition nor properties are uniform throughout the mixture.

Answer : C

Question. 3.65 gms of HCl is dissolved in 16.2 gms of water. The mole fraction of HCl in the resulting solution is:

a. 0.4

b. 0.3

c. 0.2

d. 0.1

Answer : D

Question : 1 M, 2.5 litre NaOH solution is mixed with another 0.5 M, 3 litre NaOH solution. Then find out the molarity of resultant solution

a) 0.80 M

b) 1.0 M

c) 0.73 M

d) 0.50 M

Answer : C

Question. A mixture has 18g water and 414g ethanol. The mole fraction of water in mixture is: (assume ideal behaviour of the mixture)

a. 0.1

b. 0.4

c. 0.7

d. 0.9

Answer : A

Question : The molarity of pure water is

a) 50 M

b) 18 M

c) 55.6 M

d) 100 M

Answer : C

Question. A solution has a 1 : 4 mole ratio of pentane to hexane. The vapour pressure of the pure hydrocarbons at 20°C are 440 mmHg for pentane and 120 mmHg for hexane. The mole fraction of pentane in the vapour phase would be:

a. 0.549

b. 0.200

c. 0.786

d. 0.478

Answer : D

Question : The mole fraction of the solute in one molal aqueous solution i

a) 0.009

b) 0.018

c) 0.027

d) 0.036

Answer : B

Question. The vapour pressure of benzene at a certain temperature is 640 mm of Hg. A non-volatile and non-electrolyte solid weighing 2.175 g is added to 39.08 g of benzene. The vapour pressure of the solution is 600 mm of Hg. What is the molecular weight of solid substance?

a. 49.50

b. 59.6

c. 69.5

d. 79.8

Answer : C

Question : What is the normality of a 1 M solution of H₃PO₄ ?

a) 0.5 N

b) 1.0 N

c) 2.0 N

d) 3.0 N

Answer : D

Question. The ratio of the value of any colligative property for KCl solution to that for sugar solution is nearly:

a. 1

b. 0.5

c. 2.0

d. 3

Answer : C

Question : For preparing 0.1 N solution of a compound from its impure sample of which the percentage purity is known, the weight of the substance required will be

a) Less than the theoretical weight

b) More than the theoretical weight

c) Same as the theoretical weight

d) None of these

Answer : B

Question. Which of the following compounds corresponds Van't Hoff factor ' i' to be equal to 2 for dilute solution?

a. K₂SO₄

b. 4 NaHSO₄

c. Sugar

d. MgSO₄

Answer : D

Question : A solution is prepared by dissolving 10 g NaOH in 1250 mL of a solvent of density 0.8 mL/g. The molality of the solution in mol kg–1 is

a) 0.25

b) 0.2

c) 0.008

d) 0.0064

Answer : A

Question. Which of the following should be done in order to prepare 0.40M NaCl starting with 100ml of 0.30M NaCl (mol.wt. of NaCl = 58.5)?

a. Add 0.585 g NaCl

b. Add 20 ml water

c. Add 0.010 ml NaCl

d. Evaporate 10 ml water

Answer : A

Question : When a solid solute is added to the solvent, some solute dissolves and its concentration increases in solution. This process is known as ______. Some solute particles in solution collide with the solid solute particles and get separated out of solution. This process is known as ______.

a) Crystallization, dissolution.

b) Dissolution, saturation.

c) Saturation, crystallization.

d) Dissolution, crystallization.

Answer : D

Question. How many grams of CH₃ OH should be added to water to prepare 150ml solution of  2MCH₃OH?

a. 9.6

b. 2.4

c. 9..6×10³

d. 2.4×10³

Answer : A

Question : The statement “If 0.003 moles of a gas are dissolved in 900 g of water under a pressure of 1 atmosphere, 0.006 moles will be dissolved under a pressure of 2 atmospheres”,illustrates

a) Dalton’s law of partial pressure

b) Graham’s law

c) Raoult’s law

d) Henry’s law

Answer : D

Question. Which of the following colligative properties can provide molar mass of proteins (or polymers or colloids) with greater precision?

a. Relative lowering of vapour pressure

b. Elevation of boiling point

c. Depression in freezing point

d. Osmotic pressure

Answer : D

Question : A beaker contains a solution of substance ‘A’. Precipitation of substance ‘A’ takes place when small amount of ‘A’ is added to the solution. The solution is ______.

a) saturated

b) supersaturated

c) unsaturated

d) concentrated

Answer : B

Question. If 5.85 gms of NaCl are dissolved in 90 gms of water, the mole fraction of NaCl is:

a. 0.1

b. 0.2

c. 0.3

d. 0.0196

Answer : D

Question : The value of Henry's constant KH is _______.

a) greater for gases with higher solubility.

b) greater for gases with lower solubility.

c) constant for all gases.

d) not related to the solubility of gases.

Answer : B

Question. The average osmotic pressure of human blood is 7.8 bar at 37°C. What is the concentration of an aqueous NaCl solution that could be used in the blood stream?

a. 0.16 mol/L

b. 0.32 mol/L

c. 0.60 mol/L

d. 0.45 mol/L

Answer : B

Question : Exactly 1 g of urea dissolved in 75 g of water gives a solution that boils at 100.114°C at 760 torr. The molecular weight of urea is 60.1. The boiling point elevation constant for water is

a) 1.02

b) 0.51

c) 3.06

d) 1.51

Answer : B

Question. A solution contains 1 mole of water and 4 mole of ethanol. The mole fraction of water and ethanol will be:

a. 0.2 water + 0.8 ethanol

b. 0.4 water + 0.6 ethanol

c. 0.6 water + 0.8 ethanol

d. 0.8 water + 0.2 ethanol

Answer : A

Question : The vapour pressure of a solvent decreases by 10 mm of Hg when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be the mole fraction of the solvent if the decrease in the vapour pressure is to be 20 mm of Hg ?

a) 0.8

b) 0.6

c) 0.4

d) 0.2

Answer : B

Question. In a mixture of 1 gm H₂ and 8gm O₂ , the mole fraction of hydrogen is:

a. 0.667

b. 0.5

c. 0.33

d. None of these

Answer : A

Question : 20 g of a substance were dissolved in 500 mL of water and the osmotic pressure of the solution was found to be 600 mm of mercury at 15°C. The molecular weight of substance is :

a) 998  

b) 1028

c) 1098

d) 1198

Answer : D

Question. The vapour pressure of pure liquid A is 0.80 atm. On mixing a non-volatile B to A, its vapour pressure becomes 0.6 atm. The mole fraction of B in the solution is:

a. 0.150

b. 0.25

c. 0.50

d. 0.75

Answer : B

Question : 0.01 M solution of KCl and BaCl2 are prepared in water. The freezing point of KCl is found to be –2°C. What is the freezing point of BaCl2 to be completely ionised ?

a) – 3°C

b) + 3°C

c) – 2°C

d) – 4°C

Answer : A

Question. For 0.1 M solution, the colligative property will follow the order:

a. NaCl > Na₂ SO₄ > Na₃ PO₄

b. NaCl < Na₂ SO₄ < Na₃ PO₄

c. NaCl > Na₂ SO₄ ≈ Na₃ PO₄

d. NaCl < Na₂ SO₄ = Na₃ PO₄

Answer : B

Question : Which of the following mixture is(are) called solution?

(i) water + ammonia (ii) water + acetone

(iii) acetone + alcohol (iv) hexane + water

a) (i), (ii) and (iii)

b) (i), (iii) and (iv)

c) (i) and (iv)

d) (ii) and (iii)

Answer : A

Question. Which one of the following aqueous solutions will exhibit highest boiling point?

a. 0.015 M urea

b. 0.01MKNO₃

c. 0.01MNa₂ SO₄

d. 0.015M glucose

Answer : C

Question : The molarity of the solution containing 7.1 g of Na2SO4 in 100 ml of aqueous solution is

a) 2 M

b) 0.5 M

c) 1 M

d) 0.05 M

Answer : B

Question. 9.8g of H₂SO₄ is present in 2 litres of a solution. The molarity of the solution is:

a. 0.1 M

b. 0.05 M

c. 0.2 M

d. 0.01 M

Answer : B

Question. A non ideal solution was prepared by mixing 30 ml chloroform and 50 ml acetone. The volume of mixture will be:

a. > 80 ml

b. < 80 ml

c. = 80 ml

d. ≥ 80 ml

Answer : B

Question. Which of the following is a colligative property?

a. Osmotic pressure

b. Boiling point

c. Vapour pressure

d. Freezing point

Answer : A

Question : 2.5 litres of NaCl solution contain 5 moles of the solute. What is the molarity?

a) 5 molar

b) 2 molar

c) 2.5 molar

d) 12.5 molar

Answer : B

Question : The volume of 4 N HCl and 10 N HCl required to make 1 litre of 6 N HCl are

a) 0.75 litre of 10 N HCl and 0.25 litre of 4 N HCl

b) 0.50 litre of 4 N HCl and 0.50 litre of 10 N HCl

c) 0.67 litre of 4 N HCl and 0.33 litre of 10 N HCl

d) 0.80 litre of 4 N HCl and 0.20 litre of 10 N HCl

Answer : C

Question. Two solutions A and B are separated by semi- permeable membrane. If liquid flows from A to B then:

a. A is less concentrated than B

b. A is more concentrated than B

c. Both have same concentration

d. None of these

Answer : A

Question : At the state of dynamic equilibrium, for solute + solvent solution.

a) Rate of dissolution = Rate of unsaturation.

b) Rate of dissolution = Rate of unsaturation.

c) Rate of dissolution = Rate of saturation

d) Rate of crystallization = Rate of saturation.

Answer : B

Question : According to Henry’s law, the amount of gas that will dissolve in blood plasma or any other liquid is determined by which of these factor?

a) Solubility of the gas in the liquid.

b) The total pressure of the gas mixture .

c) pH of the liquid.

d) The osmotic pressure of the gas mixture.

Answer : A

Question. A solution of urea (mol. mass 56g mol^–1) boils at 100.18°C at the atmospheric pressure. If K_f and K_b for water are1.86 and 0.512K kg mol^–1 respectively the above solution will freeze at:

a. – 6.54°C

b. 6.54°C

c. 0.654°C

d. 0.654°C

Answer : D

Question. If 1 M and 2.5 litre NaOH solution is mixed with another 0.5 M and 3 litre NaOH solution, then molarity of the resultant solution will be:

a. 1.0 M

b. 0.73 M

c. 0.80 M

d. 0.50 M

Answer : B

Question. Elevation in boiling point was o 0.52 C when 6gm of a compound X was dissolved in 100gm of water. Molecular weight of X is: b (K for water is 0.52 per 1000 gm of water)

a. 120

b. 60

c. 180

d. 600

Answer : B

Question. Calculate the molal depression constant of a solvent which has freezing point 16.6^o C and latent heat of fusion 180.75 Jg⁻¹

a. 2.68

b. 3.86

c. 4.68

d. 2.86t6

Answer : B

Question : Maximum amount of a solid solute that can be dissolved in a specified amount of a given liquid solvent does not depend upon __________.

a) Temperature

b) Nature of solute

c) Pressure

d) Nature of solvent

Answer : C

Question. Which of the following is not a colligative property?

a. Osmotic pressure

b. Elevation in B.P.

c. Vapour pressure

d. Depression in freezing point

Answer : C

Question : Which of the followingfactor(s) affect the solubility of a gaseous solute in the fixed volume of liquid solvent ?

(i) Nature of solute (ii) Temperature (iii) Pressure

a) (i) and (iii) at constant T

b) (i) and (ii) at constant P

c) (ii) and (iii) only

d) (iii) only

Answer : A

Question :   12g of urea is dissolved in 1 litre of water and 68.4 g of sucrose is dissolved in 1 litre of water. The lowering of vapour pressure of first case is

a) equal to second

b) greater than second

c) less than second

d) double that of second

Answer : A

Question. A liquid mixture boils without changing constituent is called:

a. Stable structure complex

b. Binary liquid mixture

c. Zeotropic liquid mixture

d. Azeotropic liquid mixture

Answer : D

Question : A solution containing 1.8 g of a compound (empirical formula CH₂O) in 40 g of water is observed to freeze at –0.465° C. The molecular formula of the compound is (K_f of water = 1.86 kg K mol^–1)

a) C₂H₄O₂

b) C₃H₆O₃

c) C₄H₈O₄

d) C₆H₁₂O₆

Answer : D

Question. The molality of 90% H₂ SO₄ solution is: [density=1.8 gm/ml]

a. 1.8

b. 48.4

c. 9.18

d. 94.6

Answer : C

Question. The amount of K₂ Cr₂ O₇ (eq.wt.49.04) required to prepare 100 ml of its 0.05 N solution is:

a. 2.9424 g

b. 0.4904 g

c. 1.4712 g

d. 0.2452 g

Answer : D

Question : Which one of the statements given below concerning properties of solutions, describes a colligative effect?

a) Boiling point of pure water decreases by the addition of ethanol

b) Vapour pressure of pure water decreases by the addition of nitric acid

c) Vapour pressure of pure benzene decreases by the addition of naphthalene

d) Boiling point of pure benzene increases by the addition of toluene

Answer : C

Question. The freezing point of a 0.01M aqueous glucose solution at 1 atmosphere is o −0.18 C. To it, an addition of equal volume of 0.002M glucose solution will; produce a solution with freezing point of nearly:

a. −0.036^o C

b. −0.108^o C

c. −0.216^o C

d. −0.422^o C

Answer : C

Question : Which of the following fluoride is used as rat poison?

a) CaF₂

b) KF

c) NaF

d) MgF₂

Answer : C

Question. If two substances A and B have P⁰_A : P⁰_B =1: 2 and have mole fraction in solution 1 : 2 then mole fraction of A in vapours:

a. 0.33

b. 0.25

c. 0.52

d. 0.2

Answer : D

Question : An X molal solution of a compound in benzene has mole fraction of solute equal to 0.2. The value of X is

a) 14

b) 3.2

c) 1.4

d) 2

Answer : B

Question. Which of the following will have the lowest vapour pressure?

a. 0.1 M KCl solution

b. 0.1 M urea solution

c. 0.1MNa₂ SO₄ solution

d. 0.1MK₄ Fe(CN)₆ solution

Answer : D

Question : On adding a solute to a solvent having vapour pressure 0.80 atm, vapour pressure reduces to 0.60 atm. Mole fraction of solute is

a) 0.25

b) 0.75

c) 0.50

d) 0.33

Answer : A

Question. 171 g of cane sugar (C₁₂ H₂₂ O₁₁) is dissolved in 1 litre of water. The molarity of the solution is:

a. 2.0 M

b. 1.0 M

c. 0.5 M

d. 0.25 M

Answer : C

Question : Molarity of H2SO4 is 18 M. Its density is 1.8 g/ml. Hence molality is

a) 36

b) 200

c) 500

d) 18

Answer : C

Question. A dry air is passed through the solution, containing the 10 gm of solute and 90 gm of water and then it pass through pure water. There is the depression in weight of solution wt by 2.5 gm and in weight of pure solvent by 0.05 gm.

Calculate the molecular weight of solute:

a. 50

b. 180

c. 100

d. 25

Answer : C

Question : A solution made by dissolving 40 g NaOH in 1000 g of water is

a) 1 molar

b) 1 normal

c) 1 molal

d) None of these

Answer : C

Question. In equimolar solution of glucose, NaCl and BaCl2, the order of osmotic pressure is as follow:

a. Glucose  >NaCl > BaCl₂

b.  NaCl > BaCl₂ > Glucose

c.  BaCl₂ > NaCl > Glucose

d. Glucose > BaCl₂ > NaCl

Answer : C

Question : Which of the following factor do not affect solubility of solid solute in liquid ?

a) Temperature

b) Pressure

c) Nature of solute

d) All of these

Answer : B

Question. The molarity of 0.006 mole of NaCl in 100 ml solution is:

a. 0.6

b. 0.06

c. 0.006

d. 0.066

Answer : B

Question : Henry’s law constant of oxygen is 1.4 × 10–3 mol. lit–1. atm–1 at 298 K. How much of oxygen is dissolved in 100 ml at 298 K when the partial pressure of oxygen is 0.5 atm?

a) 1.4 g

b) 3.2 g

c) 22.4 mg

d) 2.24 mg

Answer : D

Question. The elevation in boiling point of a solution of 13.44g of CuCl₂ in 1kg of water using the following information will be: (Molecular weight of CuCl₂=134.4 and K_b=0.52K molal⁻¹)

a. 0.16

b. 0.05

c. 0.1

d. 0.2

Answer : A

Question : Value of Henry's constant KH _______.

a) increases with increase in temperature.

b) decreases with increase in temperature.

c) remains constant.

d) first increases then decreases.

Answer : A

Question. When 10g of a non-volatile solute is dissolved in 100 g of benzene, it raises boiling point by o 1 C then molecular mass of the solute is: b (K_b for benzene = 2.53k-m^–1)

a. 223 g

b. 233 g

c. 243 g

d. 253 g

Answer : D

Question : The vapour pressure of benzene at 30°C is 121.8 mm. By adding 15 g of non-volatile solute in 250 g of benzene, its vapour pressure is decreased to 120.2 mm. The molecular weight of solute is :

a) 156.6 g

b) 267.4 g

c) 356.3 g

d) 467.4 g

Answer : C

Question. A 5% solution of canesugar (mol. wt. = 342) is isotonic with 1% solution of a substance X. The molecular weight of X is:

a. 34.2

b. 171.2

c. 68.4

d. 136.8

Answer : C

Question : “The importance of many pure substance in life depends on their composition.” Which of the following statement justify the above fact?

a) 1 ppm of fluoride ions in water prevents tooth decay.

b) 1.5 ppm of fluoride ions causes tooth decay.

c) Concentration above 1.5 ppm can be poisonous.

d) All of the above.

Answer : D

Question. On dissolving 1 mole of each of the following acids in 1 litre water, the acid which does not give a solution of strength 1 N is?

a. HCl

b. Perchloric acid

c. HNO₃

d. Phosphoric acid

Answer : D

Question : The vapour pressure of pure benzene at 25°C is 640 mm Hg and that of solution of solute A is 630 mm Hg. The molality of solution is

a) 0.2 m

b) 0.4 m

c) 0.5 m

d) 0.1 m

Answer : A

Question. Acetic acid dissolved in benzene shows a molecular weight of:

a. 60

b. 120

c. 180

d. 240

Answer : B

Question : 200 ml of water is added to 500 ml of 0.2 M solution. What is the molarity of this diluted solution ?

a) 0.5010 M

b) 0.2897 M

c) 0.7093 M

d) 0.1428 M

Answer : D

Question. Which one of the following mixtures can be separated into pure components by fractional distillation?

a. Benzene–toluene

b. Water–ethyl alcohol

c. Water–nitric acid

d. Water–hydrochloric acid

Answer : A

Question : The freezing point of equimolal aqueous solution will be highest for

a) C₆H₅NH₃ ⁺Cl^–  

b) Ca(NO₃)₂

c) La(NO₃)₂        

d) C₆H₁₂O₆

Answer : D

Question. Which of the following 0.10m aqueous solution will have the lowest freezing point?

a) Al₂ (SO₄)₃

b) C₃ H₁₀ O₅

c) KI

d) C₁₂ H₂₂ O₁₁

Answer : A

Question : Pure benzene freezes at 5.45°c. A 0.374 m solution of tetrachloroethane in benzene freezes at 3.55°c. The Kf for benzene is:

a) 0.508

b) 5.08

c) 50.8  

d) 508

Answer : B

Question. The amount of urea to be dissolved in 500 ml of water (K =18.6K mole⁻¹ in 100g solvent) to produce a depression of o 0.186 C in freezing point is:

a) 9 g

b) 6 g

c) 3 g

d) 0.3 g

Answer : C

Question : Most of the processes in our body occur in

a) solid solution

b) liquid solution

c) gaseous solution

d) colloidal solution

Answer : B

Question. The number of moles of KCl in 1000 ml of 3 molar solutions is:

a) 1

b) 2

c) 3

d) 1.5

Answer : C

Question : 4.0 g of NaOH is dissolved in 100 ml solution. The normality of the solution is

a) 0.1 N

b) 0.5 N

c) 4.0 N

d) 1.0 N

Answer : D

Question. Vapour pressure of CCl₄ at o 25 C is 143mm of Hg 0.5gm of a non-volatile solute (mol. wt.=65) is dissolved in 100mlCCl₄ . Find the vapour pressure of the solution:

(Density of CCl₄ = 1.58g / cm²)

a) 141.43mm

b) 94.39mm

c) 199.34mm

d) 143.99mm

Answer : A

Question : Mole fraction of the solute in a 1.00 molal aqueous solution is

a) 0.1770

b) 0.0177

c) 0.0344

d) 1.7700

Answer : B

Question : Which of the following units is useful in relating concentration of solution with its vapour pressure?

a) mole fraction

b) parts per million

c) mass percentage

d) molality

Answer : A

Question : At equillibrium the rate of dissolution of a solid solute in a volatile liquid solvent is ______.

a) less than the rate of crystallisation.

b) greater than the rate of crystallisation.

c) equal to the rate of crystallisation.

d) zero

Answer : C

Question : Which of the following 0.10 m aqueous solutions will have the lowest freezing point ?

a) Al₂(SO₄)₃

b) C₆H₁₂O₆

c) KCl           

d) C₁₂H₂₂O₁₁

Answer : A

Question : A solution containing 10g per dm³ of urea (molecular mass = 60 gmol^–1) is isotonic with a 5% solution of a non volatile solute. The molecular mass of this non volatile solute is

a) 300 g mol^–1

b) 350 g mol^–1

c) 200 g mol^–1

b) 250 g mol^–1

Answer : A

Question : Which of the following is a quantitative description of the solution?

a) Dilute

b) Concentrated

c) Saturated

d) Molar

Answer : D

Question : 10 g of NaCl is dissolved in 106g of the solution. Its concentration is

a) 100 ppm

b) 0.1 ppm

c) 1 ppm

d) 10 ppm

Answer : D

Question : If N/10 50 ml H2SO4,N/3 30 ml HNO3, N/2 10 ml HCl is mixed and solution is made to 1L. Then normality of resultant solution is

a)N/20

b)N/40

c) 50/N

d) N

Answer : C

Question : Which of the following statements is incorrect?

a) A solution in which no more solute can be dissolved at the same temperature and pressure is called a saturated solution.

b) An unsaturated solution is one in which more solute can be dissolved at the same temperature.

c) The solution which is in dynamic equilibrium with undissolved solute is the saturated solution.

d) The minimum amount of solute dissolved in a given amount of solvent is its solubility.

Answer : D

Question : Low concentration of oxygen in the blood and tissues of people living at high altitude is due to _________.

a) low temperature

b) low atmospheric pressure

c) high atmospheric pressure

d) both low temperature and high atmospheric pressure

Answer : B

Question : 0.450 g of urea (mol.wt.60) in 22.5 g of water show 0.170°C of elevation in boiling point. The molal elevation constant of water is:

a) 0.051°C

b) 0.51°C

c) 5.1°C    

d) 0.83°C

Answer : B

Question : Molarity of liquid HCl will be, if density of solution is 1.17 gm/cc

a) 36.5

b) 32.05

c) 18.25

d) 42.10

Answer : B

Question : How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3

a) 90.0 g conc. HNO3

b) 70.0 g conc. HNO₃

c) 54.0 g conc. HNO3

d) 45.0 g conc. HNO₃

Answer : D

Question : The average osmotic pressure of human blood is 7.8 bar at 37°C. What is the concentration of an aqueous NaCl solution that could be used in the blood stream?

a) 0.16 mol/L  

b) 0.31 mol / L

c) 0.60 mol / L

d) 0.45 mol / L

Answer : B

Question : 5 ml of N HCl, 20 ml of N/2 H2SO4 and 30 ml of N/3 HNO3 are mixed together and volume made to one litre. The normality of the resulting solution is

a)N5

b)N10

c)N20

d) N/40

Answer : D

Question : On dissolving sugar in water at room temperature solution feels cool to touch. Under which of the following cases dissolution of sugar will be most rapid ?

a) Sugar crystals in cold water.

b) Sugar crystals in hot water.

c) Powdered sugar in cold water.

d) Powdered sugar in hot water.

Answer : D

Question : The solubility of a solid in a liquid is significantly affected by temperature changes.

Solute + Solvent → Solution.

The system being in a dynamic equilibrium must follow

Le-chatelier’s principle. Considering the Le-chatelier’s

principle which of the following is correct?

a) △H_sol > 0; solubility ↑ ; temperature ↓

b) △H_sol < 0; solubility ↓ ; temperature ↑

c) △H_sol > 0; solubility ↓; temperature ↑

d) △H_sol < 0; solubility ↓ ; temperature ↑

Answer : B

Question : A 5% solution (by mass) of cane sugar in water has freezing point of 271 K and freezing point of pure water is 273.15 K. The freezing point of a 5% solution (by mass) of glucose in water is

a) 271 K    

b) 273.15K

c) 269.07 K

d) 277.23 K

Answer : C

Question : 25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a titre value of 35ml. The molarity of barium hydroxide solution was

a) 0.07

b) 0.14

c) 0.28

d) 0.35

Answer : A